Asolution is prepared by dissolving 0.56 g of benzoic acid (c6h5co2h, ka 6.4 ) in enough water to make 1.0 l of solution. calculate [c6h5co2h], , , , and the ph of this solution.

The values of

Explanation:

Dissolving benzoic acid

Water in solution

Step 1:

Mass of benzoic acid dissolved in water

Final volume

The benzoic acid dissociation constant:

The number of moles of benzoic acid:

Molarity of benzoic acid:

Step 2:

Calculate the molarity (M) of benzoic acid.

For this, we must first calculate the molar mass and the number of moles (n) of benzoic acid:

Step 3:

Dissociation equations and the dissociation constants:

Step 4:

The approximation for is 0. (because of autonization)

Step 5:

Symbol x represents the change in the concentrations.

Step 6:

Substituting x into the equilibrium expression:

We must determine if the is much smaller than to decide whether the following approximation is valid or not:

The approximation is not valid since more than of acid is dissociated.

Step 7:

Calculating the concentrations of the species and the :

Use the quadratic formula to calculate .

Thus we can say the results are:

To learn more about pH of the solution, refer:

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