Question

A saturated solution of Pb(IO3)2 in pure water has a lead ion concentration of 5.0 x 10-5 Molar. What is the Ksp value of Pb(IO3)2? A. 1.0 x 10-5 Molar B. 5.0 x 10-5 Molar C. 1.0 x 10-13 Molar D. 2.5 x 10-13 Molar E. 5 x 10-13 Molar

Answer 1

E) 5 x 10-13 Molar

Step-by-step explanation:

plato

Answer 2

Option (E) is correct

Step-by-step explanation:

Solubility equilibrium of
`Pb(IO_(3))_(2)` is given as follows-

`Pb(IO_(3))_(2)\rightleftharpoons Pb^(2+)+2IO_(3)^(-)`

Hence, if solubility of
`Pb(IO_(3))_(2)` is S (M) then-

`[Pb^(2+)]=S(M)` and
`[IO_(3)^(-)]=2S(M)`

Where species under third bracket represent equilibrium concentrations

So, solubility product of
`Pb(IO_(3))_(2)` ,
`K_(sp)=[Pb^(2+)][IO_(3)^(-)]^(2)`

Here,
`[Pb^(2+)]=S(M)=5.0* 10^(-5)M`

So,
`[IO_(3)^(-)]=2S(M)=(2* 5.0* 10^(-5))M=1.0* 10^(-4)M`

So,
`K_(sp)=(5.0* 10^(-5))* (1.0* 10^(-4))^(2)=5.0* 10^(-13)`

Hence option (E) is correct