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13 Dec 2019

Determine the solubility of CuI in 0.42 M KCN solution. The Ksp of CuI is 1.1×10−12 and the Kf for the Cu(CN)−2 complex ion is 1×1024.

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Irving Heathcote
Irving HeathcoteLv2
17 Dec 2019

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Related questions

146. Find the solubility of Cul in 0.40 M HCN solution. The Ksp of Cul is 1.1 x 10-12 and the K for the Cu(CN)2 complex ion is 1 X 1024

A 2.50 g sample of a bronze gong was cut out and dissolved insuklfuric acid. The copper sulfate produced was mixed with KI toform CuI and the triiodide ion, I3-. The I3- ion was then titratedwith thiosulfate, S2O3 2-.

Cu+ 2 H2SO4 -> Cu SO4 + SO2 + 2 H2O
2CuSO4 + 5 I- -> 2 CuI + I3- + 2SO4 2-
I3- + 2S2O3 2- -> 3I- + S4O6 2-

If it took 31.5 mL of 1.00 M thiosulfate for this titration, howmany mols of copper were present in the original 2.50 g sample?

This experiment involved mixing aqueous solutions of Cu(NO3)2(Copper nitrate) and KI (potassium iodide)

2 Cu(NO3)2 (aq) + 4 KI (aq) ---- > 2 CuI (s) + I2 (aq) +4KNO3 (aq)


You have two test tubes labeled A and B. Both test tubes havethe same solution in them. The solution is 2.0 mL of 0.50 MCu(NO3)2 and 5.0 mL of 0.50 M KI. After centrifuging the test tubesfor 5 minutes the preciptate (CuI) settles to the bottom. Thesupernatant is removed from each test tube and then the precipitateis dried. Once it is dry, the precipitate is weighed in each testtube. Test tube A ended up with a precipitate weighing 0.3 gramsand test tube B had a precipitate weighing 0.33 grams.

Given this information, calculate the following:

1.) average moles of product (CuI)


2.) average moles of Cu(NO3)2


3.) average moles of KI


4.) theoretical moles of product based Cu(NO3)2


5.) theoretical moles based on KI


6.) percent error in moles of CuI

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