What is the ph of a 3.5*10^-11 m h + solution

Question

Kerr

Chemistry

15 January, 02:50

What is the ph of a 3.5*10^-11 m h + solution

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Answers (1)

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Craig Huber · Answer 1

The pH of the solution is 10,46.

Explanation:

The pH gives us an idea of the acidity or basicity of a solution. More precisely, it indicates the concentration of H30 + ions present in said solution. The pH scale ranges from 0 to 14: from 0 to 7 corresponds to acid solutions, 7 neutral solutions and between 7 and 14 basic solutions. It is calculated as:

pH = - log (H30 + )

pH = - log (3.5*10^-11)

pH = 10,46