Calculate the pH of a solution that is 0.240 mol L^-1 in nitrous acid ( $\mathrm { HNO } _ { 2 }$ )and 0.320 mol L^-1 in potassium nitrite ( $\mathrm { KNO } _ { 2 }$ ).The acid dissociation constant of nitrous acid is 4.50 × $10 ^ { - 4 }$ . A)12.885 B)4.461 C)3.222 D)10.528 E)3.472

Question

Quizplus · Accepted Answer

The solution is a buffer, and the pH can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]). Here, pKa = -log(4.50 × 10^-4) = 3.347, [A-] = 0.320, and [HA] = 0.240. Thus, pH = 3.347 + log(0.320/0.240) = 3.472.

Calculate the PH of a Solution That Is 0 HNO2\mathrm { HNO } _ { 2 }HNO2​

Calculate the PH of a Solution That Is 0 $\mathrm { HNO } _ { 2 }$