[Joniaguis]

What would be the solubility of silver chromate in 0.04M silver nitrate solution?
The answer should be expressed in mg/l of silver.

Ksp of silver chromate is 1.0985x10^-12


My answer is 11.69mg/L of Ag. I don't know if it's good

[AWK]

too much !!

Show your attempt

[Joniaguis]

Ksp = [2s+0.04]²
s = 6.9x10^-5M

Therefore 6.9x10^-5M x 332 = 21.57mg/L

21.57mg/L x (180/332) = 11.69mg/L of Ag

[AWK]

Ksp = [Ag⁺]²[CrO₄^2-]
You have an external and quite high concentration of Ag⁺, hence solubility of silver chromate can be approximated by a concentration of chromate anion. Can you now calculate it?

[Joniaguis]

Yes I know that the solubility is calculated by finding the solubility of the chromate anion. But is this equation correct:

Ksp=(2s + 0.04) (s)


And if it is correct, how would you give the answer in terms of silver? By multiplying by (180/332)??

Thanks

[AWK]

Yes I know that the solubility is calculated by finding the solubility of the chromate anion. But is this equation correct:

Ksp=(2s + 0.04) (s)


And if it is correct, how would you give the answer in terms of silver? By multiplying by (180/332)??

Thanks

Your equation is correct for pure water solutions only. Just rearrange the equation given by me previously

[Joniaguis]

I've got an answer of 1.116x10^-7mg/l of Ag

Is it correct?