0.00162 is the Ksp of Ag2CO3 at 10 degrees.
Explanation:
Ag2CO3(s) --- 2Ag+ (aq) + CO3 ^-2(aq)
The product of molar solubility of each ion in moles/litre gives the solubility product.
The molar solubility of Ag2CO3 is 0.074 M at 10 degrees.
From the above reaction we can see that
2 Moles of Ag and 1 mole of carbonate ions,
So, [Ag2CO3]= 2[Ag]^2[CO3^2-]
Ksp of Ag+= 2*0.074
= 0.148
Ksp of CO3^-2= 0.074
= 0.148
Ksp of AgNO3= [0.148]^2 [0.074]
Ksp of AgNO3 = 0.00162 AT 10 degrees
