Problem: Kf for the complex ion Ag(NH3)2+ is 1.7 X 107. Ksp for AgCl is 1.6 X 10 -10. Calculate the molar solubility of AgCl in 1.0 M NH3.

🤓 Based on our data, we think this question is relevant for Professor Carlon's class at UCB.

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Step 1:

Step 2:

AgCl (s)  Ag+ (aq) + Cl- (aq)

Ksp = [Ag+][Cl-]

Ag+ (aq) + 2 NH3+ (aq)  [Ag(NH3)2+] (aq)

Kf =[AgNH32+][Ag+][NH3]2

AgCl (s) + NH3 (aq)  Cl- (aq) + Ag(NH3)2+ (aq)

K = [AgNH32+][Cl-][NH3]2K = Ksp×Kf =[Ag(NH3)2+][Cl-][NH3]2


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Problem Details

Kf for the complex ion Ag(NH3)2+ is 1.7 X 107. Ksp for AgCl is 1.6 X 10 -10. Calculate the molar solubility of AgCl in 1.0 M NH3.

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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 Carlon's class at UCB.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.