Calculate the pH of 1.36 times 10^{-2} M sol | vedclass

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Question

(B) Perchloric acid $(HClO_4)$ is a strong monobasic acid,so it dissociates completely in water. $[H_3O^{+}] = [HClO_4] = 1.36 	imes 10^{-2} \ M$ $pH

Vedclass · Accepted Answer

$1.86$

Vedclass · Answer

(B) Perchloric acid $(HClO_4)$ is a strong monobasic acid,so it dissociates completely in water. $[H_3O^{+}] = [HClO_4] = 1.36 	imes 10^{-2} \ M$ $pH = -\log_{10}[H_3O^{+}]$ $pH = -\log_{10}(1.36 	imes 10^{-2})$ $pH = -(\log_{10} 1.36 + \log_{10} 10^{-2})$ $pH = -\log_{10} 1.36 - (-2)$ $pH = 2 - 0.1335$ $pH = 1.8665 \approx 1.87$ Given the options,the closest value is $1.86$.

Calculate the $pH$ of $1.36 \times 10^{-2} \ M$ solution of perchloric acid.

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