At 25,^oC,the pH of a solution is 2. If the p | vedclass

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(D) The initial $pH$ of the solution is $2$. The concentration of hydronium ions $[H_3O^+]$ is given by the formula $[H_3O^+] = 10^{-pH}$.For $pH = 2$

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decrease to $1/100$th of its original value

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(D) The initial $pH$ of the solution is $2$. The concentration of hydronium ions $[H_3O^+]$ is given by the formula $[H_3O^+] = 10^{-pH}$.For $pH = 2$,$[H_3O^+]_{initial} = 10^{-2} \, M$.If the $pH$ is doubled,the new $pH = 2 	imes 2 = 4$.The new concentration of hydronium ions is $[H_3O^+]_{final} = 10^{-4} \, M$.The ratio of the final concentration to the initial concentration is $\frac{10^{-4}}{10^{-2}} = 10^{-2} = \frac{1}{100}$.Therefore,the concentration of hydronium ions decreases to $1/100$th of its original value.

At $25\,^oC$,the $pH$ of a solution is $2$. If the $pH$ is doubled,the concentration of hydronium ions in the solution will ............

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