Ionic EquilibriumMedium
Question
The active ingredient in aspirin is acetyl salicylic acid
with Ka = 4.0 × 10–9. The pH of the solution obtained by dissolving two aspirin tablets (containing 0.36 g of acetyl salicylic acid in each tablet) in 250 ml of water is (log 2 = 0.3)
Options
A.5.1
B.8.9
C.10.2
D.5.25
Solution
Conc. of aspirin = $\frac{2 \times 0.36/180}{0.250} = 0.016\text{ M}$
Now, $\left\lbrack H^{+} \right\rbrack = \sqrt{K_{a}.C} = \sqrt{4 \times 10^{- 9} \times 0.016} = 8 \times 10^{- 6}\text{ M}$
∴ PH = 5.1
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