First slide

Solubility product(KSP)

Question

What is the minimum concentration of SO₄^2– required to precipitate BaSO₄ in a solution containing 1.0 × 10^–4 mole/lit of Ba²⁺ ? (K_sp of BaSO₄ = 4 × 10^–10)

Easy

A

$\large 2\, \times \,{10^{ - 5}}M$
B

$4\, \times \,{10^{ - 10}}M$
C

$4\, \times \,{10^{ - 6}}M$
D

$2\, \times \,{10^{ - 3}}M$

Solution

For precipitation, $\large {K_{IP}} \geqslant {K_{sp}}$
$\large OR\left [ {B{a^{ + 2}}} \right] \times \left[ {SO_4^{ - 2}} \right] = 4 \times {10^{ - 10}}$
$\large \Rightarrow {10^{ - 4}} \times \left[ {SO_4^{ - 2}} \right] = 4 \times {10^{ - 6}}$
$\large \Rightarrow \left[ {SO_4^{ - 2}} \right] = 4 \times {10^{ - 6}}$

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