For a buffer solution containing weak acid HA and its salt NaA, the pH is approximately:
ApKa
BpKa - log([salt]/[acid])
CpH = 7
DpKa + log([salt]/[acid])
Answer & Solution
Correct answer: D. pKa + log([salt]/[acid])
Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]) = pKa + log([salt]/[acid]). Buffer resists pH change on adding small amounts of acid or base.
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: