The solubility of lead chromate is 4.5×10^-5. Calculate the solubility product of this compound

1 answer

The solubility product (Ksp) of lead chromate (PbCrO4) can be calculated using the following equation:

Ksp = [Pb2+][CrO42-]

where [Pb2+] is the concentration of lead ions and [CrO42-] is the concentration of chromate ions.

Since the solubility of lead chromate is given as 4.5×10^-5, we can assume that the concentration of lead ions and chromate ions in equilibrium is also 4.5×10^-5. Therefore:

[Pb2+] = 4.5×10^-5 M
[CrO42-] = 4.5×10^-5 M

Substituting these values into the equation for Ksp:

Ksp = (4.5×10^-5)(4.5×10^-5) = 2.025×10^-9

Therefore, the solubility product of lead chromate is 2.025×10^-9.