What is the pH of a 0.380 M aqueous solution of ethylamine?
K_b = 4.3 × 10^-4

Question

What is the pH of a 0.380 M aqueous solution of ethylamine? K_b = 4.3 × 10^-4 A)12.1 B)1.9 C)10.2 D)5.5 E)8.5

Quizplus · Accepted Answer

The correct answer is A because the pH of a 0.380 M aqueous solution of ethylamine can be calculated using the Kb value of ethylamine and the concentration of the solution. The Kb value for ethylamine is 4.3 × 10-4, and the concentration of the solution is 0.380 M. The pH can be calculated using the following equation:pH = 14 - 1/2 pKb - 1/2 log[B]where [B] is the concentration of the base. Substituting the values into the equation, we get:pH = 14 - 1/2 pKb - 1/2 log[0.380]pH = 14 - 1/2 (-log 4.3 × 10-4) - 1/2 log[0.380]pH = 14 - 1/2 (3.37) - 1/2 (-0.42)pH = 14 - 1.68 + 0.21pH = 12.1

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