Question

Calculate the molar solubility of lead thiocyanate in pure water. The molar solubility is the maximum amount of lead thiocyanate the solution can hold.

Answer 1

Answer:

$Molar solubility(S)=1.71\times10^{-2} mole/litre$

Explanation:

Assume Ksp of $Pb(SCN)_{2}$=$2\times10^{-5}$( it is general value ,i took it because not given in question)

molar solubilty means how much maximum mole of lead thiocynate is dissolved in one litre of solvent.

Ksp=solubility product;

$Pb(SCN)_2= Pb^{2+} +2SCN^-$

Lets molar solubilty of $Pb(SCN)_2$ is S then

$[Pb^{+2}]=S;$

$[SCN^{-1} ]=2S;$

$Ksp =S\times(2S)^{2} =2\times10^{-5}$

$4S^{3}=2\times10^{-5}$

$S=1.71\times10^{-2} mole/litre$