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

Calculate the $\mathrm{pH}$ of $1.36 \times 10^{-2} \mathrm{M}$ solution of perchloric acid.
  1. $1.43$
  2. $1.86$
  3. $2.43$
  4. $2.86$

Solution

Perchloric acid is a strong monobasic acid. Hence, $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=1.36 \times 10^{-2} \mathrm{M}$ $\begin{aligned} \therefore \quad \mathrm{pH} & =-\log _{10}\left[\mathrm{H}_3 \mathrm{O}^{+}\right] \\ & =-\log _{10}\left[1.36 \times 10^{-2}\right] \\ & =-\log _{10} 1.36-\log _{10} 10^{-2} \\ & =-\log _{10} 1.36+2 \\ & =2-0.1335 \\ \therefore \quad \mathrm{pH} & =1.86 \end{aligned}$

Asked in: MHT CET 2023 (11 May Shift 1)

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