USEFUL FORMULApKa = - log KapH = pKa + log A- / HApH = pKa + log A-/ HApH = pKa + log (equivalent salt-%3D%3Dequivalent acid added).(equivalent acid +equivalent acid added)Buffer capacity = no. of%3Dequivalent acid/base added4 in pH x vouтein litersPart II1. A buffer is prepared containing 1.00 molar AceticAcid and 1.00 molar Sodium Acetate. What is its pHif the Ka of acetic acid is 1.77 x 10 -52. Calculate the pH using Henderson-Hasselbalchequation of a 50mL buffer solution made from 0.20M HC2H302 and 0.50 M C2H3O2- that has an aciddissociation constant, Ka for HC2H302 of 1.8 x 10a.) What will be the change in pH of thebuffer solution after the addition of 1.0 mL of 0.10NHCIb.) What is the total buffer capacity of thesolution?

A buffer solution is made by the mixture of a weak acid with its conjugate base or by the mixture of…

Answered: 1. A buffer is prepared containing 1.00…

1. A buffer is prepared containing 1.00 molar Acetic Acid and 1.00 molar Sodium Acetate. What is its pH if the Ka of acetic acid is 1.77 x 10 -5

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

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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

USEFUL FORMULA
pKa = - log Ka
pH = pKa + log A- / HA
pH = pKa + log A-/ HA
pH = pKa + log (equivalent salt-
%3D
%3D
equivalent acid added).
(equivalent acid +
equivalent acid added)
Buffer capacity = no. of
%3D
equivalent acid/base added
4 in pH x vouтe
in liters
Part II
1. A buffer is prepared containing 1.00 molar Acetic
Acid and 1.00 molar Sodium Acetate. What is its pH
if the Ka of acetic acid is 1.77 x 10 -5
2. Calculate the pH using Henderson-Hasselbalch
equation of a 50mL buffer solution made from 0.20
M HC2H302 and 0.50 M C2H3O2- that has an acid
dissociation constant, Ka for HC2H302 of 1.8 x 10
a.) What will be the change in pH of the
buffer solution after the addition of 1.0 mL of 0.10N
HCI
b.) What is the total buffer capacity of the
solution?

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