Question

Which of the following reactions would occur to a measurable extent in water?

NH_4^+(aq) + H_2O(I) ---> NH_3(aq) + H_3O^+(aq)
Cl^-(aq) + H_2O(l) ---> HCI(aq) + OH^-(aq)
F^-(aq) + H_2O(l) ---> HBr(aq) + OH^-(aq)
Br^-(aq) + H_2O(l) ---> HBr(aq) + OH^-(aq)

Answer 1

The reaction NH4+(aq) + H2O(l) → NH3(aq) + H3O+(aq) would occur to a measurable extent in water.

Step-by-step explanation:

The reaction that would occur to a measurable extent in water is NH4+(aq) + H2O(l) → NH3(aq) + H3O+(aq).

In this reaction, the NH4+ ion acts as an acid, donating a proton to water to form NH3 and H3O+. The equilibrium constant, Ka, for this reaction is greater than 1, indicating that the reaction occurs to a measurable extent in water.

The other reactions listed do not occur to a measurable extent in water. HCl is a strong acid and does not undergo significant base hydrolysis. The reactions involving F- and Br- do not result in the formation of HBr and OH-.

Answer 2

The reaction among the choices that would occur to a measurable extent in water is the acid-base reaction involving ammonium ions and water, resulting in ammonia and hydronium ions.

Step-by-step explanation:

The reaction that would occur to a measurable extent in water is NH4+(aq) + H2O(l) → NH3(aq) + H3O+(aq). This is because the ammonium ion (NH4+) is the conjugate acid of ammonia (NH3), which is a weak base, and its reaction with water will result in the formation of NH3 and hydronium ions (H3O+). The chloride ion, on the other hand, is the conjugate base of hydrochloric acid, a strong acid, so its reaction with water is negligible and doesn't occur to an appreciable extent.