A weak base BOH has Kb = 1.8 × 10⁻⁵. pH of 0.1 M solution is approximately:
A9
B11
C3
D8
Answer & Solution
Correct answer: B. 11
[OH-] ≈ √(Kb × C) = √(1.8 × 10⁻⁶) ≈ 1.34 × 10⁻³. pOH = -log(1.34 × 10⁻³) ≈ 2.87. pH = 14 - 2.87 ≈ 11.13.
Related questions
For the dissociation of a weak acid HA, the degree of dissociation α is given (approximateAccording to Brønsted-Lowry, an acid is a substance that:If Q (reaction quotient) > K_c at some instant, the reaction will:Le Chatelier's principle states that a system at equilibrium under stress:K_sp of a sparingly soluble salt AB at 25 °C is 4 × 10⁻¹⁰. Molar solubility s of AB is:A buffer solution is most resistant to pH change when:K_w (ionic product of water at 25 °C) is:The pH of a 0.01 M HCl solution is: