Find $\left[\mathrm{OH}^{-}\right]$if a monoacidic base is $3 \%$ ionised in its $0.04 \mathrm{M}$ solution.

Find $\left[\mathrm{OH}^{-}\right]$if a monoacidic base is $3 \%$ ionised in its $0.04 \mathrm{M}$ solution.
  1. $3.1 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1}$
  2. $4.5 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1}$
  3. $9.0 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1}$
  4. $1.2 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1}$

Solution

For a monoacidic base, $\begin{aligned} & {\left[\mathrm{OH}^{-}\right]=\mathrm{c} \times \alpha} \\ & {\left[\mathrm{OH}^{-}\right]=0.04 \times \frac{3}{100}} \\ & {\left[\mathrm{OH}^{-}\right]=1.2 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1}} \end{aligned}$

Asked in: MHT CET 2023 (12 May Shift 1)

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