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(D) For a polyprotic acid $H_2A$,the dissociation steps are:$H_2A ightleftharpoons H^{+} + HA^{-}$; $K_1 = \frac{[H^{+}][HA^{-}]}{[H_2A]} = 1.0 	im

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$5.0 	imes 10^{-15}$

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(D) For a polyprotic acid $H_2A$,the dissociation steps are:$H_2A ightleftharpoons H^{+} + HA^{-}$; $K_1 = \frac{[H^{+}][HA^{-}]}{[H_2A]} = 1.0 	imes 10^{-5}$$HA^{-} ightleftharpoons H^{+} + A^{2-}$; $K_2 = \frac{[H^{+}][A^{2-}]}{[HA^{-}]} = 5.0 	imes 10^{-10}$The overall dissociation reaction is the sum of these two steps:$H_2A ightleftharpoons 2H^{+} + A^{2-}$The overall dissociation constant $K$ is the product of the individual dissociation constants:$K = K_1 	imes K_2$$K = (1.0 	imes 10^{-5}) 	imes (5.0 	imes 10^{-10})$$K = 5.0 	imes 10^{-15}$

$A$. $HI$	$(i)$ $3.2 \times 10^9$
$B$. $HF$	$(ii)$ $3.5 \times 10^{-4}$
$C$. $HCl$	$(iii)$ $1.3 \times 10^6$
$D$. $HBr$	$(iv)$ $1.0 \times 10^9$

The first and second dissociation constants of an acid $H_2A$ are $1.0 \times 10^{-5}$ and $5.0 \times 10^{-10}$ respectively. The overall dissociation constant of the acid will be

Similar Questions

Which of the following is a Lewis acid but not a Bronsted acid?

Identify the conjugate acid and conjugate base respectively in the following reaction:
$H_2O + HCl_{(aq)} \leftrightharpoons H_3O^{+} + Cl_{(aq)}^{-}$

Which one of the following statements is not correct?

Match the given ionisation constant values with the corresponding acids.
$A$. $HI$ $(i)$ $3.2 \times 10^9$
$B$. $HF$ $(ii)$ $3.5 \times 10^{-4}$
$C$. $HCl$ $(iii)$ $1.3 \times 10^6$
$D$. $HBr$ $(iv)$ $1.0 \times 10^9$

The correct match is:

The conjugate base of $NH_4^{+}$ is

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