Question

The value of the Solubility Product Constant for lead phosphate is ____________

Answer 1

Answer: The reaction for the $K_{sp}$ value of lead phosphate is given below and the value of solubility product for the same is $3.0\rightarrow 10^{-44}$

Explanation:

Solubility product is defined as the product of concentration of ions present in a solution each raised to the power its stoichiometric ratio. It is expressed as $K_{sp}$

The chemical formula of lead phosphate is $Pb_3(PO_4)_2$

The equation for the hydration of the lead phosphate is given as:

$Pb_3(PO_4)_2(s)+H_2O(l)\rightarrow 3Pb^{2+}(aq.)+2PO_4^{3-}(aq.)$

The solubility product of lead phosphate is $3.0\rightarrow 10^{-44}$. This means that it is highly insoluble in water as the solubility product is very very low.

Hence, the reaction for the $K_{sp}$ value of lead phosphate is given above and the value of solubility product for the same is $3.0\rightarrow 10^{-44}$