For this problem, we’re being asked to calculate the molar solubility (in mol/L) of AgCl(s) in 3.0 M NH3.
• Since the AgCl ionic, it will form ions when dissociating in a solution. The dissociation of AgCl in a solution is as follows:
AgCl(s)⇌ Ag+(aq) + Cl–(aq) Ksp = 1.8x10-10
Note that each concentration is raised by the stoichiometric coefficient: both [Ag+] and [Cl-] are raised to 1. Also, solids are ignored in Ksp expression.
Calculate the molar solubility of AgCl (K sp = 1.8 x 10 -10 at 25 degrees C) in 3.0 M NH3
Ag+(aq) + 2NH3(aq) ⇌ Ag(NH3)2+(aq)
Kf = 1.6 x 107
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Formation Constant concept. If you need more Formation Constant practice, you can also practice Formation Constant practice problems.