Problem: Calculate the solubility of silver chloride in a solution that is 0.160 M in NH3 (initial concentration).

FREE Expert Solution

We’re being asked to calculate the solubility of Silver Chloride (AgCl) in 0.160 M NH3. The presence of NH3 would increase the solubility of AgCl because Ag+ would be consumed to form Ag(NH3)2+(aq)


There are two reactions involved:


Reaction 1:

AgCl (s) ⇌  Ag+(aq)  +   Cl- (aq) 

Ksp = [Ag+][Cl-]  =  1.6x10-10   (you can get the Ksp value in books or the internet)


Reaction 2:

Ag+(aq)  +  2  NH(aq)  ⇌   Ag(NH3)2+ (aq)        A coefficient of 2 is added to NHto balance the reaction.

Kf=[AgNH32][Ag+][NH3]2=1.7×107  (you can get the Kvalue in books or the internet)


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Problem Details

Calculate the solubility of silver chloride in a solution that is 0.160 M in NH3 (initial concentration).

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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.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Shetty's class at Ferris State University.