The base-dissociation constant of ethylamine (C₂H₅NH₂)is 6.4 × 10^-⁴ at 25.0 °C. The [H⁺] in a 1.4 × 10^-² M solution of ethylamine is ________ M.

Question

Quizplus · Accepted Answer

The correct answer is A because the [H+] in a 1.4 × 10^-2 M solution of ethylamine can be calculated using the base-dissociation constant (Kb) and the concentration of the ethylamine solution. The Kb for ethylamine is 6.4 × 10^-4 at 25.0 °C, and the concentration of the ethylamine solution is 1.4 × 10^-2 M. Using the equation Kb = [H+][A-]/[B], where [H+] is the concentration of hydrogen ions, [A-] is the concentration of the conjugate base (ethylamine), and [B] is the concentration of the weak base (ethylamine), we can solve for [H+]. Plugging in the values for Kb and [B], we get: 6.4 × 10^-4 = [H+][1.4 × 10^-2]/[1.4 × 10^-2]. Solving for [H+], we get: [H+] = 3.7 × 4.9 × 10^-12 M.

The Base-Dissociation Constant of Ethylamine (C2H5NH2)is 6

The Base-Dissociation Constant of Ethylamine (C₂H₅NH₂)is 6