Calculate the $[\mathrm{OH}]$ if pOH of solution is 4.94

Calculate the $[\mathrm{OH}]$ if pOH of solution is 4.94
  1. $2.356 \times 10^{-5} \mathrm{M}$
  2. $1.881 \times 10^{-5} \mathrm{M}$
  3. $\quad 1.417 \times 10^{-5} \mathrm{M}$
  4. $1.148 \times 10^{-5} \mathrm{M}$

Solution

$\begin{array}{ll} & \mathrm{pOH}=-\log _{10}\left[\mathrm{OH}^{-}\right] \\ \therefore \quad & \log _{10}\left[\mathrm{OH}^{-}\right]=-4.94 \\ \therefore \quad & {\left[\mathrm{OH}^{-}\right]=10^{(-4.94)}=1.148 \times 10^{-5} \mathrm{M}}\end{array}$

Asked in: MHT CET 2024 (04 May Shift 2)

Practice more Ionic Equilibria questions on Aicharya