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Questions  >>  JEEMAIN and NEET  >>  Chemistry  >>  Equilibrium
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Q)

The hydronium ion concentration in pure water is $1 \times 10^{-7}$ mol$L^{-1}$. The degree of dissociation of water is

(a) $1.8 \times 10^{-9}$

(b) $0.8 \times 10^{-8}$

(c) $9.8 \times 10^{-6}$

(d) $3 \times 10^{-9}$

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A)
Answer: $1.8 \times 10^{-9}$
 
If $\alpha$ is degree of dissociation
 
$H_2O \rightleftharpoons H^+ + OH^-$
 
Initial Concentration, [$H_2O$] = C mol$L^{-1}$
Equilibrium concentration, $[H_2O] = C(1-\alpha)$ mol $L^{-1}, [H^+] = C\alpha$ mol $L^{-1}, [OH^-] = C\alpha$ mol $L^{-1}$
 
$[H^+] = C\alpha \Rightarrow \alpha = \frac{[H^+]}{C} = \frac{1 \times 10^{-7}}{55.5} = 1.8 \times 10^{-9}$

 

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