Titration Questions and Answers
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What is the concentration of methanol in grams per 100 mL of solution after standardizing a methyl alcohol solution using a titration with potassium permanganate, given that 100 mL of the aqueous m...
A 16.42 mL volume of .1327 M KMnO_4 solution is needed to titrate to completion a 25.00 mL solution of a FeSO_4. What is the molarity of the FeSO_4 solution? 5Fe^{2+} + MnO_4^- + 8H^+ to Mn^{2+} +...
What experimental method would you use to determine the amount of vitamin C in an 8 oz glass of orange juice, assuming that this amount of juice contains a day's supply of vitamin C? How much orang...
Calculate the permanganate activity in an aqueous 0.18 M KMnO_4 solution.
The blood alcohol (C_2H_5OH) level can be determined by titrating a sample of blood plasma with an acidic potassium dichromate solution, resulting in the production of Cr^3+(aq) and carbon dioxide....
How could you use a conductometric titration to determine the molarity of H2SO4 and Ba(OH)2, assuming you knew the concentration of one?
Sketch a photometric titration curve for the titration of Sn2+ with MnO4-. What color radiation should be used for this titration? Explain.
For the following substance, give at least one reason why it would be unacceptable as a primary standard for standardizing aqueous solutions of bases? Stearic acid, C_(17)H_(35)COOH, which is inso...
For the following substance, give at least one reason why it would be unacceptable as a primary standard for standardizing aqueous solutions of bases? Hydrocyanic acid, HCN
Please match the following responses below with the questions further below. A) KHC_8H_4O_4 (potassium hydrogen phthalate) B) Titrant C) Phenolphthalein D) Primary Standard E) Pump Dispenser...
The iron in a 6.675 g sample containing some Fe2O3 is reduced to Fe2+. The Fe2+ is titrated with 14.42 mL of 0.1467 M K2r2O7 in an acid solution. 6Fe2++Cr2O2-7+14H+ 6Fe3++2Cr3++7H2O( ) Find the mas...
Al in the presence of concentration HNO_3 becomes passive due to the formation of an Al_2O_3 layer. H_2SO_4 also is an oxidizing acid. Explain whether the concentration H_2SO_4 does or does not a...
A 20.0 mL solution containing 0.250 M Ni^{2+} ion was titrated with 0.0500 M EDTA while the system was buffered at pH=4.00. Determine the volume of EDTA needed to reach the equivalence point.
A possible method to determine the zinc content of an aqueous solution is by precipitation of Zn(OH)2. A solution containing an unknown amount of zinc was titrated using a 0.226 molar solution of N...
If 27.0 mL of 0.0200 M KMnO_4 were required to titrate a 0.425 g sample of K_3(Fe(C_2O_4)_3) . 3H_2O, what is the % purity of the complex?
You take an unknown solution and measure 1 mL of it into a flask. You dilute it with 25 mL of water and 10 mL of H2SO4. You titrate the solution with 19.80 mL of KMnO4. The (MnO4)- is reduced to (M...
You take an unknown solution and measure 1 mL of it into a flask.You dilute it with 25 mL of water and 10 mL of H2SO4. You titrate the solution with 19.80 mL of KMnO4. The (MnO4)- is reduced to (Mn...
In this experiment, 10.00 mL of the unknown solution to be analyzed is diluted to 100.0 mL. Then 10.00 mL of the dilute solution is titrated with a standardized permanganate solution. Why not skip...
The iron in a 6.675 g sample containing some Fe_2O_3 is reduced to Fe^{2+}.The Fe^{2+} is titrated with 14.53 mL of 0.2456 M K_2Cr_2O_7 in an acid solution. Find the percentage of Fe in the sample.
What is the molarity of oxalic acid in a solution if 34.56mL if 0.0123M potassium permanganate is needed to titrate 25.00mL of the unknown solution?
As a laboratory technician, you are presented with an aqueous sample that was collected from highway runoff during a rain storm. You are to quantitatively analyze for Pb, Zn and Cu in the aqueous s...
What is the purpose of the blank solution in the volumetric analysis method?
What are 3 reasons why pipets are the most precise glassware?
If a 100.0 mL solution containing Fe^{2+} ions is titrated with 15.2 mL of 0.135 M Cr_2O_7^{2-}, calculate the molar concentration of Fe^{2+} ions in the solution. Cr_2O_7^{2-}(aq)
If the pH is 8.0 at the equivalence point for the titration of a certain weak acid with sodium hydroxide, what indicator might you use?
If 29.0 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.829 g of precipitate, what is the molarity of silver ion in the original solution?
When the titration is performed, which sample, if any, will require the largest volume of the 0.01 M NaOH for neutralization? Three acid samples are prepared for titration by 0.01 M NaOH: 1. Sampl...
Why can't HCl and NaOH be used as primary standards?
A sample containing both HCl and HNO_3 had a density of 1.083 gram/mL. A 10.0 mL aliquot of this sample required 28.44 mL of 0.1163 M NaOH for titration. Another 10 mL aliquot of samples required 1...
What is the equivalence point pH for the titration of 100 mL of 0.155 M HCNO (K_a = 2.0 times 10^{-4}) with 100 mL of 0.155 M LiOH?
If you are given a standard KIO_3 solution with a concentration of 0.01 M, what is the volume of the standard KIO_3 solution needed to titrate 300 mg of ascorbic acid?
If a 25.00 mL sample of 0.0100 M KIO_3 is reacted with an excess of KI and it requires 32.04 mL of Na_2S_2O_3 solution to titrate the I_3^- ions formed, what is the molarity of the Na_2S_2O_3?
A 30.0 mL sample of a 0.200 M acetic acid solution is titrated with a 0.100 M NaOH solution. Calculate the pH after 10.0 mL of NaOH has been added.
What will be the color of an ammonia hydroxide solution when the indicator phenolphthalein is added?
Consider the titration of 80.0 mL of 0.150 M ethylamine with 0.100 M HCl. Calculate the pH after 40.0 mL of HCl has been added.
Calculate the molality of KMnO_4 solution needed to titrate 50.00 mL of a saturated solution of this oxalate salt. It should take 7.50 mL of KMnO_4 solution to titrate the saturated oxalate solution.
Suppose you add 2 mL of 1.0 M NaOH to 20 mL of 0.60 M HC2H3O2. Calculate the pH. (Ka for HC2H3O2 = 1.8 x 10-5)
Titration of an oxalate sample gave the following percentages: 15.53%, 15.55% and 15.56%. Calculate the average and the standard deviation.
A 10.0-mL sample of aqueous NaOCl is treated with excess KI in an acidic solution. The quantity of iodine that is liberated is such that 28.02 mL of 0.0250 M Na_2S_2O_3 solution must be added to ca...
A student performed the iodata analysis and found that it took 7.80 mL of 0.02 M Na_2S_2O_3 to titrate 4.00 mL of saturated copper iodate. Calculate the number of moles of iodate in 7.80 mL of 0.02...
Why is a solution of NaOH which was standardized yesterday unsuitable to be used as a standard solution today?
For the reaction: NiCl_2 (aq) + 2NaOH (aq) to Ni(OH)_2 (s) +2NaCl (aq). What is the molarity of 30.0 mL of NiCl_2 solution that reacts completely with 15.3 mL of a 0.330 M NaOH solution?
In the laboratory, you dissolve 12.6 g of barium hydroxide in a volumetric flask and add water to a total volume of 375 mL. What is the concentration of the hydroxide anion?
Methylene blue and diphenylbenzidine sulfonic acid are redox indicators that turn from colorless in the reduced state to blue(methylene blue) or violet (diphenylbenzidine sulfonic acid) in the oxid...
How many mL of a 1.20 M H_3PO_4 solution are required to titrate 85.5 mL of a 0.465 M LiOH solution? H_3PO_4(aq) + 3LiOH (aq) \to Li_3PO_4(aq) + 3H_2O(l)
What is the correct procedure when an indicator has not been added to the analyte? (a) Add the indicator as soon as possible. (b) Start over. (c) Try to observe the pH using a pH meter instead. (d)...
A 23.74-mL volume of 0.0981 M NaOH was used to titrate 25.0 mL of a weak monoprotic acid solution to the stoichiometric point. Determine the molar concentration of the weak acid solution. Express y...
Consider the titration of 50.0 mL of 0.125 M phosphorous acid, H_3PO_3, (K_{a1} = 3 \times 10^{-2}, K_{a2} = 1.62 \times 10^{-7}) with 0.250 M NaOH. The titration reaction occurring is: H_3PO_3 +...
Why can the calibration of a buret be omitted if the buret is used for both a standardization and an analysis with the same solution?
Does the endpoint coincide with the stoichiometric point? Briefly explain and suggest how the discrepancy may be corrected.
A 25.0 mL solution of 0.0460 M EDTA was added to a 49.0 mL sample containing an unknown concentration of V^{3+} . All V^{3+} present formed a complex, leaving excess EDTA in solution. This solution...
A 50 g Acetylsalicylic acid (C_9H_8O_4) tablet is titrated and it is found that it contained 42 g of acid. Determine the percentage purity of the tablet.
Ni^2+ can be analyzed by back titration using standard Zn^2+ at pH 5.5 with xylenol orange indicator. A solution containing 25.00 mL of Ni^2+ in dilute HCl is treated with 25.00 mL of 0.05283 M Na_...
A sample of calcium oxalate (CaC2O4) is dissolved in excess acid, followed by its titration with permanganate, according to this reaction. C2O42-(aq) + MnO4-(aq) arrow Mn2+(aq) + CO2(aq) + H2O(l) I...
If 34.24 mL of a 0.0185 M KMnO_4 solution were required to titrate the iron in a 0.989 g of unknown iron sample. Calculate the percent iron in the sample.
Why should a standardized NaOH solution be kept in a stoppered bottle with a rubber stopper?
Consider the titration of 50.00 mL of 0.100 M benzoic acid (Ka = 6.3 x 10-5) with 0.0500 M KOH. What volume of titrant (KOH) is required to reach a pH of 4.20?
Calculate the normality of an unknown acid if 21.8 mL is required to titrate a 25.0 mL sample of 1.02 N NaOH. a. 1.02 N b. 1.17 N c. 0.855 N d. 0.889 N e. There is insufficient information to answe...
A group of students performed a titration experiment. They took 25.00 mL of solution of phosphoric acid of unknown concentration, and then added drop wise the 0.125 M solution of sodium hydroxide.W...
Suppose it takes 27.1 mL of 0.100 M NaOH to titrate 5.00 mL of vinegar. Determine the mass percent of acetic acid in the vinegar. Assume that the vinegar density is 1.000g/mL.
A sample of a tin ore weighing 0.3550 g was dissolved in an acid solution and all the tin in the sample was changed to tin(II). In a titration, 7.90 mL of 0.0401 M KMnO_4 solution was required to o...
Calcium in blood or urine can be determined by precipitation as calcium oxalate, C a C 2 O 4 . The precipitate is dissolved in strong acid and titrated with potassium permanganate. The products of...
Give the reason for the following: Iodometric titrations are usually performed in neutral or mildly alkaline (pH 8) to weakly acid solution.
In a certain experiment, 20.00 ml of 0.800 M H C l were added to a 0.1022 gram sample of M C O 3 . The excess H C l required 5.64 ml of 0.1000M N a O H for neutralization. Calculate the mola...
The amount of ascorbic acid, C6H8O6, in orange juice was determined by oxidizing the ascorbic acid to dehydroascorbic acid, C6H6O6, with a known excess of I2, and back titrating the excess I2 with...
Which of the following correctly defines a standard solution? a) A solution which always has the same molecular geometry. b) A solution in which the concentration is precisely known. c) A solution...
Describe titration and its use in conjunction with molar stoichiometry to determine concentration.
What is titration?
Determine the molarity of a NaOH solution when each of the following amounts of acid neutralizes 25.0 mL of the NaOH solution. (a) 20.0 mL of 0.250 M HNO_3 (b) 5.00 mL of 0.500 M H_2SO_4 (c)...
A solution was prepared by dissolving 0.450 g of MgSO4 in 0.500 L of water. A 50.0 mL aliquot of this solution consumed 37.60 mL of EDTA solution in a titration. How many mg of CaCO3 will react wit...
Which of the following describes the process of titration? (a) When the acid has exactly neutralized a base or vice versa (b) To cause a separation from solution or suspension (c) The technique of...
A 20.00mL sample H3Y was titrated with 0.1000 M NaOH. The first equivalence point was reached after the addition of 14.98 mL of base. The second equivalence point was reached after the addition of...
A tablet of vitamin C was analyzed to determine whether it did in fact contain, as the manufacturer claimed, 1 g of the vitamin. One tablet was dissolved in water to form 100 mL of solution, and 10...
What is the molarity of a NaOH solution if 28.50 mL of it is needed to titrate a 0.7154 g sample of KHP?
The concentration of a solution sodium iodide ion will be determined by titrating 90 mL of it using potassium permanganate. After 60.0 mL of 0.250 M KMnO_4 is added the purple color of potassium pe...
A 3.00 L sample of urban air was bubbled through a solution containing 50.0 mL of 0.0116 M Ba(OH)_2, which caused the CO_2 in the sample to precipitate as BaCO_3. The excess base was back-titrated...
A 16.7 mL sample of vinegar, containing acetic acid, HC2H3O2, was titrated using 0.5168 M NaOH solution. The titration required 19.28 mL of the base. What was the molar concentration of acetic acid...
What mass of sodium oxalate, Na_2C_2O_4, is required for a titration where the equivalence point occurs at 30.00 mL of 0.0200 M KMnO_4 solution? Assuming that your synthesized compounds have 2.5 L...
A sample of an arsenic salt weighing 100.0 mg was dissolved, and the arsenic converted to arsenite, which required 10.98 mL of 0.01234 M permanganate solution for complete reaction. What is the pe...
You are performing an iodometric titration of ascorbic acid using a K I O 3 standard solution. Suppose that the amount of ascorbic acid in the sample you are about to titrate is 85 mg. Calculate...
A sample mixture weighing 38.8626 g containing only F e C l 3 and K C l required 126.22 mL of 5.6878 M A g N O 3 for complete titration of the chloride. How many parts per million (ppm) of po...
15.57 mL of 0.0259 M KMnO4 was required to oxidize a 1.441 g sample of Fe2+. What is the percentage of Fe2+ in the sample?
If 0.1154 g of sodium oxalate requires 28.97 mL KMnO4 solution to reach the end point, what is the molarity of the KMnO4 solution?
An 8.75-g sample of iron ore (mixture) is transformed to a solution of iron(II) sulfate, and this solution is titrated with 0.150 M K2Cr2O7 potassium dichromate. If it requires 67.8 mL of potassium...
If 9.51 mL of 0.106 M sodium hydroxide is required to titrate the acetylsalicylic acid in an aspirin tablet, how many milligrams of acetylsalicylic acid are in the tablet?
Distinguish between back titration and redox titration.
The point in a neutralization reaction where the number of moles of hydrogen ions is equal to the number of moles of hydroxide ions is called the _____. a. reference point b. equivalence point c...
How to do a titration. Write a procedure for how to find the concentration of an unknown monoprotic acid using a sample of 5 mL. Describe what equipment to use and how to set it up.
Which of the following statements is correct? (a) An internal standard is a known amount of a compound, similar to that analyte, that is added to the unknown sample. (b) To use an internal standa...
The phosphorus in a 4.258-gram sample of a plant food was converted to PO43- and precipitated as Ag3PO4 through the addition of 50 mL of 0.0820 M AgNO3. The excess AgNO3 was back-titrated with 4.86...
The volume of water added moving a half-drop of titrant from the tip of the burette to the analyte selection during the end of the titration may be ignored in your calculations. Why is this so?
You have the task of determining the concentration of a sample of hydrogen peroxide, H2O2, by titration with acidic potassium permanganate, KMnO4. Explain briefly how to perform the titration, how...
What volume of 0.240 M K_2S solution is required to completely react with 155 mL of 0.140 M Co(NO_3)_2?
Experiment on Titration of Acids and Bases Suppose some deionized water was left in the buret before it was filled with the oxalic acid solution you were using as a primary standard. When you perfo...
If an initial burette reading is 14.28 mL and the final burette reading is 51.09 mL, then the volume of the solution delivered is _____?
During the titration of an H C l O 4 solution with 0.1032 M N a O H , quantitative analysis student Al Cohol became distracted and overshot the end point. A fellow student, I.M. Smart, suggested...
An acid-base titration starts at a pH of 3.4 and reaches an endpoint of pH 8.5. Describe the type of sample and titrant being used in the titration
The current EPA standard for Cl- in drinking water sets a maximum concentration of 250 mg/L. Suppose a water sample is analyzed via precipitation titration using 0.0150 M AgNO3 to titrate the sampl...
A sample of 0.6805 g iron ore was dissolved in concentrated HCl. After reduction of all Fe^(3+) to Fe^(2+) with SnCl2, the solution needed 45.50 ml of 0.515 M K2Cr2O7 to reach the end point. What i...
If a hydrochloric acid solution was standardized with contaminated sodium carbonate, what would be the effect on the calculated mass percentage in an unknown sample and why?
A solution of baking soda NaHCO_3 prepared from 0.755 g dissolved in 100 mL of water was used as an antacid. 25.00 mL of 0.960 M HCl were used to digest the sample. The volume of 0.595 M NaOH use...
Determine the concentration of H_2O_2 \text{ using } KMnO_4. Titrant: Potassium Permanganate Solution
0.5073 g of impure K2S2O8 (molar mass 270.32 g/mol) was analyzed by treatment with excess standard Na2C2O4 by the following reaction: K2S2O8 + Na2C2O4 = Na2SO4 + K2SO4 + 2CO2 After reacting with 50...
Hydrogen peroxide (H2O2) can be purchased in drug stores for use as an antiseptic. A sample of such a solution weighing 1.000 g was acidified with H2SO4 and titrated with a 0.02000 M solution of KM...
Samples of a sodium carbonate solution of unknown concentration were titrated with a standardized hydrochloric acid solution using methyl orange as the indicator. The results of the titration of 25...
The Ksp of AgI is 8.3 10-17. You titrate 25.00 mL of 0.08900 M NaI with 0.05010 M AgNO3. Calculate pAg after the following volumes of AgNO3 are added: (a) at 36.20 mL (b) at Ve (c) at 47.50 mL
A 15.0 g vinegar is titrated with 85.40 mL of 0.150 M NaOH. How much acetic acid is in the vinegar? Commercial vinegar is sold as 3-5%. Can this sample be sold to the public? Explain the answers a...
A 0.020 M K M n O 4 solution was used to determine the percent iron in a sample containing iron(II according to the equation M n O 4 + 5 F e 2 + + 8 H + M n 2 + + 5 F e 3 + + 4 H 2 O . It t...
Match the statement with the type of titration: 1. strong acid-strong base 2. weak acid-strong base 3. strong acid-weak base it would apply to. Titration types can be used more than once or not at...
If a 20.0 mL aliquot of the unknown chloride solution is titrated against 0.105 M
The iron content in drinking water can be measured by titration with potassium permanganate. The reaction is represented by the equation: 5 F e 2 + ( a q ) + K M n O 4 ( a q ) + 8 H + ( a q ) 5 F...
When a sample of the aqueous layer with a volume of 10.93 mL is collected, it requires 18.19 mL of a titrant solution of S2O32- with a concentration of 0.01085 M to reach the endpoint. The reaction...
What are precautions to be taken when doing titrations?
At the beginning of a titration to standardize a NaOH solution, student A adjusted very carefully the initial burette volume to 0.00 mL, but he did not notice an important air bubble in the tip of...
A student analyzed powdered cultured buttermilk. A 2.270-gram sample of the powdered buttermilk required 37.18 mL of 1.183 x 10-2 M EDTA solution for titration of the Ca2+ ion. a. How many moles of...
What are 3 inherent sources of error that could occur during a titration lab?
A 30.0 mL sample of barium nitrate solution is titrated with a solution of copper (II) sulfate until no more precipitate forms. The precipitate is reclaimed by filtration, dried and weighed. If 275...
When dissolving a solid acidic sample with water, does it matter how much water we use to dissolve it? (Will it change the calculations of the titration?)
The initial volume of a hydrochloric acid solution is 98 mL with a concentration of 0.945 M HCl. An antacid tablet is added to the solution. Then a back titration is done with a 0.78 M NaOH solutio...
A person's blood alcohol (C2H5OH) level can be determined by titrating a sample of blood plasma with a potassium dichromate solution. The balanced equation is as follows. 16H+(aq) + 2Cr2O72-(aq) +...
Suppose that a student is determining the total base content of an antacid tablet by performing a back titration. He/she weighs out a 0.3012-gram portion of a tablet whose total weight is 1.5312 gr...
Can the pH of a titration be calculated without using a titration curve?
During a volumetric analysis of Cu2+, explain two possible problems that might ensue from adding the titrant too quickly.
A 0.405-gram sample of KHP is dissolved in 50 ml of water. The sample is then
An impatient chemistry student fails to thoroughly mix the standard solutions.
Calculating the determination of Iron (II). You have a 25 mL sample of iron (II) solution, 50 mL of distilled water and 12 mL of 2 M phosphoric acid and titrate using standardized permanganate solu...
The amount of I3-(aq) in a solution can be determined by titration with a solution containing a known concentration of S2O32-(aq) (thiosulfate ion). The determination is based on the net ionic equa...
1. A solution of iodine was standardized with ascorbic acid. A 0.1150 g sample of ascorbic acid required 28.37 mL of I_2 to reach a starch end point. Calculate the molarity of the iodine solution....
What is the gravimetric factor for phosphorous (P) in KH_2PO_4?
What should the crucible be placed on a wire mesh to cool?
What is the mass of KIO3 needed to titrate 300 mg of ascorbic acid?
When vitamin C (ascorbic acid, C6H8O6) reacts with iodine (I2) in solution, C6H8O6(aq) + I2(aq) \rightarrow C6H6O6(aq) + 2H^+(aq) + 2I^-(aq). What is the mass of KIO3 needed to titrate 300 mg of...
Use the data below to determine the Molarity of KMnO4 to THREE decimal places. (MM sodium oxalate = 134 g/mol). mass of sodium oxalate (g) : 0.091 initial buret reading (mL) : 0.09 final buret rea...
A titration is performed as follows: 8.367 mL of Fe2+ solution of unknown concentration is charged into a 100 mL beaker. 45 mL of deionized water is added. The solution is titrated with a 0.803 M C...
For the following reaction between Mohr's salt (iron as F e S O 4 ( N H 4 ) 2 S O 4 6 H 2 O ) and potassium dichromate (dichromate as K 2 C r 2 O 7 ) determine the volume (in milliliters) of a...
i really need help with these 4 questions :/, i dont understand them at all alt="idk chem.png" /> The amount of 13 (aq) in a solution can be determined by titration with a solution containing a kno...
I. A titration is the progressive addition of one reagent to another. II. A titration involves a chemical reaction between an acid and a base. III. The indicator endpoint shows that chemically equi...
A 25.00-mL aliquot of a standard calcium solution (M = 0.0068; 0.3412 grams of CaCO3 was added to a 500 mL flask) was titrated with a previously prepared EDTA solution. In the titration, 32.55 mL o...
To calculate carbonates in the water, explain why \frac{1}{2} CO_{3}^{2-} is taken?
A titration is performed as follows: *4.004 mL of Fe2+ solution of unknown concentration is charged into a 100 mL beaker *45 mL of deionized water is added *the solution is titrated with 0.695 M Ce...
25.00 mL of a sample solution of oxygen-based bleach was treated with H2SO4 and titrations with 0.125 M solution of KMnO4. 12.0 mL of the titrant was used. Calculate the number of moles of H2O2 pre...
Arsenic(III) oxide, As2O3, can be titrated with potassium bromate in aqueous solution to produce potassium bromide and arsenic acid, H3AsO4. A mixture contained arsenic(III) oxide and arsenic(V) ox...
How does the pH of a solution affect the reduction of manganese? In addition, how does the pH of the solution change the color of manganese?
I. A titration is the progressive addition of one reagent to another. II. A titration involves a chemical reaction between an acid and a base. III. The indicator endpoint shows that chemically eq...
A buffered solution containing calcium ions, Ca^{2+}, was titrated to the end point using 29.51 mL of 0.2211 M EDTA. How many moles of Ca^{2+} were present in the solution?
A standard K_2Cr_2O_7 solution was first prepared by dissolving 1.2275 grams of previously dried potassium dichromate with deionized water in a 250 mL volumetric flask and diluting to the mark with...
Which of the following must be clear when titration is carried out? (a) the concentration of all the reactants (b) the stoichiometric ratio of the reactants (c) both (a) and (b) (d) neither (a)...
Calculate the ppm of CaCO3 = mg CaCO3 / Liters H2O used. The titration of 25.00 mL took 19.290 mL of 3.765x 10-3 M EDTA solution to reach the endpoint.
Calculate the number of grams of CaCO3 present and convert to mg. The titration of 25.00 mL took 19.290 mL of 3.765x10-3 M EDTA solution to reach the endpoint.
The total hardness is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3 /kg H2O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO3 per lit...
The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, de...
The equivalence point is: a. The point at which the concentrations of base and acid are equal. b. The point at which the volumes of base and acid are equal. c. The point at which the concentration...
The iron content of iron ore can be determined by titration with a standard KMnO4 solution. The iron ore is dissolved in HCl, and all the iron is reduced to Fe^2+ ions. This solution is then titrat...
Ten drops of an indicator was added to a 10.00 mL sample of powdered drink mix. The sample was titrated with a sodium hydroxide solution that was determined to be 0.1421 M. The initial burette read...
Calculate the mass in grams of undiluted bleach that was in the sample of bleach titrated, based on the following conditions. A student diluted and titrated an unknown bleach exactly as described i...
Calculate the number of moles of ClO- in the sample titrated given the following conditions. A student diluted and titrated an unknown bleach exactly as described in the experimental procedure, exc...
Suppose a student diluted and titrated an unknown bleach exactly as described in the experimental procedure, except only a single titration was performed, which required 12.78 mL of 0.100 M Na2S2O3...
Formic acid (CH_2O_2) and is added to animal feed as a preservative, especially for silage to be stored through the winter because it inhibits fermentation and maintains the nutritional quality of...
Given the balanced chemical reaction equation and titration data below, calculate the molarity of the H3PO4 solution. H3PO4(aq) + 3NaOH(aq) arrow 3H2O(l) + Na3PO4(aq) Volume of acid solution (H3PO4...
If 0.135 g of CuCl2 is dissolved in 25.00 mL of water and titrated with 35.45 mL of Na2S2O3 solution (of unknown concentration) to reach the end point, what mass of copper atoms is present in the s...
100 mL of a 0.025 M Fe^{2+} are titrated with 0.025 M Tl^{3+} \space (Tl^{3+} + 2Fe^{2+} \to Tl^+ + 2Fe^{3+}).This titration is done as a potentiometric titration using Pt as indicator electrode. T...
If you require 11.8 ml of 0.0448 KMnO_4 solution to titrate the Na_2C_2O_4 solution, what is the mass of Na_2C_2O_4 present in the solution?
If it takes 35.0 mL of 0.250 M Fe2+ to titrate 100 mL of a solution containing Cr2O72-, what is the molar concentration of Cr2O72-?
Consider the following two reactions involving oxalic acid. 2MnO_4^- + 5H_2C_2O_4 + 6H^+ \rightarrow 2Mn^{2+} + 10CO_2 + 8H_2O H_2C_2O_4 + 2OH^- \rightarrow C_2O_4^{2-} + 2H_2O a) What volume of 0....
A 0.2250 g of sample of a mixture containing only of iron and ferric oxide (Fe_2O_3) was brought into solution and the iron was reduced to the divalent state and titrated with permanganate.
What volume, in milliliters, of 0.250 M K2Cr2O7 is required to completely react with 0.0200 L of a 0.250 M solution of Mohr's salt?
Determine the volume, in milliliters, of a 0.250 M solution of Mohr's salt ((NH4)2Fe(SO4)26H2O) needed to completely react with 0.0200 L of 0.25 M potassium dichromate (K2Cr2O7).
Compare Na2S2O3 and KMnO4 as titrants for redox titrations with respect to at least three factors.
How much 8080 octane gas and 9696 octane gas should be blended to make 1616 gallons of 9494 octane gas?
A 25.0 mL sample of H3PO4 is titrated with NaOH. If 29.2 mL of 0.738 M NaOH is needed to reach the endpoint, what is the concentration (M) of the H3PO4 solution?
A dilute solution is prepared by transferring 40 mL of a 0.3433 M stock solution and adding 710 mL of water. What is the molarity of the dilute?
If it took 320 mL of an HNO3 solution to neutralize 490 mL of a 2.4 M KOH solution, then what was the molarity of the HNO3 solution?
23.48 mL of a NaOH solution is needed to neutralize 0.5468 g of KHP. What is the concentration of the NaOH solution?
It requires 32.98 ml of sodium hydroxide to reaction with 44.65 ml of 0.2118 m sulfuric acid. What is the molarity of the sodium hydroxide solution?
How many grams of sucrose would you need to prepare 100 mL of a 24% sucrose solution?
How many gallons of 25% alcohol solution and 45% alcohol solution must be mixed to get 16 gallons of 30% alcohol solution?
A drop of NaOH is hanging from the buret tip before the titration of KHP. Once the student begins the titration that drop falls into the KHP solution. The calculated concentration for the standardi...
How can you calculate molar mass from the titration curve?
104g sample of impure was acidified and analysed using excess iodine ion. The reaction is . Then is titrated with 0.300M
A 0.500 g sample of impure CaO (a solid) is added to 50.0 mL of 0.100 M HCl. The excess HCl is titrated by 5.00 mL of 0.125 M NaOH. What is the percentage of CaO in the sample?
What else could the Volhard method be used in Chemistry for?
Why is it important to keep the NaOH solution (being used during titration) stoppered at all times when it is not in use? And why is it all right to use a wet flask for a titration experiment?
A 1.252 g sample containing iron is dissolved and converted to Fe2+ followed by addition of 25 mL of 0.01 M K2Cr2O7. The excess K2Cr2O7 required 6.85 mL of 0.015 M. Find the percentage Fe3O4 FW 231...
What is important about oxygen being formed during a titration?
What happens to the color of the FeCl_2 when the equivalence point is reached?
Why is it unwise to boil the oxalate solution in preparation for its titration with permanganate?
Predict the most likely redox reaction and use the spontaneity rule to predict whether the reaction will occur spontaneously: An aqueous solution of potassium permanganate was reacted with an acidi...
In Iodometry, I know that I- will be oxidized to I2 if the titration of Cu(II) is not done immediately, but what effect does it have to the molarity of S2O3^2-?
Why Fe(III) can be estimated in acidic medium by dichromate, not by permanganate?
Construct the data chart and the pH curve for the titration of 25 mL of 0.1 M CH3COOH with 0.1 M NaOH. Add the titrant 1 mL at a time and calculate the pH after each addition.
How do you calculate the concentration of vinegar?
A 0.750 g sample of an unknown solid is dissolved in 100 mL of water and acidified with 25 mL of 3 M H_2SO_4 then titrated with a 0.0200 M KMnO_4 solution. If the unknown solid requires 12.5 mL of...
What are the principles/techniques involved in double-indicator titration? especially in carbonate mixtures.
A 2.7 M solution of phosphoric acid (H_3PO_4) is to be reacted with a 7.5 M solution of sodium hydroxide to make sodium phosphate and water. How many litre of the H_3PO_4 solution will react with 0...
If a student used an iron scoopula, instead of a plastic one, to add the unknown metal to the HCl solution, will it affect the calculated molar mass of the unknown metal?
A 25.0 mL sample of drinking water suspected to contain lead (II) ions is treated with excess 0.800 M sodium chloride. A precipitate forms, which is filtered, dried, and weighed. 1.36 g of precipit...
Commercial aqueous hydrogen peroxide was diluted 150 times. 25 cm^3 of the sample solution was titrated with 0.020 M KMnO_4 and 26.3 cm^3 was required to reach the endpoint. Calculate the molar con...
Fe3+ is added to excess Ag+ prior to titration with KSCN. When all the excess Ag+ has reacted, the red complex of Fe(SCN)2+ forms. This red complex is visible when the (SCN-) is about 2 x 10^-4 M....
A solution of potassium permanganate (KMnO_4) was standardized by titrating with 0.1908 g of Na_2C_2O_4 dissolved in 50 cm^3 of acidified water. The endpoint was reached after 24.50 cm^3 of the sol...
A 0.1818 g sample of sodium oxalate required 28.12 ml of a potassium permanganate solution to reach the endpoint (assume the reaction was carried out in excess acid). A 5.000 g sample of tin (II) s...
How many liters of CO_2 and water vapor are produced by burning .3 liters of C_2H_2 (Acetylene) with .75 liters of O_2? The balanced equation is: 2C_2H_2 + 5O_2 \rightarrow 2 H_2O + 4CO_2
How do we know that the moles of ascorbic acid originally present in the juice is equal to the moles of I_2 that we added when the color change occurred?
A 2.304 gram sample containing an unknown amount of arsenic trichloride and the rest inerts was dissolved into a NaHCO_3 and HCl aqueous solution. To this solution was added 1.500 grams of KI and 5...
A 10.0 mL volume of Ultra Bleach is diluted in a volumetric flask. A 25.0 ml sample of this solution is analyzed according to the procedure in this experiment. Given that 33.75 mL of 0.135 M Na_2S_...
A solution of I_2 was standardized with ascorbic acid. Using a 0.1000 g sample of pure ascorbic acid, 25.32 mL of I_2 were required to reach the starch end point. A. What is the molarity of the iod...
In a titration of 0.5 M HCl and an unknown concentration NaOH, 25.0 ml of NaOH was required to completely neutralize 25.0 ml of HCl. What is the concentration of the NaOH?
Why are standard solutions of reductants less often used for titrations than solutions of oxidants?
A 5.0 mL aqueous sample containing hydrogen peroxide as diluted to 25 mL and analyzed by titration with permanganate. 2MnO4- + 5H2O + 6H+ arrow 5O2 + 2Mn^2+ + 8H2O The sample required 42.8 mL of 0....
A 2.00 mL sample of an aqueous solution of hydrogen peroxide, H2O2(aq), is treated with an excess of Kl(aq). The liberated I2 requires 12.40 mL of 0.1025 M Na2S2O3 for its titration. Is the H2O2 up...
How many mL of 0.175 M H3PO4 are needed to neutralize 15.00 mL of 0.33 M NaOH?
If a chemist titrates 300.0 mL of H_2SO_4 with a 3.0 M solution of NaOH and requires only 3.4 mL of the base to reach the endpoint, what is the concentration of the sulfuric acid?
In the chlorine titration of a solution prepared by the dissolution of 0.2110 g of commercial hypochlorite was spent 19.50 ML of sodium thiosulphate solution 0.1002 mol / L. Calculate the percentag...
If 26.223 mL of potassium permanganate solution is required to titrate 1.041 g of ferrous ammonium sulfate hexahydrate, FeSO4(NH4)2So46H2O, calculate the molarity of the KMnO4 solution. MnO4- + 8H+...
Write a reduction half-reaction for the reaction between iron (II) sulfate and potassium permanganate in a sulfuric acid solution.
1. Why are standard KMnO4 solutions seldom used for the titrations of solutions containing HCl? 2. Why are standard solutions of reductants less often for titrations than standard solutions of oxid...
How many mL of 0.0500 M phosphoric acid (H3PO4) are needed to titrate completely 50.0 mL of 0.150 M barium hydroxide (Ba(OH)2)) solution?
Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide can be titrated against a solution of potassium permang...
A 10.0-mL sample of vinegar, which is an aqueous solution of acetic acid, CH3COOH, requires 16.5 mL of a 0.500 M NaOH solution to reach the endpoint in a titration (where the moles of acid are equa...
How many milliliters of .50 M NaOH solution are required to titrate 40.0 mL of a 0.10 M H_2SO_4 solution to an end joint?
A 10.0 ml sample of vinegar which is an aqueous solution of acetic acid, requires 16.5 ml of a 0.500 M NaOH solution to reach the endpoint in a titration (where the moles of acid are equal to the m...
A potassium permanganate solution containing 1.58 g of KMnO_4 per liter is added into 5 ml of an acidified iron (||) sulfate solution. Decolorizing of KMnO_4 solution ceases when 10 ml of the solut...
What will happen if ammonium chloride solution is used to standardize potassium tetraoxomanganate (VII) solution instead of ammonium iron (II) sulphate?
The chloride ion concentration in a solution may be determined by the precipitation of silver chloride. Ag+(aq) + Cl-(aq) ? AgCl(s) A student finds that 17.08 mL of 0.6000 M silver nitrate is nee...
A 2.53 * 10-2 L sample of a solution of Cu + requires 3.22 * 10-2 L of 0.134 M KMnO4 solution to reach the equivalence point. The products of the reaction are Cu^2+ and Mn^2+. What is the concentra...
1.Calculate the molar mass of sodium oxalate Na2C2O4. 2.A 0.516 g portion of a sample that contains sodium oxalate is dissolved in water to which sulfuric acid has been added. The end point of the...
Calculate the value for total water hardness (amount of Ca + Mg). This will be reported in terms of CaCO3 in mg/L. The moles of (Ca+Mg) is equal to the moles of EDTA used in the titration. Multiply...
1. Very briefly, explain the difference between a buffered solution and an unbuffered solution in terms of changes to the pH when small amounts of 3 M HCl solution is added. 2. Use the periodic ta...
Given the following data, determine the % by mass of oxalate (C_2O_4^2-) in a sample of an iron oxalate complex with the general formula K_z[Fe_x(C_2O_4)_y].wH_2O. The reaction between oxalate and...
Back titration is required for the determination of acetylsalicylic acid in aspirin as shown in the following chemical equations. CH_3COO-C_6H_4-COOH + 2NaOH ? CH_3COONa + HO-C_6H_4-COONa NaOH +...
How many moles of Na2S2O3 react with each mole of KIO3 used in the standardization. Show all work.
Write a balanced oxidation-reduction equation for the reaction of oxalic acid with potassium permanganate in an acidic solution then, from the indicated molar ratio, calculate how many moles of MnO...
Explain why it is acceptable to add water to the titration flask while vinegar is being titrated. Explain why adding water does not change the molarity (moles / liter) of the vinegar.
1. A. To determine the concentration of a sodium thiosulfate solution as in this experiment, a student pipetted 25.0 mL of 0.0100 M potassium iodate (KIO3) solution into a 125 mL Erlenmeyer flask....
1. Given the following balanced equation for the titration of oxalate ion with permanganate ion: 5C2O4 (2-) + 2MnO4 (-) +16 H (+) ---> 10CO2 +8H2O +2Mn A student titrated .184 g green K3[Fe(C2O4)...
A geothermal heat pump operating at steady state with R-22 as the working fluid is shown schematically below. The heat pump uses 55 F water from the geothermal wells as the thermal source. Operatin...
Why is the titration curve nearly flat at the end of the titration, well past the equivalence point?
Oxalic acid (H_2C_2O_4) is present in many plants and vegetables. Balance the following equation in acidic solution: MnO_4^- + H_2C_2O_4 --> Mn^2+ + CO_2 If a 1.08 gram sample of impure H_2C_2O_...
The vanadic ion V3+ forms green salts and is a good reducing agent. In a neutral aqueous solution, it is transformed into the colorless vanadic hydroxide ion, V(OH)4 + . The salt, vanadic sulfate V...
A 20 mL sample of 0.100 M U?+4 in a 1 M sulfuric acid solution is titrated with 0.100 M Ce4+, also in 1 M sulfuric acid. a) What volume of Ce4+ is required to reach the equivalence point? b) Wh...
In one analysis, a 1.00 g sample containing sodium oxalate was first dissolved in acid to form oxalic acid. Then, the solution was titrated with a standard 0.100 M potassium permanganate, KMnO_4, s...
a. The amount of I3-(aq) in a solution can be determined by titration with a solution containing a known concentration of S_2O_32-(aq) (thiosulfate ion). The determination is based on the net ionic...
How many grams of potassium permanganate are needed to completely oxidize 2g of chlorotoluene? Show a correctly balanced oxidation-reduction equation for this reaction. Also, determine the oxidatio...
Potassium permanganate. KMnO_4. is a powerful oxidizing agent The products of a given redox reaction with the permanganate ion depend on the reaction conditions used. In basic solution, the followi...
The amount of l_3^-(aq) in a solution can be determined by titraction with a solution containing a known concentration of S_2O_3^2-(aq) (thlosulfate Ion). The determination Is based on the net IonI...
I did a gravimetric analysis experiment with 8-hydroxyquinoline to find the amount of aluminum I had in an unknown powder. I've gotten three weights for the precipitate that's supposed to allow me...
In a series of titration experiments, why is it that you always work with the smallest sample first? Explain.
An impure sample of sodium carbonate, Na_2CO_3, is titrated with 0.150 M HCl according to the reaction below. 2 HCl (aq) + Na_2CO_3(aq) --->CO_2(g) + H_2O(l) + 2 NaCl (aq) What is the percent of Na...
For the baking soda titration, write the chemical reaction that occurs when the solution is boiled just before the endpoint. Why is doing this helpful in the titration?
Calculate the redox potential for the reduction of TiO2+ to Ti2+ Using appropriate information gleaned from the Handbook of Chemistry and Physics, or the internet, draw a latimer diagram for titani...
1. Dichromate and ferrous ions react in acidic solution to form chromic and ferric ions, respectively. If 1, 285 grams of iron (II) bisulfate dissolved in sulfuric acid solution requires 35.78 mL...
1. Write the balanced net ionic equation for the reaction between MnO_4^- ion and Fe^2+ ion in acid solution. 2. How many motes of Fe^2+ ion can he oxidized by 1.3 times 10^-2 moles MnO_4^- ion in...
A flask contains 1.53 g of acid and a few drops of phenolphthalein indicator dissolved in water. A buret contains 0.270 M NaOH. Assuming the acid is monoprotic, what is its molar mass?
1. Calculate the percent error in the calculated molar mass of the unknown acid that would be caused by titrating one drop past the end point. Assume that the mass of the acid is 1.000 g and that 3...
Orange juice is not the only juice containing vitamin C. Grapefruit juice, the pink-red juice in the figure below, contains 93.90 mg of vitamin C per cup. How many mL of 0.0150 M iodine solution w...
When a pink aqueous solution of potassium permanganate, faintly acidified with dilute sulfuric acid was treated with 10% aq. hydrogen peroxide, the reaction took place with the evolution of gas bub...
A sample of a new cleaning product, "Joe's Famous Bleach Cleaner," with a mass of 48.0 g , was diluted with an acetic acid solution containing excess I?. A small amount of starch indicator solution...
Question 6 (2 points) Suppose a student failed to dry (remove the water from) the KHP before using it to standardize the NaOH solution. What effect would this have on the calculated molarity of the...
An NaOH solution of unknown concentration was standardized using php. A. Calculate the number of moles of php used? B. How many moles of NaOH were used? C. what is the molarity of the NaOH solut...
1. Potassium permanganate is another strong oxidizing substance similar to potassium dichromate. An acidic solution of purple permanganate ions can be reduced to colorless Mn^2+ ions in the presenc...
Consider a different titration for this exercise. Potassium permanganate (KMnO_4)
What is the concentration of the unknown H_2C_2O_4 solution? Express your answer using four significant figures.
as the acid solution is titrated, the pink color forms where the drops first enter the solution but disappears as the solution is mixed. Explain why this happens
Why should you not condition the buret with water and then fill it with NaOH? What type of error would result on your calculated NaOh molarity?
Why is it important to know the exact concentration of a base used in the titration?
A titration is carried out to determine the concentration of the acid in an old bottle of aqueous HCl whose label has become unreadable. What is the HCl concentration if 65.2 mL of 0.300 M NaOH is...
Robin, a student in your class, started the titration but forgot to add the phenolphthalein indicator to the "vinegar" solution at the start. Upon adding three drops of indicator a while later, the...
EXPERIMENT 10: Oxidation-Reduction Titration: Determination of the concentration of an unknown solution. How would your calculation of the molarity of KMnO been affected, if at all: (Clearly explain
A student followed the procedure of this experiment to determine the percent NaOCl in a commercial bleaching solution that was found in the basement of an abandoned house. The student diluted 50.00...
Use the following experimental titration data to calculate the unknown concentration and pH of the acid. Observation: The initial solution of acetic acid is clear and colourless. A few drops of ph...
Rank the following titrations in order of increasing pH at the halfway point to equivalence (1 = lowest pH and 5 = highest pH). 1) Rank the following titrations in order of increasing pH at the hal...
Commercial hydrogen peroxide contains small amounts of organic compounds that are added to stabilize it. If these compounds react with permanganate, how would this affect your results?
Titration Acetic acid (HC_2H_3O_2) is an important ingredient of vinegar. A sample of 50.0 mL of a commercial vinegar is titrated against a 1.00 M NaOH solution. What is the concentration (in M) of...
A 24.0-mL solution of 0.100 M CH_3 COOH is titrated with a 0.200 M KOH solution. Calculate the PH after the following additions of the KOH solution: a. 10.0 mL b. 12.0 mL c. 15.0 mL
Why is it important to do multiple trials of a titration instead of only one trial?
What is the purpose of a titration curve?
What is spectrophotometric titration?
What is coulometric titration used for?
Why is back titration used to determine calcium carbonate?
What are the types of titration?
What is Karl Fischer titration?
Is a titration a neutralization reaction?
What is indirect titration?
What is an iodometric titration?
What unknown quantity can be calculated after a titration?
What is volumetric titration?
What is the purpose of the trial titration?
What is analyte in titration?
What happens in a redox titration?
What is photometric titration?
What is EDTA titration?
How do you perform back titration?
How do you know when a titration is finished?
What happens at the equivalence point during a titration?
What happens at the endpoint of a titration?
Why is DST used in Karl Fischer titration?
How do you determine the endpoint in a potentiometric titration?
What is the principle of Karl Fischer titration?
How many types of titration are there in chemistry?
Is titration qualitative or quantitative?
How is titration used in the food industry?
When is back titration used?
How do you find pKa1 and pKa2 from a titration curve?
How do you eliminate dissolved carbon dioxide in titration?
How does Karl Fischer titration work?
How do you calculate percentage purity in titration?
What is the importance of adding an indicator during titration?
Why is starch added near the endpoint in iodometric titration?
How does EDTA titration work?
Why do we use back titration?
Why is KI used in iodometric titration?
Why is eriochrome black T used in complexometric titration?
When should back titration be used instead of direct titration?
What is direct titration?
What is redox titration used for?
How is titration used in the pharmaceutical industry?
How can one improve titration technique?
What industries use titration?
What does titration determine?
Why is starch used as an indicator in iodometric titration?
What is a titrant in a titration?
What is standardization in titration?
How to calculate a back titration
How to calculate moles of NaOH used in titration
What is conductometric titration in chemistry?
How do you do a titration equation?
How do you calculate concentration in titration?
How do you plot titration curve?
What is argentometric titration?
How do you calculate molarity from a titration?
What is a titration curve?
Why is titration important in chemistry?
How do you read a titration curve?
What is an acid-base titration?
How does titration work?
What is titration used for?
What is the purpose of titration?
How do you find the equivalence point on a titration curve?
What is titration in chemistry?
An HOOCCOOH (aq) solution was tittered with 0.485 mol/L KOH (aq) to the second endpoint, using phenolphthalein. Using the following evidence, calculate the concentration of the HOOCCOOH (aq).
The following plot shows two pH titration curves, each representing the titration of 50.0 mL of 0.100 M acid with 0.100 M NaOH: a) Which of the two curves represents the titration of a strong acid...
Calculate the molar mass and the acid dissociation constant for aspirin if 0.500g of sample is dissolved in 250 mL. The 50.0 mL of the solution is titrated with 0.01225 M NaOH and the endpoint is d...
Consider the titration of 40.0 mL of 0.250 M HF with 0.200 M NaOH. How many milliliters of the base are required to reach the equivalence point? Calculate the pH at each of the following points. A...
Which method for determining a halide is better? Is there any significant difference between volumetric, gravimetric and potentiometric?
What is the endpoint volume (Ve) of the titration of 50.00 mL of 0.025 00 M MES with 0.100 0 M NaOH, where MES is a weak acid with pKa = 6.27? Additionally, describe the behavior at each of the fou...
If 25 mL of 0.055 M HCl is added to 35 mL of distilled H2O, what is the final pH? A) 0.20 B) 1.26 C) 1.41 D) 1.64
A student performed the standardization of sodium hydroxide by titrating a 3.5 grams sample of potassium hydrogen phthalate (KHP) with a given sodium hydroxide solution. The initial burette reading...
What is the pH before the addition of NaOH in the titration of 20.00 mL of 0.500 M acetic acid with 0.500 M NaOH, given that Ka=1.8*10^-5?
What is the pH after the addition of 8.00 mL of NaOH in the titration of 20.00 mL of 0.500 M acetic acid with 0.500 M NaOH, given that Ka=1.8*10^-5?
What is the pH after the addition of 20.00 mL of NaOH in the titration of 20.00 mL of 0.500 M acetic acid with 0.500 M NaOH, given that Ka=1.8*10^-5?
Can you calculate the percentage by mass of Mg(OH)2 in a mixture containing both Mg(OH)2 and Al(OH)3, if 0.2527 grams of the mixture was reacted with 50.00 mL of 0.225 mol L^{-1} HCl(aq) and then t...
What is the pH of a solution obtained by titrating 50 mL of 0.50 M formic acid with 0.50 M sodium hydroxide? Determine the pH value before any titrant is added, after adding 15.0 mL of titrant, whe...
How many moles of sodium carbonate are present in a mixture of sodium bicarbonate, sodium carbonate, and a neutral component if 6.0 mL of 0.100 M HCl were used to titrate 0.200 g of this mixture wi...
a. Prepare a theoretical titration curve for titration of 25.0 mL of 0.1037 M formic acid (HCOOH; pK_a = 3.75) solution (diluted to 100 mL volume with deionized water) by 0.0964 M solution of KOH ....
How much sulfamic acid (H2NSO3H) should be used to standardize an approximately 0.200 M NaOH solution if the titration requires 40.00 mL of NaOH solution?
In an acid-base titration experiment, 26.00 mL of the base is required to neutralize a 20 mL sample of an unknown acid solution. The pH of the solution when exactly 13.00 mL of the base is added is...
How much additional HCl needs to be added to a solution containing 100 mL of 7.00*10^-2 M HCl and 100 mL of 5.00*10^-2 M NaOH to create a 1.00 L solution with a pH of 2.70, assuming that the final...
We mixed 25 mL of 0.1 M lactic acid (CH3CH(OH)COOH) with 0.1 M sodium hydroxide (NaOH) and plotted the data on a graph called a titration curve is shown below. What is the approximate pKa value? Ad...
What are the pCu2+ values at the following points during the titration of 50.00 mL of 0.001 00M Cu2+ with 0.001 00M ETA at pH 11.00 in a solution with a fixed NH3 concentration of 0.100 M: a) 0 mL,...
The pOH of an aqueous solution of HNO3 is 2.00. Calculate the (H3O^+), (OH^-), and pH for this solution. What are the steps involved in your calculation, and what are your final answers?
Using the general pKa values for ionizable groups from any source, draw titration curves for glutamic acid with NaOH and histidine with NaOH.
What would the pH curve look like during the titration of a 0.150 M solution of a weak acid, HA (with a Ka of 5.4 10^-6), using 0.150 M KOH? Sketch the pH curve and indicate the pH values at the...
If the amount of HCL is increased in the beaker of a titration, would it take more NaOH to reach the end point?
How can you calculate the average number of moles of OH- used in titrations and the average number of moles of HC4H4O6- in a 25.0-mL sample of a solution containing bitartrate, which is a weak acid...
A 20.0-mL sample of a 0.200 M HBr solution is titrated with a 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of the base have been added. A. 16 mL B. 19.8 mL C....
Create a titration curve by titrating 100.00 mL of 0.100 M sodium leucinate (in the L^- form of leucine) with 1.00 M HCl, and determine the pH of the resulting solution at the following volumes of...
A corrosion technologist pipetted a 100.00 mL hard water sample and titrated it with 37.64 mL of 0.01 M EDTA solution for a total hardness endpoint and 29.32 mL of 0.01 M EDTA solution for a calciu...
Calculate the volume of a 1.170 M nitric acid (HNO_3) solution required to titrate 20 mL of a 1.850 M sodium hydroxide solution (NaOH). Record your answer in milliliters to one decimal point.
0.346 grams of KHP are placed in an Erlenmeyer flask, followed by the addition of some water and a drop of phenolphthalein. The buret is then filled with an aqueous solution of NaOH of unknown conc...
75 mL of 0.50 M solution of NaOH is titrated with a 0.50 M solution of HCl. Calculate the initial pH.
If 37.5 mL of an aqueous solution of HCl requires 22.7 mL of 0.72 M NaOH to reach the endpoint, what is the molarity of the HCl solution?
Sample of solid Ca(OH)2 is allowed to stand in contact with water at 30 degrees C for a long time, until the solution contains as much dissolved Ca(OH)2 as it can hold. A 100 mL sample of this stro...
Define the following terms as they relate to titrations: (a) aliquot; (b) analyte; (c) titrant; and (d) scout titration (not associated with Boy Scouts).
You have 5 mL of vinegar in a flask and 2 drops of phenolphthalein indicator. You titrate exactly 36.9 mL of 0.1 mol/L NaOH from a burette directly into the flask which gives you a pale pink color....
What would be the impact on the calculated molarity if the liberated iodine is not titrated immediately during the standardization process of Na2S2O3 solution? Explain your answer.
What volume of 0.23 M Benzoic acid (K_a=6.3\times 10^-5) is needed to reach equivalence with 32.92 ml of 0.23 M NaOH?
Lead(II) nitrate and ammonium iodide react to form lead(II) iodide and ammonium nitrate according to the reaction. Pb(NO_3)_2(aq)+2NH_4I(aq)\to PbI_2(s)+2NH_4NO_3(aq) What volume of a 0.170 M NH_4I...
Potassium hydrogen phthalate is commonly used as a standard in acid-base titrations. Consider a 25mL sample of unknown KHP concentration mixed with 3 drops of phenolphthalein and titrated with 0.01...
True or false? The chemical reaction involved in an acid-base titration is a neutralization reaction.
Consider the titration of 50.0 mL of 1.0 M glycine hydrochloride [[(H_3NCH_2COOH)Cl], with 1.0 M NaOH. For ^(+)H_3NCH_2COOH, K_a for the carboxylic acid group is 4.3\times 10^(-3) and K_b for the a...
a) What is an acid-base indicator? b) Define the equivalence (stoichiometric) point and the endpoint of a titration. Why should you choose an indicator so that the two points coincide? c) Do the...
Determine the normality of the titrant for the following: 0.9757 grams KHC8H4O4, 46.26 mL KOH.
Consider the following four titrations: i. 100.0 mL of 0.10 M HCl titrated with 0.10 M NaOH ii. 100.0 mL of 0.10 M NaOH titrated with 0.10 M HCl iii. 100.0 mL of 0.10 M CH_3NH_2 titrated with 0....
Calculate the volume of a 0.500M NaOH solution needed to neutralize (titrate to the endpoint): A) 10.0 mL 0.300M HCl B) 10.0 mL 0.200M H_2SO_4 C) 4.16 g KHP (MM 204 g/mol)
The following information relates to the actual question further below: "Assuming that you performed the titrations described above using 100.00 mL samples of zinc nitrate, what volumes of 0.200 M...
What is the molar concentration of NaOH if a 0.920 grams sample of potassium hydrogen phthalate (KHC8H4O4) is dissolved in water and titrated to the equivalence point using 26.45 ml of NaOH? KHC8H4...
Calculate the pH for each of the following cases in the titration of 25.0 mL of 0.210 M pyridine, C5H5N(aq) with 0.210 M HBr(aq). Given Kb = 1.7 * 10^9. a) After the addition of 25.0 mL of HBr. b)...
Suppose that the lab prep staff incorrectly recorded the masses of KHP. You are told they used 0.50 g of KHP to standardize the NaOH solution; however, they actually used 0.10 g KHP in the standard...
If the bubble in the tip of the buret is not removed prior to performing the HCl titration, will the reported concentration of the HCl be greater than, less than, or equal to the true concentration...
Why it is not always necessary to refill the buret after every titration? Why it is not necessary to dry the Erlenmeyer flask after rinsing it out between successive trials? Explain.
A flask contains 0.383 g of acid and a few drops of phenolphthalein indicator dissolved in water. The buret contains 0.260 M NaOH. What volume of base is needed to reach the endpoint of the titrati...
A 0.200 g sample of a triprotic acid (molar mass = 165.0 g/mol) is dissolved in a 50.00 mL aqueous solution and titrated with 0.0500 M NaOH. After 10.50 mL of the base was added, the pH was observe...
Phenolphthalein turns pink in solutions that are roughly 1.0 times 10^{-5} M in hydroxide ions. The only source of hydroxide ion is your Ca(OH)_2. Let's assume the amount of water left behind in th...
A given 40 mL sample of a crushed Vitamin C tablet was dissolved in 40 mL of H2SO4 and 20 mL of water. Two grams of KI and 40 mL of 0.00653 M KIO3 solution was added, and the mixture was titrated t...
How can one use the principles of stoichiometry when preparing food in the kitchen? What are some examples of how stoichiometry is used to manufacture products found at home?
In a titration experiment, 25.0 mL of sodium hydroxide, NaOH, with a concentration of 0.204 mol/L was transferred via pipette into a conical flask. Sulfuric acid, H2SO4, of unknown concentration wa...
What is the difference between a strong acid-base titration curve and a weak acid-strong base titration curve?
Twenty vitamin C tablets (total mass = 6.3287 g) were powdered and 0.3231 g were dissolved in dilute sulphuric acid. This solution was then titrated with 0.0992 M ammonium cerium (IV) sulfate and 2...
Consider the titration of a generic weak acid HA with a strong base that gives the following titration curve: On the curve indicate the points that correspond to the following. a. the equivalence p...
An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and...
Consider the following pH curves for 100.0 mL of two different acids with the same intital concentration each titrated by 0.10 M NaOH: a. Which plot represents a pH curve of a weak acid, and which...
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