50 mL of H2O is added to 50 mL of 1 × 10-3 M barium hydroxide solution. What is the pH of the resulting solution?

Question

50 mL of H2O is added to 50 mL of 1 × 10-3 M barium hydroxide solution. What is the pH of the resulting solution? (A) 3.0 (B) 3.3 (C) 11.0 (D) 11.7

Tardigrade Admin · Accepted Answer

In water, barium hydroxide is hydrolysed as follows,

B a (O H)_{2} ⇌ B a^{2 +} + 2 O H^{-}

cone, of

B a^{2 +} = 1 \times 1 0^{- 3} M

cone. Of

[O H^{-}] = 2 \times 1 \times 1 0^{- 3} M

= 2 \times 1 0^{- 3} M

pO H = - lo g [O H^{-}]

= - lo g (2 \times 1 0^{- 3})

= 2.69

p H + pO H = 14

p H = 14 - pO H

= 14 - 2.69

= 11.3

= 11.0

Q. 50mL of H2​O is added to 50mL of 1×10−3M barium hydroxide solution. What is the pH of the resulting solution?