The pH of a solution of 4-chlorobutanoic acid is measured to be . Calculate the acid dissociation constant of 4-chlorobutanoic acid. Round your answer to significant digits.

Explanation:

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In this case, as you are not indicating the molarity of the solution and its pH we are going to assume they are 1.4 M and 2.19 respectively as typical problems over this. In such a way, based on the pH we can compute the concentration of hydrogen ions in the solution:

Next, the dissociation of 4-chlorobutanoic acid is:

Since it is a weak acid, therefore, its equilibrium expression is:

Since the concentration of hydrogen ions equal the concentration of 4-chlorobutanoate ions at equilibrium and the concentration the 4-chlorobutanoic acid equals 1.4 M minus the concentration of hydrogen ions, which is related to the reaction extent , the acid dissociation constant is:

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answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error