Answers: 3
and 0.0390 M 
. What will be the concentration of 
(aq) when 
begins to precipitate? What percentage of the 
![[Ag^{+}]](/tpl/images/0526/4790/52db7.png)
= 0.0390 M
precipitates then expression for 
will be as follows.![K_{sp} = [Ag^{+}]^{2}[SO^{2-}_{4}]](/tpl/images/0526/4790/4148c.png)
![1.20 \times 10^{-5} = (0.0390)^{2} \times [SO^{2-}_{4}]](/tpl/images/0526/4790/e9f5a.png)
![[SO^{2-}_{4}]](/tpl/images/0526/4790/a4a68.png)
= 0.00788 M
![K_{sp} = [Ca^{2+}][SO^{2-}_{4}]](/tpl/images/0526/4790/0d847.png)
![4.93 \times 10^{-5} = [Ca^{2+}] \times 0.00788](/tpl/images/0526/4790/02a50.png)
![[Ca^{2+}]](/tpl/images/0526/4790/17576.png)
= 0.00625 M
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Sodium sulfate is slowly added to a solution containing 0.0500 M Ca 2 + ( aq ) and 0.0390 M Ag + ( a...
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