Question

What is the pH of a 0.0100 M sodium benzoate solution? Kb (C7H5O2-, ) = 1.5 x 10^-10

Answer 1

The pH of a 0.0100 M sodium benzoate solution with a Kb of 1.5 × 10-¹⁰ is 5.91 (option B).

How to calculate pH?

The pH of a solution in chemistry refers to the notation expressing the acidity or alkalinity of a solution.

The pH is measured on a logarithmic scale of which 7 is neutral, lower values are more acid and higher values more alkaline.

The pH of a solution can be calculated using the following formula;

pH = - log {H+}

pH = - log {0.0100}

pH = 2

Therefore, the pH of a 0.0100 M sodium benzoate solution with a Kb of 1.5 × 10-¹⁰ is 5.91.

Learn more about pH at: brainly.com/question/11300720

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