Select the two Brønsted-Lowry bases in the following equation: CH₃NH₂(aq) + H₂O(l) ⇌ CH₃NH₃⁺(aq) + OH^-(aq) A)CH₃NH₂and H₂O B)CH₃NH₂and OH^- C)H₂O and OH^- D)CH₃NH₂and CH₃NH₃⁺ E)CH₃NH₃⁺and OH^-

Question

Quizplus · Accepted Answer

In an acid-base reaction, a Brønsted-Lowry acid donates a proton (H+) and a Brønsted-Lowry base accepts a proton. In this equation, the H₂O(l) donates a proton to form OH^-(aq), making it the Brønsted-Lowry acid. The CH₃NH₂(aq) and OH^-(aq) both accept protons, making them both Brønsted-Lowry bases. Therefore, the best choice is B because it includes both of these bases.

Select the Two Brønsted-Lowry Bases in the Following Equation: CH3NH2(aq)

Select the Two Brønsted-Lowry Bases in the Following Equation: CH₃NH₂(aq)