Homework Help is Here – Start Your Trial Now!
Science
Chemistry
15.64 Calculate the pH of a buffer solution that is 0.20 M in HCN and 0.12 M in NaCN. Will the pH change if the solution is diluted by a factor of 2? Explain.

15.64 Calculate the pH of a buffer solution that is 0.20 M in HCN and 0.12 M in NaCN. Will the pH change if the solution is diluted by a factor of 2? Explain.

Chemistry
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...
See similar textbooks
icon
Related questions
icon
Concept explainers
Question

Can you please answer 15.64 and show all of the steps to the solution 

Here’s a transcription and explanation suitable for an educational website: --- **Buffer Capacity Exercises** **15.62** Evaluate the pH change when equal volumes of the two solutions are mixed: - (a) 0.10 M NH₃ and 0.10 M HCl - (b) 100 mL of 0.10 M HCl and 0.10 M NaOH **15.63** Which of the following buffer solutions has the greater buffer capacity? - (a) 50 mL of 0.30 M HNO₂-0.30 M NaNO₂ - (b) 50 mL of 0.40 M NH₄Br-0.60 M NH₃ **15.64** Calculate the pH of a buffer solution that is 0.20 M in HCN and 0.12 M in NaCN. Will the pH change if the solution is diluted by a factor of 2? Explain. **15.65** Calculate the pH of a buffer solution prepared by dissolving 4.2 g of NaHCO₃ and 5.3 g of Na₂CO₃ in 0.20 L of water. Will the pH change if the solution volume is increased by a factor of 10? Explain. --- *Explanation*: The exercises focus on understanding buffer solutions, which resist changes in pH when small amounts of acids or bases are added. Exercises probe into the effect of dilution and concentration on buffer capacity and pH, encouraging the application of the Henderson-Hasselbalch equation for calculating pH.
Transcribed Image Text:Here’s a transcription and explanation suitable for an educational website: --- **Buffer Capacity Exercises** **15.62** Evaluate the pH change when equal volumes of the two solutions are mixed: - (a) 0.10 M NH₃ and 0.10 M HCl - (b) 100 mL of 0.10 M HCl and 0.10 M NaOH **15.63** Which of the following buffer solutions has the greater buffer capacity? - (a) 50 mL of 0.30 M HNO₂-0.30 M NaNO₂ - (b) 50 mL of 0.40 M NH₄Br-0.60 M NH₃ **15.64** Calculate the pH of a buffer solution that is 0.20 M in HCN and 0.12 M in NaCN. Will the pH change if the solution is diluted by a factor of 2? Explain. **15.65** Calculate the pH of a buffer solution prepared by dissolving 4.2 g of NaHCO₃ and 5.3 g of Na₂CO₃ in 0.20 L of water. Will the pH change if the solution volume is increased by a factor of 10? Explain. --- *Explanation*: The exercises focus on understanding buffer solutions, which resist changes in pH when small amounts of acids or bases are added. Exercises probe into the effect of dilution and concentration on buffer capacity and pH, encouraging the application of the Henderson-Hasselbalch equation for calculating pH.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Ionic Equilibrium
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS