What is the molar concentration of Ag⁺(aq) in a 1.00 M solution of Ag(NH₃) ₂⁺with no excess ammonia?
Given: K_f = 1.70 * 10⁷ for Ag(NH₃) ₂⁺.

Question

What is the molar concentration of Ag⁺(aq) in a 1.00 M solution of Ag(NH₃)₂⁺with no excess ammonia? Given: K_f = 1.70 * 10⁷ for Ag(NH₃)₂⁺.

Quizplus · Accepted Answer

The correct answer is A because the molar concentration of Ag+(aq) in a 1.00 M solution of Ag(NH3)2+(aq) with no excess ammonia can be calculated using the dissociation constant Kf for the complex ion Ag(NH3)2+. The Kf value is 1.70 * 10^7, which means that the equilibrium constant for the dissociation reaction Ag(NH3)2+(aq) <=> Ag+(aq) + 2 NH3(aq) is 1.70 * 10^7. This means that at equilibrium, the concentration of Ag+(aq) will be much lower than the concentration of Ag(NH3)2+(aq). Using the ICE table, we can calculate the concentration of Ag+(aq) to be 2.45 * 10^-3 M.

What Is the Molar Concentration of Ag+(aq) in a 1

What Is the Molar Concentration of Ag⁺(aq) in a 1