The pH of two equimolar weak acids are 3.0 an | vedclass

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Question

(C) The relative strength of acids is defined as the ratio of their hydrogen ion concentrations.For the first acid,$pH = 3.0$,so $[H^{+}]_1 = 10^{-3.0

Vedclass · Accepted Answer

$100:1$

Vedclass · Answer

(C) The relative strength of acids is defined as the ratio of their hydrogen ion concentrations.For the first acid,$pH = 3.0$,so $[H^{+}]_1 = 10^{-3.0} \, M$.For the second acid,$pH = 5.0$,so $[H^{+}]_2 = 10^{-5.0} \, M$.The relative strength is the ratio of $[H^{+}]_1$ to $[H^{+}]_2$:$	ext{Relative Strength} = \frac{[H^{+}]_1}{[H^{+}]_2} = \frac{10^{-3.0}}{10^{-5.0}} = 10^{(-3.0 - (-5.0))} = 10^{2.0} = 100$.Thus,the ratio is $100:1$.

The $pH$ of two equimolar weak acids are $3.0$ and $5.0$ respectively. Their relative strength is

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