Answer:
[tex]Sr_3(PO_4)_2(s)\rightleftharpoons 3Sr^{+2}(aq)+2(PO_4)^{-3}(aq)[/tex]
[tex]Ksp=[Sr^{+2}]^3[(PO_4)^{-3}]^2[/tex]
Explanation:
Hello,
In this case, for strontium phosphate, we find an ionic equation for its dissociation as shown below:
[tex]Sr_3(PO_4)_2(s)\rightleftharpoons 3Sr^{+2}(aq)+2(PO_4)^{-3}(aq)[/tex]
Next, the solubility product is found by applying the law of mass action, considering that the solid salt is not considered but just the aqueous species due to heterogeneous equilibrium:
[tex]Ksp=[Sr^{+2}]^3[(PO_4)^{-3}]^2[/tex]
Best regards.
