Question

Please help I have to submit this assignment by today.


When 0.01 M HCl is solution is added to 0.01 M Pb(No3)2 will a precipitate of Pbcl2 be formed or not?
Ksp = 1.6 * 10^ -5

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Answer 1

Precipitation of $PbCl_2$  will not formed.

Explanation:

$HCl(aq)\rightarrow H^+(aq)+Cl^-(aq)$

Concentration of HCl = $[HCl]=0.01 M$

From the reaction :Concentration of chloride ions

$[HCl]=[Cl^-]=0.01M$

$Pb(NO_3)_2(aq)\rightarrow Pb^{2+}(aq)+2NO_3^{-}(aq)$

Concentration of lead nitrate = $[Pb(NO_3)_2]=0.01 M$

From the reaction : the concentration of lead (II) ion:

$[Pb^{2+}]=[Pb(NO_3)_2]=0.01 M$

Solubility product of lead (II)( chloride =$K_{sp}=1.6\times 10^{-5}$

$PbCl_2(aq)\rightleftharpoons Pb^{2+}(aq)+2Cl^-(aq)$

Ionic product of the lead (II) chloride in solution will be given as:

$Q_i=[Pb^{2+}][Cl^-]^2=0.01 M\times (0.01M)^2=1\times 10^{-6}$

$K_{sp}>O_i$( no precipitation)

Hence, precipitation of $PbCl_2$  will not formed.

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