HCI, NH3, K2CrO4, and HNO3 were used in my lab to identify the presence of Ag, P

Question

HCI, NH3, K2CrO4, and HNO3 were used in my lab to identify the presence of Ag, Pb2+, and hg2 2+.

Please help on #3. what are the reagants, and what is the net ionic equation. Please include states! and color if possible like yellow precitipitate for pbcro4 Name Jsing a single reagent and only reaction chemis how could you distinguish between the following pairs of substances contained in separate test tubes? Explain in words how you could tell, and give the net-ionic equation for any reaction that occurs in the test. 3. b. PbCl, and AgCl solids Reagent: HNO, and HCl solutions Reagent: c. A student has an unknown solution that can contain any combination of Groug I cations. A white precipitate (P1) forms when excess 6 M HCI is added t the unknown. After discarding the supernate (S1), hot water is added to th precipitate (P1I) and the mixture boiled for 5 minutes. Afer removing the mis hath, it is left at room temperature for 10 minutes befor (D2) S2 give

Explanation / Answer

(a)

By adding HCl , Pb2+ forms a white precipitate of PbCl2 but not Ca2+.

Pb(NO3)2 (aq.) + 2 HCl (aq.) ----------> PbCl2 (s) + 2 HNO3 (aq.)

Complete ionic equation:

Pb2+ (aq.) + 2 NO3- (aq.) + 2 H+ (aq.) + 2 Cl- (aq.) ------> PbCl2 (s) + 2 H+ (aq.) + 2 NO3- (aq.)

Net ionic equation:

Pb2+ (aq.) + 2 Cl- (aq.) ----------> PbCl2 (s)

(b)

By ammonia solution, AgCl solid gets dissolved but not PbCl2.

AgCl (s) + 4 NH3 (aq.) ---------> [Ag(NH3)4]Cl (aq.)

Net ionic equation:

AgCl (s) + 4 NH3 (aq.) ----------> [Ag(NH3)4]+ (aq.) + Cl- (aq.)

(c)

By adding AgNO3, HCl forms a white precipitate of AgCl but not HNO3

HCl (aq.) + AgNO3 (aq.) ----------> AgCl (s) + HNO3 (aq.)

Complete ionic equation:

H+ (aq.) + Cl- (aq.) + Ag+ (aq.) + NO3- (aq.) ------> AgCl (s) + H+ (aq.) + NO3- (aq.)

Net ionic equation:

Cl- (aq.) + Ag+ (aq.) ----------> AgCl (s)

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