Calculate the pH at 25°C of a 0.86M solution of potassium butanoate KC3H7CO2. Note that butanoic acid HC3H7CO2 is a weak acid with a pKa of 4.82.Round your answer to 1 decimal place.
Question
Calculate the pH at 25°C of a 0.86M solution of potassium butanoate KC3H7CO2. Note that butanoic acid HC3H7CO2 is a weak acid with a pKa of 4.82.Round your answer to 1 decimal place.
Solution
To calculate the pH of a solution of a salt resulting from a weak acid, we can use the formula for the pH of a weak base. This is because the anion of the weak acid will act as a weak base. The formula is:
pOH = 1/2 * (pKa - log[base])
First, we need to calculate the pOH of the solution.
pOH = 1/2 * (4.82 - log[0.86]) pOH = 1/2 * (4.82 + 0.065) pOH = 1/2 * 4.885 pOH = 2.4425
Then, we can find the pH by subtracting the pOH from 14 (since pH + pOH = 14 at 25°C).
pH = 14 - pOH pH = 14 - 2.4425 pH = 11.5575
Rounding to one decimal place, the pH of the solution is 11.6.
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