A chemist dissolves of pure barium hydroxide in enough water to make up of solution. calculate the ph of the solution. (the temperature of the solution is.) be sure your answer has the correct number of significant digits.

Question

Madilynn Graves

Chemistry

22 March, 13:46

A chemist dissolves of pure barium hydroxide in enough water to make up of solution. calculate the ph of the solution. (the temperature of the solution is.) be sure your answer has the correct number of significant digits.

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Gabriela Michael · Answer 1

Barium Hydroxide is a strong base, so it would completely dissociate to Ba²⁺ and OH⁻. But it is crucial to know the concentration of the Ba (OH) ₂ solution. For example, if you dissolve 1 g in 1 L of solution, then the concentration would be:

C = (1 g) (1 mol Ba (OH) ₂/171.34 g) / 1 L = 5.84*10⁻³ M

So, the concentration of [OH⁻] is

[OH⁻] = 5.84*10⁻³*2 = 0.0117 M

pH = 14 - - log (0.0117)

pH = 12.07