Question

What is the pH of a 0.0100 M sodium benzoate solution? Kb (C7H5O2-, ) = 1.5 x 10^-10. Show how it is worked out.

Answer 1

The pH of a 0.0100 M sodium benzoate solution is determined as 8.09.

What is pH of a solution?

The pH of a solution is a measure of hydrogen (H+) ion concentration, which is, in turn, a measure of acidity of the solution.

pH is can also be determined from pOH of the solution as shown below;

pH = 14 - pOH

pH of the benzoate solution

let the hydroxyl concentration, OH = x

x²/M = kb

x²/0.01 = 1.5 x 10⁻¹⁰

x² = 1.5 x 10⁻¹²

x = √(1.5 x 10⁻¹²)

x = 1.2247 x 10⁻⁶

pOH = - log(OH⁻)

pOH = -log( 1.2247 x 10⁻⁶)

pOH = 5.91

Calculate the value of the pH

pH = 14 - 5.91

pH = 8.09

Thus, the pH of a 0.0100 M sodium benzoate solution is determined as 8.09.

Learn more about pH here: brainly.com/question/13557815

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