Determine the pH at the point in the titrationof 40.0 mL of 0.200 M HC,H,02 with 0.100 MSr(OH)2 after 10.0 mL of the strong base hasbeen added. The value of Ka for HC4H,O2 is 1.5x 10-5.124>Based on your ICE table and definition of Ka,set up the expression for Ka in order todetermine the unknown. Do not combine orsimplify terms.Ka == 1.5 x 10-55 RESET[0][0.100][0.120][0.140][0.0200][0.0400][x][2x][0.100 + x][0.100 - x][0.120 + x][0.120 - x][0.140 + x][0.140 - x][0.0200 + x][0.0200 - x][0.0400 + x][0.0400 - x] Determine the pH at the point in the titrationof 40.0 mL of 0.200 M HC4H,O2 with 0.100MSr(OH)2 after 10.0 mL of the strong base hasbeen added. The value of Ka for HC,H,02 is 1.5x 10-5.1234Based on your ICE table and Ka expression,determine the pH of the solution.pH =5 RESET4.354.49 x 10-9.653.9910.02.23 x 10-101.403.23

The expression for the degree of dissociation of a weak acid is: α=KaC Therefore, the concentration…

Answered: Determine the pH at the point in the…

Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC,H,O2 with 0.100 M Sr(OH)2 after 10.0 mL of the strong base has been added. The value of Ka for HC4H,O2 is 1.5 x 10-5.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.52QE

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Determine the pH at the point in the titration
of 40.0 mL of 0.200 M HC,H,02 with 0.100 M
Sr(OH)2 after 10.0 mL of the strong base has
been added. The value of Ka for HC4H,O2 is 1.5
x 10-5.
1
2
4
>
Based on your ICE table and definition of Ka,
set up the expression for Ka in order to
determine the unknown. Do not combine or
simplify terms.
Ka =
= 1.5 x 10-5
5 RESET
[0]
[0.100]
[0.120]
[0.140]
[0.0200]
[0.0400]
[x]
[2x]
[0.100 + x]
[0.100 - x]
[0.120 + x]
[0.120 - x]
[0.140 + x]
[0.140 - x]
[0.0200 + x]
[0.0200 - x]
[0.0400 + x]
[0.0400 - x]

Determine the pH at the point in the titration
of 40.0 mL of 0.200 M HC4H,O2 with 0.100M
Sr(OH)2 after 10.0 mL of the strong base has
been added. The value of Ka for HC,H,02 is 1.5
x 10-5.
1
2
3
4
Based on your ICE table and Ka expression,
determine the pH of the solution.
pH =
5 RESET
4.35
4.49 x 10-
9.65
3.99
10.0
2.23 x 10-10
1.40
3.23

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