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What is the pH at the equivalence point for the titration of 20.0 mL of 0.500 M acetic acid (HC2H3O2) with 0.350 M potassium hydroxide (KOH), given that the Ka for acetic acid is 1.8 × 10^-5?
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18. Aqueous Equilibrium
Acid-Base Indicators
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What is the pH of a solution after adding 4.3 mL of a strong acid beyond the equivalence point in a titration with a strong base?
A
pH = 7.0
B
pH = 12.0
C
pH = 9.5
D
pH = 2.5
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Identify the strong acid and strong base involved in the titration. Strong acids and bases completely dissociate in water, which simplifies calculations.
Determine the concentration of the strong acid and strong base used in the titration. This information is crucial for calculating the moles of acid and base present.
Calculate the moles of strong acid added beyond the equivalence point using the formula: \( \text{moles} = \text{volume (L)} \times \text{concentration (M)} \).
Since the solution is beyond the equivalence point, calculate the excess moles of strong acid remaining after neutralization by the strong base.
Use the excess moles of strong acid to find the concentration of \( \text{H}^+ \) ions in the solution, and then calculate the pH using the formula: \( \text{pH} = -\log[\text{H}^+] \).
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