Ionic EquilibriumMedium

Question

The first and second ionization constants of a weak dibasic acid $H_{2}\text{ }A$ are $8.1 \times 10^{- 8}$ and $1.0 \times 10^{- 13}$ respectively. 0.1 mol of $H_{2}\text{ }A$ was dissolved in 1L of 0.1 M HCl solution. The concentration of ${HA}^{-}$ in the resultant solution is :

Options

A.0.1 M
B.$9.53 \times 10^{- 6}M$
C.$8.1 \times 10^{- 8}M$
D.$1.0 \times 10^{- 13}M$

Solution

Sol. [Key Concept: In excess strong acid the common-ion effect suppresses dissociation, so $\lbrack{HA}^{-}\rbrack \approx \ K_{a1}$.]

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