Calucating the solubility product of Silver Chloride

AI Thread Summary
The discussion revolves around calculating the solubility product (Ksp) of silver chloride (AgCl) after treating it with sodium carbonate (Na2CO3). The remaining solution contained 0.003 g of Cl- per liter, leading to a calculated concentration of Cl- as 8.45 x 10-5 M. Participants discussed the impact of excess carbonate on the solution and how to relate the solubility of Ag2CO3 to the Ksp of AgCl. The final calculation yielded a Ksp of AgCl at 1.073 x 10-8. The relevance of the Na2CO3 concentration and volume was questioned, suggesting further clarification on its role in the reaction.
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Homework Statement


A sample of AgCl was treated with 5ml of 2M Na2CO3 solution to produce Ag2CO3. The remaining solution contained 0.003 g of Cl- per litre. Calculate the solubility product of AgCl.(Ksp of Ag2CO3 = 8.2 ×10-12)

Homework Equations


ksp of AgCl = [Ag+]×[Cl-]
ksp of Ag2CO3 = [2Ag+]2×[CO3--]

The Attempt at a Solution



I couldn't think of any idea. So, entered this forum. Please help.
 
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Can you calculate concentration of Cl-?

There was a huge excess of carbonate. Did it concentration change much?
 
Yes. I calculated the concentration by dividing gm/litre by 35.5 to give molarity. But, I don't know where to go beyond.
 
I asked you a question, have you tried to answer it?
 
I don't know how to start.
 
Try to describe what is happening in the solution when the carbonate is added.
 
I tried this:
Ksp of Ag2CO3 = [2xSolub.]2x[Solub.]
=> Solubility = 1.270334x10-4 = [Ag+]
Now,
[Cl-]=0.003/35.5 M = 8.45 x 10-5
Ksp of AgCl = 1.270334x10-4 x 8.45 x 10-5 = 1.073 X 10-8.

Why was concentration and volume of Na2CO3 was given if this is correct?
 
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