Aqueous solutions of ammonia (NH₃)and hydrogen cyanide (HCN)react to produce ammonium cyanide,(NH₄CN)according to the following equilibrium reaction. NH3(aq)+ HCN(aq)D NH₄⁺(aq)+ CN−(aq) Given the following equilibrium constants,which statement best describes the reaction once equilibrium is established? (K_w = 1.01 × 10^-14) NH₄⁺ K_a = 5.6 × 10^-10 HCN K_a = 4.0 × 10^-10

Question

Quizplus · Accepted Answer

The reaction is reactant favored because the equilibrium constants for the dissociation of ammonium (Ka = 5.6 × 10^-10) and HCN (Ka = 4.0 × 10^-10) are both significantly smaller than the Kw (1.01 × 10^-14), indicating that the formation of NH4+ and CN- ions is not favored, thus favoring the reactants.

Aqueous Solutions of Ammonia (NH3)and Hydrogen Cyanide (HCN)react to Produce

Aqueous Solutions of Ammonia (NH₃)and Hydrogen Cyanide (HCN)react to Produce