What is the actual concentration of the molecular form of HF in a 1.0 M HF solution given that K_a of HF is 6.8 $\times$ 10^-4?

Question

Quizplus · Accepted Answer

The actual concentration of the molecular form of HF can be calculated using the equation: [H2F2] = [HF] / (1 + (K_a / [HF])) Plugging in the given values, we get: [H2F2] = 1.0 M / (1 + (6.8 x 10^-4 / 1.0 M)) [H2F2] = 1.0 M / (1 + 6.8 x 10^-4) [H2F2] = 1.0 M / 1.00068 [H2F2] = 0.997 M Therefore, the actual concentration of the molecular form of HF is 0.997 M, which is closest to choice B (0.97 M).

What Is the Actual Concentration of the Molecular Form of HF