Ionization of weak acids and bases
Ionic Equilibrium · Chemistry
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0.1 M NH₃, K_b = 1.8×10⁻⁵. Find [OH⁻], pH. Step 1: [OH⁻] ≈ √(K_b·C) = √(1.8×10⁻⁵ × 0.1) = √(1.8×10⁻⁶) = 1.34×10⁻³ M. Step 2: pOH = −log(1.34×10⁻³) = 2.87. Step 3: pH = 14 − 2.87 = 11.13. Step 4: α = 1.34×10⁻³/0.1 = 1.34% — weak base confirmed. Same K as acetic acid's K_a — NH₃/NH₄⁺ mirror CH₃COOH/CH₃COO⁻.