What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.44?...
What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.44? The Ka for acetic acid is 1.76 x 10^-5.
The answer choices are
A) .39:1
B) .49:1
C) 1.07:1
D) 1.33:1
E) 4.44:1
It is NOT A according to my professor counting that wrong on the exam, I just want the answer and how it works please!
Homework Answers
Solution:
pH of an acidic buffer is calculated by Henderson equation as:
pH = pKa + log [ salt] / [acid]
Given, ka for acetic acid = 1.76 x 10^-5
Therefore, pKa = -log ka = - log 1.76 x 10^-5
= 5 - log 1.76 = 5 - 0.246 = 4.75
pH = 4.44
Hence, using Henderson equaion,
pH = pka + log [CH3COO- ] /[CH3COOH]
4.44 = 4.75 + log [CH3COO- / CH3COOH]
log [CH3COO- / CH3COOH ] = - 0.31
[CH3COO- / CH3COOH] = antilog -0.31 = 0.49
Therefore, ratio of ,
[CH3COO- / CH3COOH] = 0.49 : 1
Hence, option B.
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