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2 years ago

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.

Chemistry

1 answer:

Yuki888 [10]2 years ago

3 0

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

<h3>What is pH of a solution?</h3>

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

<h3>pH of the benzoate solution</h3>

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

<h3>Calculate the value of the pH</h3>

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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$n_1,M_1\text{ and }V_1$ are the n-factor, molarity and volume of acid which is $H_2SO_4$

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Hence, the concentration of original sulfuric acid solution is 1.62 M

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