If [H^{+}] ion concentration of a solution is | vedclass

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(C) The $pH$ of a solution is defined as $pH = -\log[H^{+}]$.Let the initial concentration be $[H^{+}]_1 = C$,then $pH_1 = -\log(C)$.If the concentrat

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Decrease by $1$

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(C) The $pH$ of a solution is defined as $pH = -\log[H^{+}]$.Let the initial concentration be $[H^{+}]_1 = C$,then $pH_1 = -\log(C)$.If the concentration is increased by $10$ times,the new concentration is $[H^{+}]_2 = 10C$.The new $pH$ is $pH_2 = -\log(10C) = -(\log(10) + \log(C)) = -(1 + \log(C)) = -1 - \log(C)$.Comparing the two,$pH_2 = pH_1 - 1$.Therefore,the $pH$ decreases by $1$.

If $[H^{+}]$ ion concentration of a solution is increased by $10$ times,its $pH$ will be:

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