Assuming that \(\mathrm{Ba(OH)_2}\) is completely ionised in aqueous solution under the given conditions the concentration of \(\mathrm{H_3O^+}\) ions in 0.005 M aqueous solution of \(\mathrm{Ba(OH)_2}\) at 298 K is ______________ \(\times 10^{-12}\) mol L-1. (Nearest integer)
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Correct Answer: 1
Solution and Explanation
\([\mathrm{H_3O^+}] = \frac{K_w}{[\mathrm{OH^-}]} = \frac{10^{-14}}{10^{-2}} = 10^{-12}\) mol L-1.
So the value is \(1 \times 10^{-12}\), x = 1.
Answer: 1
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