What is the K_b for methylamine (CH₃NH₂) if a 0.10 M solution of this weak base is 6.8% ionized?

Question

Quizplus · Accepted Answer

The correct answer is A because the Kb for methylamine is 5.0 x 10^-4. This can be calculated using the formula Kb = [OH-]^2 / [CH3NH2], where [OH-] is the concentration of hydroxide ions and [CH3NH2] is the concentration of methylamine. In this case, [OH-] = 0.068 M and [CH3NH2] = 0.10 M, so Kb = (0.068 M)^2 / (0.10 M) = 5.0 x 10^-4.

What Is the Kb for Methylamine (CH3NH2) If a 0

What Is the K_b for Methylamine (CH₃NH₂) If a 0