×
Log in to StudySoup
Get Full Access to Quantitative Chemical Analysis - 8 Edition - Chapter 8 - Problem 8-29
Join StudySoup for FREE
Get Full Access to Quantitative Chemical Analysis - 8 Edition - Chapter 8 - Problem 8-29

Already have an account? Login here
×
Reset your password

Why does buffer capacity increase as a solution becomes very acidic (pH 1) or very basic

Quantitative Chemical Analysis | 8th Edition | ISBN: 9781429218153 | Authors: Daniel C. Harris ISBN: 9781429218153 475

Solution for problem 8-29 Chapter 8

Quantitative Chemical Analysis | 8th Edition

  • Textbook Solutions
  • 2901 Step-by-step solutions solved by professors and subject experts
  • Get 24/7 help from StudySoup virtual teaching assistants
Quantitative Chemical Analysis | 8th Edition | ISBN: 9781429218153 | Authors: Daniel C. Harris

Quantitative Chemical Analysis | 8th Edition

4 5 1 409 Reviews
16
0
Problem 8-29

Why does buffer capacity increase as a solution becomes very acidic (pH 1) or very basic (pH 13)?

Step-by-Step Solution:
Step 1 of 3

Equilibrium Calculations • ex. CO(g) + H2O(g)⁶CO2(g) + H2(g) Kc=0.64 You start with 1.0 mol CO and 1.0 mol CO2 in a 1 L flask. You then add 2.0 mol H2O. What is the concentration of H2 at equilibrium Check for equilibrium first: Q does not equal 0—>system not in equilibrium Make ICE table: CO(g) + H2O(g) ⁶ CO2(g) + H2(g) Initial 1.0 M 2.0 M 1.0 M 0 M Change -x -x +x +x Equilibrium (1.0-x) (2.0-x) (1.0+x) x Kc = 0.64 = [1.0+x][x] [1.0-x][2.0-x] 0.64 = x + x^2 2 - 3x + x^2 0.64(2 - 3x + x^2) = x + x^2 -0.36x^2 - 2.92x + 1.28 = 0 *sta

Step 2 of 3

Chapter 8, Problem 8-29 is Solved
Step 3 of 3

Textbook: Quantitative Chemical Analysis
Edition: 8
Author: Daniel C. Harris
ISBN: 9781429218153

Other solutions

People also purchased

Related chapters

Unlock Textbook Solution

Enter your email below to unlock your verified solution to:

Why does buffer capacity increase as a solution becomes very acidic (pH 1) or very basic