First slide

Solubility product(KSP)

Question

The addition of NaCl to AgCl decreases the solubility of AgCl because

Difficult

A

solubility product decreases
B

solubility product remains constant
C

solution becomes unsaturated
D

solution becomes supersaturated

Solution

$AgCl ⇌ {Ag}^{+} + {Cl}^{-} - - - (1)$
After addition of NaCl , $NaCl ⇌ {Na}^{+} + {Cl}^{-} - - - (2)$
The Concentration of Cl^- increases and equilibrium shifts in the backward direction (acc. to Lechatlier's principle)
So, solubility of AgCl decreases and solubility product remains same.
$K_{sp} = [{Ag}^{+}] [{Cl}^{-}]$
Because of common ion effect(increased concentration of Cl^-)
$∴ K_{sp} < [{Ag}^{+}] [{Cl}^{-}]$
Hence the solution is a supersaturated solution.

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