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Pb(IO(3))(2) is a sparingly soluble salt...

`Pb(IO_(3))_(2)` is a sparingly soluble salt `(K_(sp) = 2.6 xx 10^(-13))`. To `35mL` of `0.15M Pb(NO_(3))_(2)` solution, `15mL` of `0.8M KIO_(3)` solution is added, and a precipiatte of `Pb(IO_(3))_(2)` is formed.
What will be the molarity of `IO_(3)^(Theta)` ions in the solution after completion of the reaction?

A

`0.152`

B

`0.081`

C

`0.41`

D

`0.03`

Text Solution

Verified by Experts

The correct Answer is:
D
`[IO_(3)^(Theta)] = (1.5 "mmol")/((15+35) mL) = 0.03M1`
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