Calculate $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$of a monobasic acid if it is $0.04 \%$ dissociated in 0…

Calculate $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$of a monobasic acid if it is $0.04 \%$ dissociated in 0.05 M solution.
  1. $1 \times 10^{-5}$
  2. $1.5 \times 10^{-5}$
  3. $2.0 \times 10^{-5}$
  4. $3.0 \times 10^{-5}$

Solution

$\begin{aligned} & \alpha=\frac{\text { Percentage dissociation }}{100}=\frac{0.04}{100}=4 \times 10^{-4} \\ & {\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=\alpha \times \mathrm{c}=4 \times 10^{-4} \times 0.05 \mathrm{M}=2.0 \times 10^{-5}}\end{aligned}$

Asked in: MHT CET 2024 (02 May Shift 2)

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