Define the common ion effect in terms of the solubility of compounds. The ion pr

Question

Define the common ion effect in terms of the solubility of compounds. The ion present in water which is in common with the ions present in the dissolved salt is called common ion. Due to the presence of a common ion the solubility of the solid will be reduced. A solution is prepared by adding 750.0 mL of 4.00 times 10-3 M Ce(NO3)3 to 300.0 mL of 2.00 times 10-2 M K103 Will Ce(103)3 (Ksp = 19 times 10-10) precipitate from this solution? A solution contains 1.0 times 10-4 M Cu+ and 2.0 times 10-3 M Pb2+. If a source of I- is added gradually to this solution, will Pbl2 (Ksp = 1.4 times 10-8) or Cul (Ksp = 5 3 times 10-12) precipitate first? Specify the concentration of 1- necessary to begin precipitation of each salt.

Explanation / Answer

Ans:

6) Step-I: Calculate the no of moles of ions as follows

No of moles of Ce+3 in 750 ml is =(750/1000)*0.004 =3 X 10-3 moles

No. of moles of IO3- in 300 ml is = (300/1000)*0.02 = 6 X 10-3 moles

Total volume of solution is = 750+300=1050ml =1.05L

StepII: Calculate concentrations of ions per 1.05L

[Ce+3] = (0.003/1.05) = 2.85 X 10-3

[IO3-] = (0.006/1.05) = 5.71 X 10-3

StepIII: Ce(NO3)3 + 3KIO3 ======> Ce(IO3)3 +3KNO3

Ionic product = [Ce+3] [IO3]3

= [2.85 X10-3] [5.71 X 10-3] 3

   = 9.85 X 10-17

Here Ksp =1.9 x 10-10 and ionic product is 9.85 X 10-17

So Ionic product is less than Solubility product, no precipitation of Ce(IO3)3

Similarly solve Problem 7 also

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