Chapter 15, Problem 101CP

a. Calculate the molar solubility of AgBr in pure water. K_sp for AgBr is 5.0 × 10⁻¹³.

b. Calculate the molar solubility of AgBr in 3.0 M NH₃. The overall formation constant for Ag(NH₃)₂⁺ is 1.7 × 10⁷, that is,

$\begin{array}{cc}{\text{Ag}}^{\text{+}}(aq)+2N{H}_3(aq)\to Ag{(N{H}_3)}_2{}^{+}(aq)& K=1.7\times {10}^7\end{array}.$

c. Compare the calculated solubilities from parts a and b. Explain any differences.

d. What mass of AgBr will dissolve in 250.0 mL of 3.0 M NH₃?

e. What effect does adding HNO₃ have on the solubilities calculated in parts a and b?