50 mL of $H_{2}O$ is added to 50 mL of $1 imes 10^{- 3}$ M barium hydroxide solution. What is the pH of the resulting solution?

Question

50 mL of $H_{2}O$ is added to 50 mL of $1 	imes 10^{- 3}$ M barium hydroxide solution. What is the pH of the resulting solution?

Dr. Abubacker · Accepted Answer

(c)
In water, barium hydroxide is hydrolysed as followers
$Ba(OH)_{2} ightleftharpoons {Ba}^{2 +} + \ 2{OH}^{-}$
Conc. Of ${Ba}^{2 +} = 1 	imes 10^{- 3}M$
Conc. of $\left\lbrack {OH}^{-} ightbrack = 2 	imes 1 	imes 10^{- 3}M$
$= 2 	imes 10^{- 3}M$
$pOH = \  - \log{\lbrack{OH}^{-}brack}$
$\ \ \ \ \ \ \ \ \  = \  - \log{(2 	imes 10^{- 3})}$
$\ \ \ \ \ \ \ \ \  = 2.69$
$pH + pOH = 14$
$\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ pH = 14 - pOH$
$= 14 - 2.69$
$\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \  = 11.3$
$\approx 11.0$

Q. 50 mL of $H_{2}O$ is added to 50 mL of $1 \times 10^{- 3}$ M barium hydroxide solution. What is the pH of the resulting solution?

Explanation

Reviewed by Dr. Abubacker

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