Using a single reagent and only chemistry that was part of this experiment, how

Question

Using a single reagent and only chemistry that was part of this experiment, how could you distinguish between the following pairs of substances contained in separate test tubes? explain in words how you can tell and give the net-ionic equation for any reaction that occurs in the test.

I believe some of the possible reagents are hot water, HCl, NH3, K2CrO4, or HNO3. These were used to identify Ag+, Pb2+, and Hg22+.....I think the reagents may be a.) ? NH3 ,b.) NH3, and c.) lead? I'm not sure what it's really asking.....

a.) Hg2(NO3)2 and Mg(NO3)2 solutions Reagent :     

b.) Hg2Cl2 and AgCl2 solutions Reagent :   

c.) Na2CrO4 and HCl solutions Reagent :   

Explanation / Answer

a) Hg2Cl2 turns black in color when ammonia solution is poured over it.
Mg(NO3)2 soluble in ammonia solution.

Net ionic equation : Hg2+2(aq) + 2NH3 + H2O ---> [Hg2NCl (H2O)] + 2NH4+(aq) + Hg(s)(Black precipitate)

b) Hg2Cl2 turns black in color when ammonia solution is poured over it.
AgCl soluble in ammonia solution.

Net ionic equation : Hg2+2(aq) + 2NH3 + H2O ---> [Hg2NCl (H2O)] + 2NH4+(aq) + Hg(s)(Black precipitate)

c) Pb+2(aq) + Na2CrO4 (aq) --> PbCrO4(s) + Na+(aq)

Net ionic equation: Pb+2(aq) + CrO4-2 (aq) --> PbCrO4(s)(yellow precipitate)

Pb+2(aq) + 2HCl (aq) --> PbCl2(s) + 2H+(aq)

Net ionic equation: Pb+2(aq) + 2Cl- (aq) --> PbCl2(s).(White precipitate)

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