Find the ph of of 100 ml of an aqueous 0.43m baoh2 solution

Question

Chemistry

Ty Hickman

4 October, 09:32

Find the ph of of 100 ml of an aqueous 0.43m baoh2 solution

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Answers (1)

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Rory Hayes · Answer 1

Answer is: pH of barium hydroxide is 13.935.

Chemical dissociation of barium hydroxide in water:

Ba (OH) ₂ (aq) → Ba²⁺ (aq) + 2OH⁻ (aq).

c (Ba (OH) ₂) = 0.43 M.

V (Ba (OH) ₂) = 100 mL : 1000 mL/L = 0.1 L.

n (Ba (OH) ₂) = 0.43 mol/L · 0.1 L.

n (Ba (OH) ₂) = 0.043 mol.

From chemical reaction: n (Ba (OH) ₂) : n (OH⁻) = 1 : 2.

n (OH⁻) = 0.086 mol.

c (OH⁻) = 0.86 mol/L.

pOH = - logc (OH⁻).

pOH = 0.065.

pH = 14 - 0.065 = 13.935.