Hydrogen ion concentration of an aqueous solu | vedclass

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(C) Initial concentration of $[H^{+}] = 1 	imes 10^{-4} \ M$. When the solution is diluted with an equal volume of water,the total volume becomes dou

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$2 	imes 10^{-10}$

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(C) Initial concentration of $[H^{+}] = 1 	imes 10^{-4} \ M$. When the solution is diluted with an equal volume of water,the total volume becomes double,so the concentration of $[H^{+}]$ is halved: $[H^{+}]_{new} = \frac{1 	imes 10^{-4}}{2} = 0.5 	imes 10^{-4} \ M$. Using the ionic product of water,$K_w = [H^{+}][OH^{-}] = 1 	imes 10^{-14}$. $[OH^{-}] = \frac{K_w}{[H^{+}]_{new}} = \frac{1 	imes 10^{-14}}{0.5 	imes 10^{-4}} = 2 	imes 10^{-10} \ mol \ dm^{-3}$.

Hydrogen ion concentration of an aqueous solution is $1 \times 10^{-4} \ M$. The solution is diluted with an equal volume of water. The hydroxyl ion concentration of the resultant solution in terms of $mol \ dm^{-3}$ is

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