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Calculate the $\mathrm{pH}$ of $1.36 \times 10^{-2} \mathrm{M}$ solution of perchloric acid.
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Verified Answer
The correct answer is:
$1.86$
Perchloric acid is a strong monobasic acid. Hence, $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=1.36 \times 10^{-2} \mathrm{M}$
$$
\begin{aligned}
\therefore \quad \mathrm{pH} & =-\log _{10}\left[\mathrm{H}_3 \mathrm{O}^{+}\right] \\
& =-\log _{10}\left[1.36 \times 10^{-2}\right] \\
& =-\log _{10} 1.36-\log _{10} 10^{-2} \\
& =-\log _{10} 1.36+2 \\
& =2-0.1335 \\
\therefore \quad \mathrm{pH} & =1.86
\end{aligned}
$$
$$
\begin{aligned}
\therefore \quad \mathrm{pH} & =-\log _{10}\left[\mathrm{H}_3 \mathrm{O}^{+}\right] \\
& =-\log _{10}\left[1.36 \times 10^{-2}\right] \\
& =-\log _{10} 1.36-\log _{10} 10^{-2} \\
& =-\log _{10} 1.36+2 \\
& =2-0.1335 \\
\therefore \quad \mathrm{pH} & =1.86
\end{aligned}
$$
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