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solubility of silver compounds

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Answer the following questions relating to the solubilities of two silver compounds. Ag2CrO4 and Ag3PO4

Silver chronate dissociates in water according to the equation shown below

Ag2CrO4 (s). = 2 Ag+ (aq) + CrO4 2- (aq)
Ksp = 2.6 x 10^-12 at 25C

A) write the equilibrium constant expression for the dissolving of Ag2CrO4 (s)

B). Calculate the concentration , in mol/L , of Ag+ (aq) , in a saturated
solution of Ag2CrO4 at 25C

C) calculate the maximum mass , in grams , of Ag2CrO4 that can dissolve in 100ml
of water at 25C

D) A 0.100 mol sample of solid AgNO3 is added to a 1.00 L saturated solution of
Ag2CrO4. Assuming no volume change does [CrO4 - ] increase , decrease or remain
the same. Justify your answer

In a saturated solution of Ag3PO4 at 25C , the concentration of Ag+ (aq) is 5.3
x 10^-5 M. The equilibrium- constant expression for the dissolving of Ag3PO4 (s)
in water is
Ksp = [Ag+ ] ^3 [PO4 3- ]

E) write the balanced equation for the dissolving of Ag3PO4 (s) in water

F) Calculate the value of Ksp for Ag3PO4 (s) at 25C

G) A 1.00 L sample of saturated Ag3PO4 solution is allowed to evaporate at 25C
to a final volume of 500ml.
What is [ Ag+] in the solution ? Justify your answer

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See Also This Related BrainMass Solution

the solubility of silver phosphate in pure water and Na3PO4

Silver Phosphate, Ag3PO4, is an ionic compound with a solubility product constant Ksp of 206 x 10 ^ - 18. Calculate the solubility of this compound in:

a) pure water

b) 0.2 mol L-1 or 0.2 M Na3PO4

I was able to solve part a, I got the solubility of silver phosphate in water to be 1.76 x 10 ^ -5 M. I am not sure how to solve part b.

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