17.48 **Exercises: Solubility and Titration****17.43**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, (c) 20.0 mL, (d) 20.1 mL, (e) 35.0 mL.**17.44**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, (c) 24.0 mL, (d) 25.0 mL, (e) 30.0 mL.**17.45**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:(a) 0 mL, (b) 17.5 mL, (c) 34.5 mL, (d) 35.0 mL, (e) 35.5 mL, (f) 50.0 mL.**17.46**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:(a) 0 mL, (b) 20.0 mL, (c) 59.0 mL, (d) 60.0 mL, (e) 61.0 mL, (f) 65.0 mL.**17.47**Calculate the pH at the equivalence point for titrating 0.100 M solutions of each of the following bases with 0.200 M HBr:(a) sodium hydroxide (NaOH),(b) hydroxylamine (NH₂OH),(c) aniline (C₆H₅NH₂

It is given that 0.080 M NaOH is reacting with the given 0.100 M solutions and to calculate the pH…

Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH: (a) hydrobromic acid (HBr), (b) chlorous acid (HCIO2), (c) benzoic acid (C,H§COOH).

Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH: (a) hydrobromic acid (HBr), (b) chlorous acid (HCIO2), (c) benzoic acid (C,H§COOH).

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

17.48

**Exercises: Solubility and Titration**

**17.43**
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, (c) 20.0 mL, (d) 20.1 mL, (e) 35.0 mL.

**17.44**
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, (c) 24.0 mL, (d) 25.0 mL, (e) 30.0 mL.

**17.45**
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:
(a) 0 mL, (b) 17.5 mL, (c) 34.5 mL, (d) 35.0 mL, (e) 35.5 mL, (f) 50.0 mL.

**17.46**
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:
(a) 0 mL, (b) 20.0 mL, (c) 59.0 mL, (d) 60.0 mL, (e) 61.0 mL, (f) 65.0 mL.

**17.47**
Calculate the pH at the equivalence point for titrating 0.100 M solutions of each of the following bases with 0.200 M HBr:
(a) sodium hydroxide (NaOH),
(b) hydroxylamine (NH₂OH),
(c) aniline (C₆H₅NH₂

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3.3