The CN^ concentration of 10.0 mL of a plating solution was determined by titration with...
Question:
The CN{eq}^- {/eq} concentration of 10.0 mL of a plating solution was determined by titration with electrogenerated hydrogen ion to a methyl orange end point. A color change occurred after 4 min and 11 s with a current of 55.6 mA. Calculate the number of grams of NaCN per liter solution.
Sodium Cyanide:
When sodium cyanide is dissolved in water, it becomes soluble. The sodium cyanide is present in white solid. The chemical formula which represents the sodium cyanide is NaCN.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerGiven Data:
- Current = 55.6 mA
- time = 4 min. 11 s
The electrochemical equivalent of NaCN is calculated as shown below:
{eq}\begin{align*} {\rm{Z}...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Formula for Mass: Definition & Examples
from
Chapter 28 / Lesson 42
63K
What is mass? Learn the mass definition and how to find the mass of an object using the mass formula. See common mass characteristics and properties.
Related to this Question
- The of a titration occurs when the indicator changes color, and the point at which an acid has completely reacted with or been neutralized by the base is known as the. a. endpoint; equivalence point b. equivalence point; endpoint c. endpoint; neutral poin
- A solution causes a yellow color with thymol blue, an orange color with methyl orange, a red color with methyl red, and a yellow color with bromthymol blue. The pH must lie between _____ and ______. The estimate pH is _______
- The pale pink color of the titration solution at the end point will fade to colorless after several minutes when exposed to the atmosphere. Account for this color change.
- In volumetric analysis, the point at which the indicator changes color is called: a. the neutralization point b. the equivalence point c. the endpoint d. a titration
- 2CrO4^2- (aq, yellow) + 2H3O^+ (aq) <---> Cr2O7^2- (aq, orange) + 3H2O( a) Describe the color change the student should observe after adding excess NaOH to the solution to the equilibrium mixture. b)
- A suitable indicator for the titration of 0.1 M NaHS with 0.1 M HCl would be A. methyl violet B. methyl orange C. phenolphthalein D. thymolphthalein
- An acid solution is titrated to the pink phenolphthalein endpoint by a base solution. As time goes by, the pink color disappears and the solution becomes colorless again. This takes about 30 seconds or so and definitely is not due to the solutions mixing
- 1. Colour of original K2Cr2O7 solution: orange Colour after the addition of NaOH: Yellow Colour after the addition of HCl: Orange Direction in which equilibrium is shifted by the addition of: NaOH:
- Cu^{2+} (aq) have a molar absorptivity of 12.7 M^{-1} cm^{-1} at 645 nm. If a solution of Cu^{2+} of unknown concentration has an absorbance of 0.418 measured in a 1.00 cm path length cell at 645 nm, what is the concentration of Cu^{2+}?
- The concentration of manganese in steel can be determined spectrophotometrically by dissolving the steel in acid and oxidizing Mn to MnO_4?. The resulting solution is purple and the absorbance at 525
- I took fresh orange juice and added 40.0 ml to a flask then added 1.0ml of a starch indicator solution. I added 0.015 M of iodine solution to a 50 ml burette. After 5.67 ml had been dispensed, it changed from orange to dark orange. The volume of the flask
- The magnesium electrode was dipped into a 1.00 M solution of MgSO4 and the cadmium electrode was dipped into a solution of unknown Cd2+ concentration. The potential of the cell was measured to be 1.54
- The point at which the indicator in the reactant solution changes color is the {Blank} of the titration. \\ A. end point B. equivalence point C. reaction point D. standard point
- Given a stock solution of yellow #5 with a concenGiven a stock solution of yellow #5 with a concentration of 2.9 x 10-4 M, calculate the concentration of yellow #5 in the 4 prepared solutions (A thru
- One method for determining the concentration of hydrogen peroxide in solution is through a redox titration with potassium permanganate under acidic conditions. In this procedure, the hydrogen peroxide reduces the pink permanganate ion. a. What is the oxi
- In an excess of NH_3(aq), Cu^2+ ion forms a deep blue complexion, Cu(NH_3)_4^2+, which has a formation constant K_f = 5.6 times 10^11. Calculate the concentration of Cu^2+ in a solution prepared by adding 4.5 times 10^-3 mol of CuSO_4 to 0.480 L of 0.35 M
- When most Fe^3+ salts are dissolved in dilute nitric acid, the solution is often yellow to orange-yellow in color. Why could you not visually detect these colors in Fe(NO3)3 stock solution?
- Metals bond with halogens to form colorless metal halides. During an experiment, bromine water was added to a solution of potassium iodide. A record of the experiment is shown. Reactants color: Br2 = light orange solution, KI = colorless solution Color of
- Given a stock solution of a food dye having a concentration of 1.0 times 10^{-5} and an absorbance of 0.700. If a new solution is made by diluting exactly 10.0 mL of the solution with exactly 15.4 mL of distilled water, what should the absorbance of the n
- H_2S(aq) can be determined by the coulometric titration technique via the generation of I_2. H_2S + I_2 \rightarrow S(s) + 2H^+ + 2I^- To a 50.00 mL sample, we added 4g of KI. Electrolysis required 812 secs at 52.6 mA. What is the concentration of H_2S in
- A solution causes a yellow color with thymol blue, an orange color with methyl orange, a red color with methyl red, and a yellow color with bromthymol blue. The pH must lie between ......... and .....
- A solution of a weak acid was tested with the indicators used in this experiment. The colors observed were as follows: methyl violet thymol blue methyl yellow violet yellow yellow congo red bromcresol green orange-red green What is the approxima
- 1. An unknown solution gave a strong yellow flame test. The solution gave no reaction with ammonium carbonate, ammonium phosphate, or ammonium sulfate. The halide test produced a yellow-orange color i
- Given a stock solution of a food dye having a concentration of 1.0 x 10^(-5) M and an absorbance of 0.700. If a new solution is made by diluting exactly 10.0 mL of the solution with exactly 46.4mL of distilled water, what should the absorbance of the new
- 1. A solution of a weak acid was tested with the indicators used in this experiment. The color observed were as follows: 2. A solution of
- Suppose 2.5 mg of hydrogen chloride gas is dissolved in 2.00 L of water. If the solution is tested with the orange IV indicator, what is the resulting color?
- The absorbance values A_t & A_0 recorded in the experiment 'Rate Law Determination of the Crystal Violet Reaction' are used in the place of the concentration values of which species?
- The concentration of manganese in steel can be determined spectrophotometrically by dissolving the steel in acid and oxidizing M n to M n O 4 . The resulting solution is purple and the absorbance at 525 nm can be monitored. A standard solution contai
- A test solution is prepared by pipetting 2.0 mL of an original sample into a 250 mL volumetric flask and then diluting to the mark. The concentration of iron in the test solution is determined (from a
- A spectrophotometric study of copper(II) ions in aqueous solution was conducted. The absorbance of a series of solutions of known concentrations of copper(II) ions was measured at 645nm, and a plot of absorbance (y-axis) vs. concentration (x-axis) was con
- Parts A.6 and B.2. For the standardization of the NaOH solution in Part A.6, the endpoint was consistently reproduced to a faint pink color. However, the endpoint for the titration of the acid solutio
- In a spectrophotometric experiment, 84.9% of the incident light is absorbed by the solution under investigation. If the solution is of concentration 0.069 mol dm^-3, and the path length of the cell is 12.5 mm, what is the molar absorption coefficient of t
- A concentration cell is constructed of two hydrogen electrodes. The pressure of H_2 is 1.00 atm in each hydrogen electrode. One of the electrodes is immersed in a solution with [H^+] = 1.0 M and the other in a solution with 0.62 M NH_3. What will be the v
- Given a stock solution of a food dye having a concentration of 1.0 x 10^(-5) M and an absorbance of 0.700. If a new solution is made by diluting exactly 10.0 mL of the solution with exactly 44.4 mL of distilled water, what should the absorbance of the new
- Given a stock solution of a food dye having a concentration of 1.0 x 10^(-5) M and an absorbance of 0.700. If a new solution is made by diluting exactly 10.0 mL of the solution with exactly 47.9 mL of distilled water, what should the absorbance of the new
- A stock solution of a food dye has a concentration of 1.0 x 10^-5 M and an absorbance of 0.700. If a new solution is made by diluting exactly 10.0 mL of the solution with exactly 20.5 mL of distilled water, what will the absorbance of the new ...
- 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 Fe2+ ions. This solution is then titrated with KMnO4 solution, producing Fe3+ and Mn2+ ions in
- When a good indicator has been chosen, the pH at which the solution changes color is very close to the................... point of the titration.
- A dilute aqueous solution of PtCl4 is a pale yellow to colorless, but a concentrated solution is a deep red. What explanation can you give for this behavior?
- In part 4 of this experiment, you are asked to prepare a solution in which the concentration of a weak acid is equal to the concentration of its conjugate base. To produce the base, you titrate a port
- A concentration cell can be prepared using a half-cell of Ag(s) electrode in a 1.5 M solution of Ag+(aq) and a half-cell of Ag(s) electrode in a 0.10 M solution of Ag+. What is the cell potential of this concentration cell?
- 3. A student, following the procedure in this experiment, studied the response of red food dye to visible light and analyzed a stock solution of red food dye of unknown concentration. A series of dilu
- A solution of an Fe^2+ complex with an unknown concentration has an absorbance value 0.467. For the absorbance analysis, the iron(II) solution was placed in a cuvette with a path length (b) of 1.0 cm.
- The protein apotransferrin binds two Fe(III) ions for cell transport. Consider when a 3.00 mL solution of apotransferrin is titrated with 108 microliters of a 1.03 M Fe(III) solution. The initially colorless solution turns red, and the color change can be
- Consider a hydrogen electrode in HBr solution at 25 degree C operating at 1.45 bar. Estimate the change in the electrode potential when the solution is changed from 5.0 mmol/L to 25.0 mmol/L.
- A substance has an extinction coefficient of 5 times 10^5 L cm^{-1} mol^{-1}. A concentrated solution of this substance has an absorbance too high to measure. You dilute 1 ml of this solution to 25 ml with distilled water; the measured absorbance is 0.2.
- A substance has an extinction coefficient of 3 times 10^5 L cm^{-1} mol^{-1}. A concentrated solution of this substance has an absorbance too high to measure. You dilute 1 mL of this solution to 25 mL with distilled water; the measured absorbance is 0.3.
- 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 titrated with a KMnO4 solution, producing Fe^3+ and Mn^2+ ions i
- Given the measured cell potential, E_cell, is -0.3521 V at 25 degrees C in the following cell, calculate the H^+ concentration H^+(s)|H_2(g, 0.797 atm)|H^+(aq, ? M)||Cd^2+(aq, 1.00 M)|Cd(s) The balanc
- Fe^{3+} (yellow) + SCN (colorless) leftrightarrow [FeSCN]^{2+}(dark red) If Fe^{3+} is added to the solution: (a) The solution turns darker red (b) The solution becomes more yellow (c) No changes in color occur (d) The solution becomes colorless
- 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 reading was 1.16 mL. When the first permanent color change occ
- A concentration cell consisting of two hydrogen electrodes (PH_2 = 1 atm), where the cathode is a standard hydrogen electrode and the anode solution has an unknown pH, has a cell voltage of 0.179 V. W
- An unknown solution containing yellow 5 dye displays an absorbance reading of 0.628. The molar extinction coefficient for yellow 5 dye is 27,300 L/mol.cm. What is the concentration of yellow 5 in the unknown? (Include units in your calculation.)
- A galvanic cell Mn(s)|Mn^{2+}(aq) || Ni^{2+}(aq)|Ni(s) is constructed using a completely immersed Mn electrode that weighs 33.7 g and a Ni electrode immersed in 539 mL of 1.00 M Ni^{2+}(aq) solution. A steady current of 0.0650 A is drawn from the cell as
- A student places a zinc electrode in a 0.80 M Zn2+(aq) solution which is connected by an electrolyte to a 1.30 M Ag+(aq) solution containing a silver electrode. (Note that the solution concentrations
- A student adds a bromine solution to a test tube containing the isomer of C_3H_6 . After shaking the sample and exposing it to UV light, the student observes that the color of the bromine solution changes from orange to clear. what was the final produc
- The logarithm of the molar absorptivity of phenol in aqueous solution is 3.812 at 211 nm. Calculate the range of phenol concentrations that can be used if the absorbance is to be greater than 0.150 and less than 1.500 with a 1.25-cm cell.
- a) For a mixture of your own choosing, how do you choose an appropriate indicator for a titration? b) Why it is important to use such a small quantity of indicator in a titration? c) What is the difference between the end point and equivalence point?
- Ten drops of water are added to two small test tubes and to each is added one drop of iodine. The solution turns from a lighter yellow to a darker orange. To one of the test tubes some powdered magnesium is added and mixed well and centrifuged.
- A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (P(H2) = 1 atm) immersed in a solution of unknown H+. If the cell potential is 0.191 V, what is the pH of the unknown solution at 298
- Consider a solution of an indicator with an acid dissociated constant of 1.42 times 10^{-5} and molar absorptivity of the indicator species at 430 nm and 570 nm. Draw the final relationship between the absorbance values were calculated above at various in
- When setting up their experiment, a student discovered that the solution in their flask turned bright pink upon adding 2 drops of the indicator, even before beginning the titration. What do you suspec
- In the example equilibrium system, a drop of methyl orange indicator was added. For this indicator, the solution will be red in high concentrations of HO+, and the solution will turn yellow in low con
- You have a protein solution with unknown concentration. Its extinction coefficient at 280 nm is 23,000 M-1cm-1. You measure the absorption at 280 nm in a 1 cm path-length cuvette and get 0.3. What is
- Clinical chemistry The concentration of Na^+ ions in red blood cells (10.0 mM) and in the surrounding plasma (142.0 mM) are quite different. (a) Calculate the electrochemical potential (emf) acros
- In spectroscopy experiments, the solution used to calibrate the spectrometer is known as the(blank.) A mixed dye solution contains an unknown amount of fluorescein dye and 5.0 * 10-6 M Blue #1 dye, b
- A calibration curve constructed from absorbance values of solutions containing a known concentration of permanganate ions has the following best-fit line: y = (3.62 x 10^3 L/mol) x, where y is the absorbance of the solution at 525 nm and x is the concentr
- Potassium permanganate, KMnO4, is a salt that dissolves in water to give an intense purple color. It has a molar absorptivity of 2.33 x 104 L/mol.cm measured at 535 nm. If you wanted to make up a solution that had an absorbance of 0.100 at this wavelength
- Methyl red solution is usually at 0.02 w/w\%. Calculate how you will prepare this solution if you start with 0.01g of methyl red and make up a solution in 100 mL using 60:40 ethanol to water solvent. Outline each step and your final concentration with uni
- A water sample was analyzed by ion chromatography to determine the concentration of Mg^{2+} and gave a peak area of 0.064 mS-min. Then 5.0 mL of water sample was spiked with 1.00 mL of 20.00 ppm Mg^{2+} and diluted to the mark with deionized water in a 10
- 1. A solution in which no more solid can be dissoved is referred to as (Blank)? 2. In such a solution, the concentration of solute is called the (Blank) when reported in g/L and the (Blank) when reported in mol/L.
- If a red light is passed through a dilute solution of chlorophyll solution, the spectrophotometer will detect what amount of transmittance of this light? a. 100% b. 50-75% c. less than 25% d. none
- A photometer with a linear response to radiation gave a reading of 595 mV with a bank in the light path and 139 mV when the blank was replaced by an absorbing solution. Calculate: a. The percent transmittance and absorbance of the absorbing solution. b. T
- A standard solution has an absorbance of 0.237. An unknown solution has an absorbance of 0.141. Is the concentration of the unknown higher, lower, or the same as the concentration of the standard? a. Higher. b. Same. c. Lower.
- The B_4 O_5 (OH)_4^(2-) ion, present in 5.0 mL of a saturated Na_2 B_4 O_5 (OH)_4 solution at a measured temperature, is titrated to the bromocresol green endpoint with 5.28 mL of 0.182 M HCI. Express
- A certain indicator, HIn, has Ka = 1.0 x 10-5. HIn has color 1 and In- has color 2. Which is true in a solution of pH = 7.00? a) It is colorless. b) It has color 2. c) It has color 1. d) It has color 1 + color 2.
- A 2.50 times 10^{-4} M solution of a dye has an absorbance of 0.680 when measured in a 1.00 cm cell at 625 nm. Calculate the % Transmittance of the solution. Will the % Transmittance increase or decrease, if the concentration of the dye is increased?
- The student takes a 2.00mL aliquot of the bleach solution and adds 1.00g of potassium iodide and 20.0mL of water. After buffering the solution, he then titrates the solution with 0.1153 M sodium thiosulfate solution and reaches the equivalence point after
- The solid KIO3 is diluted shy of the 100mL mark in the volumetric flask. Does this technique error result in a reported molar concentration of KIO3 being too high or too low?
- An 8.00 g sample of an iron ore was dissolved in an acid solution and the iron converted to the +2 oxidation state. The resulting solution took 75.0 mL of 0.200 M KMnO_4 solution to titrate to a light pink color.
- At around 660 nm a 0.033 M solution of Ni(NO_3)_2. 6H_2O gave an absorbance of 0.225. The absorbance of an "unknown" solution of Ni(NO_3)_2. 6H_2O gave an absorbance of 0.61. What is the concentration of Ni(NO_3)_2. 6H_2O in the "unknown"? (Assume Beer's
- A photometer with a linear response to radiation gave a reading of 690 mV with a blank in the light path and 169 mV when the blank was replaced by an absorbing solution. Calculate: A) the transmittance and absorbance of the absorbing solution. B) the expe
- A chemist prepares a solution of mercury(II) iodide, HgI2, by measuring out 0.0139 g of mercury(II) iodide into a 400 mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's mercury(II) iodid
- Introduction to Chromatography: Quantification of copper in solution - the standardized solution of NaOH is used: o Will the solution coming off of the ion exchange column and collected in a beaker or flask be acidic, basic, or neutral?
- If it is unnecessary to add an indicator to KMnO4 titration because of its intense deep purple color, will the end point of the titration coincide with the stoichiometric point? Explain.
- If phenolphthalein is used as an indicator for titrating Ca(OH)2 with titrant HCl instead of methyl orange, which is the recommended indicatory, would the reported solubility product for calcium hydroxide be too high, too low, or unaffected? Explain.
- Consider the concentration of the final solution made in two volumetric flasks. In flask A, the liquid was filled to a level above the mark. In flask B, the liquid was filled to a level below the mark
- When placed in a 1% glucose solution, a red blood cell will: a. not change b. undergo hemolysis c. undergo crenation
- When placed in a 5% glucose solution, a red blood cell will: a. not change b. undergo hemolysis c. undergo crenation
Explore our homework questions and answers library
Browse
by subject