What is the equilibrium pH of an initially 4.9 M solution of hypoiodous acid, HOI, at 25°C (K_a = $2.3 \times 10 ^ { - 11 }$ ; K_w = 1.01 × 10^-14)?

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Quizplus · Accepted Answer

The equilibrium pH can be calculated using the formula for weak acid dissociation. Given the very small K_a, the concentration of H⁺ ions will be low, leading to a pH close to neutral. Calculating the pH using the formula pH = -log[H⁺] with the given K_a and initial concentration gives a pH of approximately 4.97.

What Is the Equilibrium PH of an Initially 4 2.3×10−112.3 \times 10 ^ { - 11 }2.3×10−11

What Is the Equilibrium PH of an Initially 4 $2.3 \times 10 ^ { - 11 }$