First slide

PH of strong acids and strong bases

Question

A 100 mL, 0.1 M solution of ammoniurn acetate is diluted by adding 100 mL of water. The pH of the resulting solution will be ( ${pK}_{a}$ of acetic acid is nearly equal to ${pK}_{b}$ of ${NH}_{4} OH)$

Moderate

A

4.9
B

5.9
C

7.0
D

10.0

Solution

Ammonium acetate is a salt of weak acid and weak base. When solutions are of weak acid and weak base, pH of solution is calculated from the following relationship.
$pH = 7 + \frac{1}{2} {pK}_{a} - \frac{1}{2} {pK}_{b}$
or ${pK}_{a} \approx {pK}_{b} (given)$
$∴ pH of solution = 7$

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