solutionC2. Effect of a base on the pH of a buffer solutionSolutionUsedInitial pHpH afteradding 5drops ofКОНpH afteraddingadditional 5Change inpHIs the testedsolution abuffer? Yesor Nodrops ofКОНWater6.9810.2511.780.1 M KCI6.409.7810.54solutionpH 12 buffersolution11.9812.1812.53pH 1 buffersolution2.052.342.65étv3MacBook AirDIIDD80888F11F9F10F8F6F7F3F4F5F1F2*#$&

Buffer solutions are solutions containing acid-base conjugate pairs, that is, weak acid and its…

Answered: Change in pH Is the tested solution a…

Science

Chemistry

Change in pH Is the tested solution a buffer? Yes or No

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 16.58QE

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Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

solution
C2. Effect of a base on the pH of a buffer solution
Solution
Used
Initial pH
pH after
adding 5
drops of
КОН
pH after
adding
additional 5
Change in
pH
Is the tested
solution a
buffer? Yes
or No
drops of
КОН
Water
6.98
10.25
11.78
0.1 M KCI
6.40
9.78
10.54
solution
pH 12 buffer
solution
11.98
12.18
12.53
pH 1 buffer
solution
2.05
2.34
2.65
étv
3
MacBook Air
DII
DD
80
888
F11
F9
F10
F8
F6
F7
F3
F4
F5
F1
F2
*
#
$
&

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A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
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8-55 We commonly refer to a buffer as consisting of approximately equal molar amounts of a weak acid and its conjugate base—for example, CH3COOH and CH3COO-. Is it also possible to have a buffer consisting of approximately equal molar amounts of a weak base and its conjugate acid? Explain.
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