(C) $H_2SO_4$ is a strong diprotic acid,so it dissociates completely as: $H_2SO_4 \rightarrow 2H^{+} + SO_4^{2-}$.Concentration of $[H^{+}] = 2 \times

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(C) $H_2SO_4$ is a strong diprotic acid,so it dissociates completely as: $H_2SO_4 \rightarrow 2H^{+} + SO_4^{2-}$.Concentration of $[H^{+}] = 2 \times 0.001 \ M = 0.002 \ M = 2 \times 10^{-3} \ M$.Using the ionic product of water at $25^{\circ}C$,$K_w = [H^{+}][OH^{-}] = 10^{-14}$.$[OH^{-}] = \frac{K_w}{[H^{+}]} = \frac{10^{-14}}{2 \times 10^{-3}}$.$[OH^{-}] = 0.5 \times 10^{-11} \ M = 5 \times 10^{-12} \ M$.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)pH of strong Acids and strong Bases

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The concentration in $M$ of $OH^{-}$ in $0.001 \ M$ $H_2SO_4$ is

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A
$1 \times 10^{-13}$
B
$0.5 \times 10^{-12}$
C
$5 \times 10^{-12}$
D
$0.5 \times 10^{-13}$

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6-2.Equilibrium-II (Ionic Equilibrium)

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pH of strong Acids and strong Bases

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The concentration in $M$ of $OH^{-}$ in $0.001 \ M$ $H_2SO_4$ is

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At $298 \, K$,what is the concentration of hydrogen ions in a $10^{-8} \, M \, HCl$ aqueous solution? $(K_W = 10^{-14})$

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