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Problem 32b
You have to prepare a pH = 5.00 buffer, and you have the following 0.10 M solutions available: HCOOH, HCOONa, CH3COOH, CH3COONa, HCN, and NaCN. How many milliliters of each solution would you use to make approximately 1 L of the buffer?
Problem 33d
The accompanying graph shows the titration curves for two monoprotic acids. (d) Estimate the pKa of the weak acid.
- Compare the titration of a strong, monoprotic acid with a strong base to the titration of a weak, monoprotic acid with a strong base. Assume the strong and weak acid solutions initially have the same concentrations. Indicate whether the following statements are true or false: (b) The pH at the beginning of the titration is lower for the weak acid than the strong acid. (c) The pH at the equivalence point is 7 no matter which acid is titrated.
Problem 34
Problem 34a
Compare the titration of a strong, monoprotic acid with a strong base to the titration of a weak, monoprotic acid with a strong base. Assume the strong and weak acid solutions initially have the same concentrations. Indicate whether the following statements are true or false. (a) More base is required to reach the equivalence point for the strong acid than the weak acid.
Problem 35a
The samples of nitric and acetic acids shown here are both titrated with a 0.100 M solution of NaOH(aq).
Determine whether each of the following statements concerning these titrations is true or false. (a) A larger volume of NaOH1aq2 is needed to reach the equivalence point in the titration of HNO3.
Problem 36a
Determine whether each of the following statements concerning the titrations in Problem 17.35 is true or false. (a) The pH at the beginning of the two titrations will be the same.
Problem 36b
Determine whether each of the following statements concerning the titrations in Problem 17.35 is true or false. (b) The titration curves will both be essentially the same after passing the equivalence point.
Problem 37a,c
Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (a) NaHCO3 titrated with NaOH (c) KOH titrated with HBr.
Problem 37b
Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (b) NH3 titrated with HCl.
Problem 38a
Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (a) formic acid titrated with NaOH.
Problem 38b
Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (b) calcium hydroxide titrated with perchloric acid.
Problem 38c
Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (c) pyridine titrated with nitric acid.
Problem 40a
Assume that 30.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HA. (a) How many moles of HA have been added at the equivalence point?
Problem 40b
Assume that 30.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HA. (b) What is the predominant form of B at the equivalence point?
Problem 40c
Assume that 30.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HA. (c) Is the pH 7, less than 7, or more than 7 at the equivalence point?
Problem 41b
How many milliliters of 0.0850 M NaOH are required to titrate each of the following solutions to the equivalence point: (b) 35.0 mL of 0.0850 M CH3COOH?
Problem 41c
How many milliliters of 0.0850 M NaOH are required to titrate each of the following solutions to the equivalence point: (c) 50.0 mL of a solution that contains 1.85 g of HCl per liter?
Problem 42a,c
How many milliliters of 0.105 M HCl are needed to titrate each of the following solutions to the equivalence point: (a) 45.0 mL of 0.0950 M NaOH? (c) 125.0 mL of a solution that contains 1.35 g of NaOH per liter?
Problem 42b
How many milliliters of 0.105 M HCl are needed to titrate each of the following solutions to the equivalence point: (b) 22.5 mL of 0.118 M NH3?
Problem 43a,b
A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added:
(a) 15.0 mL
(b) 19.9 mL.
Problem 43c
A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added:
(c) 20.0 mL.
Problem 43e
A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added: (e) 35.0 mL.
Problem 44a,b
A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added: (a) 20.0 mL. (b) 23.0 mL.
Problem 44c
A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added: (c) 24.0 mL.
Problem 44d,e
A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added: (d) 25.0 mL. (e) 30.0 mL.
- A 35.0-mL sample of 0.150 M acetic acid (CH3COOH) is titrated with 0.150 M NaOH solution. Calculate the pH after the following volumes of base have been added: (c) 34.5 mL, (d) 35.0 mL, (e) 35.5 mL, (f) 50.0 mL.
Problem 45
Problem 45b
A 35.0-mL sample of 0.150 M acetic acid 1CH3COOH2 is titrated with 0.150 M NaOH solution. Calculate the pH after the following volumes of base have been added: (b) 17.5 mL.
Problem 46b,c
Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCl. Calculate the pH after the following volumes of titrant have been added: (b) 20.0 mL (c) 59.0 mL.
Problem 46e,f
Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCl. Calculate the pH after the following volumes of titrant have been added: (e) 61.0 mL (f) 65.0 mL.
Problem 47a
Calculate the pH at the equivalence point for titrating 0.200 M solutions of each of the following bases with 0.200 M HBr: (a) sodium hydroxide (NaOH).