First slide

Solubility product(KSP)

Question

Statement I : On mixing 500mL of 10^–6M Ca²⁺ ion and 500 mL of 10^–6MF^-1ion, the precipitate of CaF₂ will be obtained K_sp(CaF₂) = 10^–18
Statement II : If K_sp is more than ionic product, precipitate will be obtained.

Moderate

A

Statement I and II are correct
B

Statement I is correct and Statement II is incorrect
C

Statement - I is incorrect and Statement II is correct
D

Both statement - I and statement - II are False

Solution

Let us calculate the ionic product of CaF₂
$K_{IP} = [{Ca}^{+ 2}] {[F^{-}]}^{2} = (\frac{10^{- 6} \times 500}{1000}) {(\frac{10^{- 6} \times 500}{1000})}^{2}$
$K_{I P} = \frac{1}{8} \times 10^{- 18}$
K_IP < K_sp ⇒ more salt can go into the solution therefore, no precipitate will occur.

Get Instant Solutions

When in doubt download our app. Now available Google Play Store- Doubts App

Recieve an sms with download link

Doubts App

OR

SCAN ME

Doubts App

Doubts App