Question

The Ksp of Ag2SO4 is 1.4 x 10-5. Woud you have expected to obtain precipitate of...

The Ksp of Ag2SO4 is 1.4 x 10-5. Woud you have expected to obtain precipitate of Ag2SO4 in any of the exeriments that you did while determining how you were going to test for chloride ion (Add 6M HNO3 to unknown sample. Test with blue litmus paper, if red, continue. If blue litmus paper stays blue, add more acid. Add a few drops of 0.02M AgNO3. If white precipitate forms, Cl- is present.)? Justify your anwer with a calculation.

Homework Answers

Answer #1

Ag2SO4(s) ---- > 2Ag+(aq) + SO42-(aq),

Ksp = 1.4 x 10-5

if We added 1 one drop (1 mL) of 0.02M AgNO3.

then moles of Ag+(aq) added = 0.02 x 1.0 x 10-3

                                              = 2.0 x 10-5 mol

If the final volume of the solution after addition of sample solution, HNO3 and AgNO3 is 10 mL,

the concentration of [Ag+(aq)] = 2.0 x 10-5 mol / 10 x 10-3 L = 2.0 x 10-3 M

Also the sulphate ion concentration would be of the same order.

Hence ionic product,

IP = [Ag+]2x[SO42-] < Ksp (1.4 x 10-5)

However for precipitation to occur IP (ionic product) should be greater than Ksp.

Hence precipitation will not occur.

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