The K_f for the complex ion Ag(NH₃)₂⁺ is 1.7 $\times$ 10⁷.The K_sp for AgCl is 1.6 $\times$10^-¹⁰.Calculate the molar solubility of AgCl in 1.0 M NH₃. A)5.2 $\times$10^-² B)4.7 $\times$ 10^-² C)2.9 $\times$ 10^-³ D)1.3 $\times$ 10^-⁵ E)1.7 $\times$ 10^-¹⁰

Question

Quizplus · Accepted Answer

The presence of NH3, a complexing agent, increases the solubility of AgCl by forming a complex ion with Ag+. The formation constant (Kf) for Ag(NH3)2+ is given as 1.7 × 10^7. The solubility product (Ksp) for AgCl is 1.6 × 10^-10. The molar solubility of AgCl in 1.0 M NH3 can be calculated using the formula involving both Ksp and Kf, leading to an increased solubility compared to pure water. The correct calculation considering the complex formation and the given concentrations leads to the solubility value provided in choice B.

The Kf for the Complex Ion Ag(NH3)2+ Is 1 ×\times× 107 ×\times×

The K_f for the Complex Ion Ag(NH₃)₂⁺ Is 1 $\times$ 10⁷ $\times$