In a titration experiment, 25.0 mL of sodium hydroxide, NaOH, with a concentration of 0.204 mol/L...
Question:
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 was added by burette until the NaOH was neutralized. 15.35 mL of the solution of sulfuric acid was needed for neutralization.
i. Name a suitable pH indicator that was used in this investigation.
ii. Calculate the concentration of the sulfuric acid. Give your answer to three significant figures.
Titration Reactions:
A titration reaction is an analytical technique used by chemists to determine the concentration of an unknown solution. This technique is performed by slowly adding a solution of known concentration to a solution of unknown concentration. The solution of known concentration is known as the titrant while the solution of unknown concentration is the analyte solution.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerpH Indicator:
The neutralization reaction between sodium hydroxide and sulfuric acid is a reaction between a strong base and a strong acid. The...
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
Titrations with Weak Acids or Weak Bases
from
Chapter 11 / Lesson 10
20K
Learn about titrations of weak acids and strong bases, strong acids and weak bases, and weak acids and weak bases. Explore types of titration curves and the pH.
Related to this Question
- In a titration experiment, 15.0 mL of 0.146 M H_2SO_4 is titrated and neutralized by 13.1 mL of a NaOH solution. What is the concentration (molarity) of the NaOH solution?
- 25 mL of a sulfuric acid solution was standardized by titrating it with 0.2500 M NaOH. 30.52 mL of NaOH was required. Calculate the molarity of the sulfuric acid.
- 25 ml of sodium hydroxide solution of an unknown concentration is added into a flask and a few drops of phenolphthalein are added to it. A 3 M sulfuric acid is added into a burette which is set over the flask containing the sodium hydroxide solution. The
- Titration reveals that 11.6 mL of 3.0 M sulfuric acid are required to neutralize the sodium hydroxide in 25.00 ml of NaOH solution. What is the molarity of the NaOH solution ? Using this equation : H
- 25 ml of sodium hydroxide solution of unknown concentration is added into a flask and a few drops of phenolphthalein are added to it. A 3 M sulfuric acid is added into a burette which is set over the flask containing the sodium hydroxide solution. The col
- If the titration of a 10.00 mL sample of sulfuric acid requires 28.15 mL of 0.100 M sodium hydroxide, what is the molarity of the acid?
- If it takes 27.5 mL of 0.768 M NaOH to titrate 16.7 mL of sulfuric acid. What is the concentration of sulfuric acid?
- In a volumetric titration experiment, 22.45 mL of 0.1 molL-1 sodium hydroxide was required to neutralise 10.00 mL of nitric acid. Determine the exact concentration of the nitric acid.
- If a 0.3502 g sample of pure KHP (molar mass = 204.2 g/mol) is titrated to a phenolphthalein endpoint with 16.24 mL of a NaOH solution, what is the concentration of the NaOH solution?
- For the titration of sulfuric acid (H_2SO_4) with sodium hydroxide (NaOH), how many moles of sodium hydroxide would be required to react with
- A 25.00 ml sample of HNO_3 is titrated with 0.2453 M NaOH. The titration requires 32.47 ml of NaOH solution to neutralize the HNO_3. What is the molarity of the H_2SO_4?
- 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)
- In a titration, 25.0 cm3 of 0.100 mol/dm3 sodium hydroxide solution is exactly neutralized by a dilute solution of hydrochloric acid. Calculate the concentration of the hydrochloric acid so
- An aqueous solution of sodium hydroxide (NaOH) was standardized by titrating it against a 0.4923 g sample of KHP. The moles of KHP is 0.002411. The initial reading taken from the buret containing the NaOH was 0.52 mL and the final volume reading was 32.8
- 20.0 cm^3 of sulfuric acid, concentration 0.30 mol/dm^3, was added to 40 cm^3 of sodium hydroxide, concentration 0.20 mol/dm^3. 2NaOH + H_2SO_4 \to Na_2SO_4 + 2H_2O (i) How many moles of H_2SO_4 were added? (ii) How many moles of NaOH were used? (iii) Wh
- An aqueous solution of sodium hydroxide is standardized by titration with a 0.110 M solution of nitric acid. If 14.1 mL of the base are required to neutralize 29.0 mL of the acid, what is the molarity of the sodium hydroxide solution?
- The molarity of NaOH for the trial is 0.5402 mol/L. Initial Volume of Acid: 0.02 mL Final Volume of Acid: 15.24 mL Used volume of Acid:15.22mL Initial Volume of Base: 0.04 mL Final Volume of Base: 24.42 mL Used volume of base:24.38mL What are th
- The molarity of NaOH for the trial is 0.5402 mol/L. Initial Volume of Acid: 15.24 mL Final Volume of Acid: 30.32 mL Used volume of acid: 15.08mL Initial Volume of Base: 1.30 mL Final Volume of Base: 25.22 mL Used volume of Base:23.92mL What are the
- A 0.50 M solution of H2SO4 is titrated with 500 ml of a 0.30 M solution of NaOH. What volume of H2SO4 was present?
- If it takes 59.62 mL of 0.3234 M HCl to titrate an unknown concentration of NaOH at the equivalence point, what is the mass of NaOH present in the sample?
- A NaOH solution of unknown concentration was standardized with potassium hydrogen phthalate, a monoprotic acid with chemical formula HC5H4O4K (204.22 g/mole). A total of 0.5038 g of KHP was obtained and titrated with the NaOH solution. 19.35 mL of the Na
- A student dissolves dicarboxylic acid(relative molecular mass of 118) in water and made up the solution to 250 cm3 in a volumetric flask. In a titration, a 25.0 cm3 sample of the acid solution needed 21.60 cm3 of 0.109 mol dm-3 sodium hydroxide solution
- How many mL of sodium hydroxide are necessary to neutralize 51.0 mL of 0.106 mol/L sulfuric acid, if the concentration of the base is concentration is 0.033 mol/L?
- In a titration of a sample of HCl(aq) with 0.113 M NaOH(aq), it took 51.2 mL of the base to reach the endpoint of the titration. Calculate the number of moles of the acid being neutralized.
- What is the molarity concentration of a 60.0 mL sample of hydrochloric acid solution that is neutralized by 50.0 mL of a 3.00 M sodium hydroxide (NaOH) solution as represented by HCl + NaOH NaCl + H2O?
- The titration of 10.00 mL of an HNO3 solution of unknown concentration requires 12.54 mL of 0.100 M NaOH solution to reach the equivalence point. What is the concentration of the unknown HNO3 solution?
- In a titration of NaOH and HCl, if you rinse the pipette used for the NaOH solution aliquot, how would this affect the final estimate of HCl concentration? (More, less or unchanged, why?)
- In a titration experiment, 20.00 mL of potassium hydroxide solution required 19.95 mL of 0.0875 mol/L phosphoric acid standard solution for complete neutralization. What is the mass of potassium hydroxide in the 20.00 mL sample solution?
- How to calculate concentration of NaOH in titration
- 100 mL of a 0.1 M solution of NaOH is neutralized to pH 7 with H2SO4. How many grams of H2SO4 are required to achieve this neutralization?
- 0.58 g of an impure sample of NaOH was dissolved in water and titrated against a 0.3 M H_2SO_4 solution. The average titre was 22.5 cm^3. Find the % purity of the NaOH.
- Consider the reaction of sulfuric acid, H2SO4, with sodium hydroxide, NaOH. H2SO4 (aq) + 2NaOH (aq) 2H2O (l) + Na2SO4 (aq) Suppose a beaker contains 34.9 mL of 0.164 M H2SO4. How many ml of 0.335 M NaOH must be added to react completely with sulfuric aci
- Titration of a 24.0 mL solution of H_2SO_4 requires 22.4 mL of 0.12 M Al(OH)_3. What is the moalarity of the H_2SO_4 solution? 3H_2SO_4 (aq) + 2Al(OH)_3 (aq) to Al_2(SO_4)_3 (aq) + 6H_2O (I)
- If 30.0ml of an H2SO4 solution is neutralized by 60.0ml of a 1.0M NaOH solution, what is the molarity of the H2SO4?
- Consider the reaction of sulfuric acid, H2SO4, with sodium hydroxide, NaOH. H2SO4(aq)+2NaOH(aq)=2H2O(l)+Na2SO4(aq) Suppose a beaker contains 34.9mL of 0.164M H2SO4. How many ml of 0.335M NaOH must be added to react completely with sulfuric acid?
- 20.0 cm^3 of sulfuric acid, concentration 0.30 mol/dm^3, was added to 40 cm^3 of sodium hydroxide,
- 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. This means the solution has reached neutralization. Calcu
- What is the concentration of an HNO3 acid solution, if during titration with NaOH, 44.10 mL of the acid requires 73.80 mL of 0.3600 M NaOH to reach the equivalence point ?
- A 0.409 g sample of KHC 8H 4O 4 (molar mass =204.44g/mol) requires 23.5 ml of a NaOH solution to reach the phenolphthalein endpoint. Calculate the molar concentration of the NaOH solution.
- How many milliliters of a 10.6 M NaOH solution are required to prepare a 0.715 L solution of NaOH with a concentration of 0.550 M?
- To determine the molarity of a solution of oxalic acid, 25.00 ml is titrated with a sodium hydroxide standard solution with a concentration of 0.05061 M. The titrated endpoint is 32.56 ml of sodium hydroxide solution (endpoint = when the reaction is over)
- In a titration experiment, 20.4 ml of 0.883M HCOOH neutralizes 19.3 ml of Ba(OH)_{2} . What is the concentration of the Ba(OH)_{2} solution?
- A student begins a titration experiment by filling her first buret with unknown acid to the 1.05 mL level. She fills her second buret with base, NaOH, and records an initial volume of 0.20 mL. At the end of the titration experiment and after the pale pink
- Consider the titration of 25.00 mL of a 0.0705 M weak diprotic acid solution with 0.100 M NaOH. a) How many mL of 0.100 M NaOH are required to reach the first equivalence point? b) How many total mL of 0.100 M NaOH are required to reach the second equiva
- What are the normality and molarity of a sulfuric acid solution if 30 ml of it are required to completely neutralize 24 ml of 0.02 N NaOH?
- A KCC student titrated 100 ml of a NaOH solution using 55.00 ml of 0.1000 M H2SO4 solution. What is the concentration of NaOH solution? H2SO4 + 2NaOH right arrow Na2SO4 + 2H2O a) 5.500 times 10^{-3} M b) 1.100 times 10^{-2} M c) 5.500 times 10^{-2} M d)
- Consider the titration below: HCl + NaOH \to NaCl + H_2O If it takes 15.70 mL of 0.117 M of NaOH to reach the equivalence point, determine the molar concentration of HCl. The volume of HCl is 5.00 mL.
- A wine is diluted 1:5 with pure water, and then 15.00 mL of the diluted wine is mixed with ~20 mL of pure water and 3 drops of phenolphthalein. Then, it is titrated to completion, which requires 23.86 mL of 0.0784 M NaOH solution. The density of the origi
- It took 23 \ mL of 0.120 \ M \ NaOH solution to reach the end-point titrating 10 \ mL of a weak acid. Assuming a 1:1 stoichiometry, what is the concentration of the acid (3 s.f.)? a. 3.62 \ M b. 0.276 \ M c. 0.120 \ M d. 0.0522 \ M
- An analytical chemist is titrating 197.5 mL of a 1.100 M solution of butanoic acid (HC_3H_7CO_2) with a 0.9300 M solution of NaOH. The
- How to calculate moles of NaOH used in titration
- What volume of 0.1 molL-1 NaOH would be needed to neutralize 20 mL of the following solutions a) 0.1 mol L-1 HCl b) 0.1 mol L-1 H2SO4?
- A 10.0 mL sample of 0.250M HCl (aq) is titrated to the endpoint with a 14.0 mL sample of NaOH (aq). A balanced equation to represent the neutralization reaction is shown below. Calculate the molarity of the NaOH (aq).
- You are presented with 25 mL of an aqueous solution of HCl in a conical flask. A titration performed using a 0.4 M aqueous NaOH solution and a pH meter reveals that the titer volume required to neutralize the acid solution is 10 mL. For each of the follow
- How many ml of a 3 mol/l naoh solution are required to make 100 ml of a 0.2 mol/l NAOH solution?
- What volume of a 5.5 M sodium hydroxide (NaOH) solution is needed to prepare 300 ml of 1.2 M NaOH solution?
- How to calculate volume of NaOH required for titration
- Calculate the volume in mL of 7.3 M NaOH solution needed to neutralize 2.3 g sulfuric acid. Report answer in units of mL.
- Calculate the new molarity if 335 \ mL of water is added to a 58.3 \ mL of 2.07 \ M sodium hydroxide, NaOH solution.
- How many milliliters of 0.200M NaOH are needed to react with 15mL of 0.400M H2SO4 solution? 2NaOH+H2SO4 yields Na2SO4+2H2O
- The following data was obtained from the titration of 1.000 \ g of unknown weak acid dissolved in 25.00 \ mL of water and then titrated with 0.200 \ M NaOH |mL of 0.200 M NaOH |pH |0.00 |2.491 |2.00 |2.959 |5.00 |3.343 |10.00 |3.700 |20.00 |4.168 |30.00|
- What is the molarity of a solution prepared by dissolving 2.24 grams of NaOH in enough deionized water to obtain 500.0 mL of solution ? The molar mass of NaOH is 40.0 g.
- A 100ml sample of natural water was titrated with NaOH ,the titration required 13.13ml of 0.1451M NaOH solution to reach a light pink phenolphthalein end point. Calculate the number of millimoles of NaOH required for the titration.
- You are presented with 25 mL of an aqueous solution of HCl in a conical flask. A titration performed using a 0.4 M aqueous NaOH solution and a pH meter reveals that the titer volume required to neutralize the acid solution is 10 mL. a) Calculate the pH of
- A standard solution of 0.25 M H2SO4 is used to determine the concentration of a 220 mL LiOH solution. The addition of 143 mL of H2SO4 resulted in complete neutralization. What is the concentration of the LiOH solution?
- The mass of KHP is 0.5096 and the moles of KHP is 0.002495. What is the volume of NaOH used (in mL) and molarity of NaOH?
- How many mL of 2.00 M NaOH are needed to react with 15 mL of 0.400 M H2SO4 solution? 2NaOH + H2SO4 rightarrow Na2SO4 + 2H2O
- 100.0 mL of 0.100 M acetic acid is placed in a flask and is titrated with 0.100 M sodium hydroxide. K_a for acetic acid is 1.7 X 10^-5. Calculate the pH in the flask at the following points in the titration. (a) after 100.0 mL of NaOH is added
- 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.
- How much 0.500 M NaOH is needed to neutralize 100 mL of 1.00 M H_2SO_4? 1) 50.0 mL 2) 100 mL 3) 200 mL 4) 400 mL 5) 800 mL
- A 750 mL solution (d = 1.05 g/mL) is made by dissolving 83.0 g of NaOH in water. a. What is the molarity of NaOH in this solution? b. What is the mole fraction of NaOH in this solution?
- If an unknown concentration of 25.00 mL HCl consumes 20 mL of 0.123 M NaOH to reach the endpoint, calculate the concentration of the HCl solution (Show calculation).
- If you titrate 100 mL of an unknown strong acid solution with 0.1 M NaOH, will the pH ever reach a value of 13? Explain.
- Twenty-five (25) mL of a nitric acid solution of unknown concentration is added to a flask. A few drops of phenolphtalein are added to the nitric acid in the flask. A 0.115 M sodium hydroxide solution is added to a buret which is set up over the flask con
- A 0.1 mole% caustic soda (NaOH) solution is to be concentrated in a continuous evaporator. The solution enters the unit at 25^oC at a rate of 150 mol /min and is concentrated to 5 \ mole% at 50^oC. Hot dry air at 200 ^oC and 1.1 bar absolute is bubbled th
- A 10.0 mL sample of 3.00 M KOH(aq) is transferred to a 250.0 ml volumetric flask and diluted to the mark. It was found that 38.5 ml of this diluted solution was needed to react the stoichiometric point in a titration of 10.0 mL of a phosphoric acid, H3PO4
- Calculate the amount in moles of solute in 2.50 L of sodium hydroxide NaOH solution with 1.00 mol/L concentration.
- How many mL of a 4.50 M solution of NaOH is needed to prepare 550. mL of a 2.50 M NaOH solution?
- We observe that 40.5 mL of an H2SO4 solution reacts with 0.265 grams of Na2CO3. What is the molarity of the H2SO4 solution? H2SO4 + Na2CO3 arrow Na2SO4 + H2O + CO2
- Calculate the molarity of the acetic acid in vinegar, if a 500ml sample of the vinegar requires 43.50 ml of 0.105 M NaOH to reach a phenolphthalein endpoint in a titration.
- A student prepares a 250.0 mL solution of NaOH from an impure source of solid sodium hydroxide. After testing, it is determined that the solution, in fact, has a concentration of 0.893 M rather than the 1.000 M goal concentration.
- A student prepared a 6.48 M solution of sodium sulfate, Na2SO4 (molar mass = 142 g/mol) in a 1-L volumetric flask. How many milliliters of solution does she need to take from the flask in order to get 0.147 moles of sodium sulfate? ______________ mL Na2SO
- Consider the titration of 30.00 mL of 0.500 M CH_3COOH with 0.500 M NaOH. Assume that the solution will reach its equivalence point when 30.00 mL of NaOH is added. a) Calculate the pH after 15.00 mL of NaOH is added (halfway to equivalence point). b) Cal
- If it takes 75.00 mL of a 2.50 M HCl solution to neutralize 55.00 mL of base NaOH of unknown concentration. i.) Calculate the concentration of an unknown basic solution. ii.) Based on the molarity of the base, calculated above, what is the pH of the solut
- An aqueous solution of nitric acid is standardized by titration with a 0.129 M solution of barium hydroxide. If 22.7 mL of the base are required to neutralize 10.3 mL of the acid, what is the molarity of the nitric acid solution?
- What volume of a 0.1600 M NaOH solution is required to titrate 24.00 mL of a 0.1150 M HCl solution?
- You are presented with 20 mL of an aqueous HCl solution in a conical flask. By titration (using a pH meter), 8 mL of 0.4 M NaOH is needed to neutralize the solution. (a) What pH reading will the neutralized solution give? (b) What is the molar concentrati
- Below is a sectional view of a burette containing NaOH solution. The numbers on the burette are in mL. Read the meniscus correctly and write the burette reading in the blank provided below. Volume of NaOH = mL
- 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. 20 mL D. 20.1 mL E. 35 mL
- 10.0 g of sulfuric acid and 2.5 grams of sodium hydroxide were added to a beaker that has a total volume of 5.5 L solution what is the resulting pH of the solution?
- What volume of 0.812 M HCl, in mL, is required to titrate 1.33 g of NaOH to the equivalence point? NaOH(aq) + HCl(aq) arrow NaCl(aq) + H2O(l)
- One way to determine the purity of aspirin is to hydrolyze it with a NaOH solution and titrate the remaining NaOH. The reaction between aspirin and NaOH is: C9H8O4(s) + 2OH-(aq) to C7H5O3-(aq) + C2H3O2-(aq) + H2O(l). After boiling 1.54 g of aspirin by add
- Is a titration a neutralization reaction?
- During a titration, 50.0 ml of 0.2 M NaOH was required to neutralize 50.0 ml of H3PO4. What is the concentration of the H3PO4 solution?
- Aqueous sulfuric acid H2SO4 will react with solid sodium hydroxide NaOH to produce aqueous sodium sulfate Na2SO4 and liquid water H2O. Suppose 94g of sulfuric acid is mixed with 49.9g of sodium hydroxide. Calculate the minimum mass of sulfuric acid that c
- How many mL of 0.246 M H_2SO_4 are needed to react with 36.0 mL of 0.322 M NaOH ?
- How do you find the concentration of a base in titration?
- A solution is made by dissolving 0.40 g of solid sodium hydroxide in 250 cm3 of water. It is found that 28.2 cm3 of this solution is needed to completely neutralise a 40.0 cm3 sample of ethanoic acid (CH3COOH) of unknown concentration. Calculate the conce
- In the laboratory you dissolve 21.1 g of copper(II) sulfate in a volumetric flask and add water to a total volume of 375 mL. a. What is the molarity of the solution? b. What is the concentration of the copper(II) cation? c. What is the concentration of th
- How do you calculate concentration in titration?
Explore our homework questions and answers library
Browse
by subject