The molar solubility of Ag2CO3 is 0.074M at 10°C.

What is the Ksp of Ag2CO3 at the same degree?

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