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  • The dissociation constants of an acid <img alt="\left(\mathrm{H}_2 \mathrm{~A}\right)" src="https://entrancecorner.oncodecogs.com/gif.latex?%5Cleft%28%5Cmathrm%7BH%7D_2%20%5Cmathrm%7B%7EA%7D%5

The dissociation constants of an acid \left(\mathrm{H}_2 \mathrm{~A}\right) are 3 \times 10^{-5} and 7 \times 10^{-9}  respectively. The overall dissociation constant of the acid will be
 

Option: 1

21 \times 10^{-14}


Option: 2

22 \times 10^{-3}


Option: 3

32 \times 10^{-5}


Option: 4

28 \times 10^{-6}


Answers (1)

best_answer

\begin{aligned} & \mathrm{H}_2 \mathrm{A}=\mathrm{HA}^{-}+\mathrm{H}^{+} \\ & \mathrm{K}_1=\frac{\left[\mathrm{HA}^{-}\right]\left[\mathrm{H}^{+3}\right.}{\left[\mathrm{H}_2 \mathrm{~A}\right]} \\ & \mathrm{HA}=\mathrm{H}^{+} \mathrm{A}^{2-} \\ & \mathrm{K}_2=\frac{\left[\mathrm{H}^{+}\right]\left[\mathrm{A}^{2-}\right]}{\left[\mathrm{HA}^{-}\right]} \end{aligned}
\text{ for Rxn}:- \mathrm{K=\frac{\left[H^{+}\right]\left[A^{2-}\right]}{\left[H_2 A\right]}=k_1 k_2}
\begin{aligned} & =3 \times 10^{-5} \times 7 \times 10^{-9} \\ & =21 \times 10^{-14} \end{aligned}

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Gautam harsolia

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