Chemistry: What is the pH of a buffer prepared by adding 0.809 mol of the weak acid HA to 0.406 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10−7.

A. Mass. And your welcome for helping u...

What is the pH of a buffer prepared by adding

crodriguez87

20.01.2022

5.94

Explanation:

Given:-

$K_{a}=5.66\times 10^{-7}$

$pK_{a}=-\log\ K_{a}=-\log\ (5.66\times 10^{-7})=6.24$

[salt] = 0.406 mol

[acid] = 0.809 mol

Considering the Henderson- Hasselbalch equation for the calculation of the pH of the acidic buffer solution as:

$
pH=pK_a+log\frac{[salt]}{acid]}
$

So,

$
pH=6.24+\log (\frac{0.406}{0.809})=5.94
$

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