Question

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

Write the reaction that corresponds to this Ksp value.

_______(Aq,S,L) +_______(Aq,S,L) <-------->_______(Aq,S,L) +_______(Aq,S,L)

Ksp values are found by clicking on the "Tables" link.

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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)`

Step-by-step 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)`