A 0.050 M solution of the weak acid HA has [H₃O⁺] = 3.77 × 10^-4 M. What is the K_a for the acid?

Name: A 0.050 M solution of the weak acid HA has [H 3 O + ] = 3.77 × 10 -4 M. What is the K a for the acid?
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Quizplus · Accepted Answer

The K_a is calculated using the formula K_a = [H₃O⁺][A^-]/[HA]. Assuming [H₃O⁺] = [A^-] and [HA] ≈ initial concentration - [H₃O⁺], K_a = (3.77 × 10^-4)² / (0.050 - 3.77 × 10^-4) ≈ 2.8 × 10^-6 M.

A 0050 M Solution of the Weak Acid HA Has [H3O+]

A 0050 M Solution of the Weak Acid HA Has [H₃O⁺]