Question

A 1.25 M solution of the weak acid HA is 9.2 % dissociated. What is the pH of the solution?

Solution

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Answered 4 months ago
Answered 4 months ago
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To calculate the concentration of H+^+, we can use this equation:

percent of ionization=concentration ionizedoriginal concentration×100%(1)\tag1\text{percent of ionization} = \dfrac{\text{concentration ionized}}{\text{original concentration}} \times 100\%

From the ionized concentration, we can calculate the concentration of H+^+ that can be used to calculate pH:

pH=log([H+])(2)\tag2\text{pH} = -\text{log}([\text{H}^+])

The data we're given in the question is:

percent of ionization = 9.2 %

original concentration = 1.25 M

[H+^+] =?

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