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Principles of General Chemistry | 2nd Edition | ISBN: 9780073511085 | Authors: Martin S. Silberberg
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In a 0.735M solution, a weak acid is 12.5% dissociated.(a)

Chapter 18, Problem 52P

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QUESTION:

Problem 52P

In a 0.735M solution, a weak acid is 12.5% dissociated.

(a) Calculate the [H3O+], pH, [OH?], and pOH of the solution.

(b) Calculate Kaof the acid.

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QUESTION:

Problem 52P

In a 0.735M solution, a weak acid is 12.5% dissociated.

(a) Calculate the [H3O+], pH, [OH?], and pOH of the solution.

(b) Calculate Kaof the acid.

ANSWER:

Step 1 of 4

pH is classified as a number that basically measures the amount of  ions in any acidic solution. For acidic solutions, this value ranges between 0-7 while for alkaline solutions, this value ranges from 7 to 14.

Given Data:

*The concentration of weak acid is 0.735 M.

*The percentage dissociation of acid is 12.5%.

Suppose the weak acid is HA. Its dissociation is as follows:

12.5% of HA has been dissociated into  and  ions.

Therefore, concentration of  is:

So, the concentration of hydronium ions is .

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