Ans :- PbI2 (s) will not form precipitates.
Explanation :-
Overall Reaction is :
2 NaI (aq) + PbS2O3 (aq) ----------------> PbI2 (s) + Na2S2O3 (aq)
From the definition of Molarity as :
Molarity = Number of moles / Volume of solution in L
So,
Number of moles of NaI = Molarity of NaI x Volume of solution
= 0.010 M x 0.010 L
= 0.0001 mol
Similarly,
Number of moles of Pb2+ = Molarity of Pb2+ x Volume of solution
= 0.020 M x 0.250 L
= 0.005 mol
Now,
Total volume becomes = 10.0 ml + 16.0 ml + 250.0 ml = 276 ml = 0.276 L
So,
Molarity of NaI or [I-] in complete solution = 0.0001 mol / 0.276 L = 0.000362 M
Also,
Molarity of Pb2+ or [Pb2+] in complete solution = 0.005 mol / 0.276 L = 0.0181 M
Partial dissociation of PbI2 in solution is :
PbI2 (s) <-------------------> Pb2+ + 2 I-
Expression of reaction quotient (Qsp) for PbI2 is :
Reaction Quotient (Qsp) is the product of the molar concentration of products raise to the power of stoichiometric coefficient with respect to each products species at any stage of the reaction. Solubility product (Ksp) is the product of the molar concentration of products raise to the power of stoichiometric coefficient with respect to each products species at equilibrium stage of the reaction. |
Qsp = [Pb2+].[I-]2
Qsp = (0.0181 M).(0.000362 M)2
Qsp = 2.37 x 10-9 M3
Which is smaller than Solubility product (Ksp) value of PbI2 i.e. 7.1 x 10-9 M3
Therefore, PbI2 (s) will not form precipitates. |
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