What is the pH of a buffer solution that consists of 0.83 M HBrO and 0.53 M KBrO?
K _a(HBrO) = 2.3×10^{- 9}

Question

What is the pH of a buffer solution that consists of 0.83 M HBrO and 0.53 M KBrO? K _a(HBrO) = 2.3×10^{- 9}

Quizplus · Accepted Answer

The pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the base form (KBrO in this case), [HA] is the concentration of the acid form (HBrO), and pKa is the negative logarithm of the acid dissociation constant (Ka). Given Ka = 2.3×10^-9, pKa = -log(2.3×10^-9) = 8.64. Plugging in the given concentrations, pH = 8.64 + log(0.53/0.83) = 8.64 - 0.19 = 8.45.

What Is the PH of a Buffer Solution That Consists