(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

What is the minimum quantity of ammonia which must be added to 1L of a solution in order to dissolve 0.1 mole silver chloride by forming [Ag(NH3)2]+.

Given Ksp- 10^-10 and Kf- 10^8

2. Relevant equations

3. The attempt at a solution

I used the equation (which I derived) s=c^2/(Ksp)(Kf) (assuming almost all amount of AgCl converts to complex and some other approximations)

where s is the solubility of AgCl and c is the concentration of NH3 (both in mol/litre)

I solved and got c as 1 mole.

But answer given is 1.2 mole.

Are my assumptions wrong, or there is some other thing?

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# Homework Help: Solubility Product

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