# The solubility product of a soluble salt A_(x)B_(y) is given by: K_(SP)= [A^(y+)]^(x) [B^(x-)]^(y). As soon as the product of concentration of A^

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The solubility product of a soluble salt A_(x)B_(y) is given by: K_(SP)= [A^(y+)]^(x) [B^(x-)]^(y). As soon as the product of concentration of A^(y+) and B^(x-) increases than its K_(SP), the salt start precipitation. It may practically be noticed that AgCI is more soluble in water and its solublity decreases dramatically in 0.1M NaCI or 0.1M AgNO_(3) solution. It may therefore be conncluded that in presence of a common ion, the solubiolity of salt decreases.
Equal volumes of two solutions are mixed. The one in which CaSO_(4) (K_(SP)= 2.4xx10^(-5)) is precipitated, is :
A. 0.02M CaCI_(2)+0.0004M Na_(2)SO_(4)
B. 0.01M CaCI_(2)+0.0004M Na_(2)SO_(4)
C. 0.02M CaCI_(2)+0.0002M Na_(2)SO_(4)
D. 0.03M CaCI_(2)+0.004M Na_(2)SO_(4)

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[Cu^(2+)][SO_(4)^(2-)]= (0.03xxV)/(2V)xx[(0.004xxV)/(2V)]
=3xx10^(-5)gt K_(SP)`
Thus precipitation.