Question

Review equation 16.10 and step B2. Ag+1(aq) and NH3(aq) will form a soluble complex ion. Use rule 3 of Water-Insoluble Salts in Appendix E to determine what would happen if Ag+1(aq) was combined with KOH instead of NH3. Write the net ionic equation with phase subscripts, where K+1 is a spectator ion which is cancelled out.

Equation 16.10:

Ag^+(aq) + Cl^-(aq) ⇄ AgCl(s)

⇅ 2NH3(aq)

[Ag(NH3)2]^+(aq)

Step B2:

Silver Chloride equilibrium. To the clear solution from part B.1, add 5 drops of 0.1 M HCL. Add drops of conc NH3 until evidence of a chemical change. Reacidify the solution with 6M HNO3 and record your observations.

Answer 1

The OH⁻ ions convert the silver ion into silver oxide, Ag₂O, which precipitate from the solution as a brown solid:

2 AgCl + 2 KOH → Ag₂O (s) + 2 KCl + H₂O

2Ag⁺ + 2 OH^-   ---> Ag₂O + H₂O​

step B2 ; on adding HCl to a clear solution will form AgCl . further on adding ammonia brown ppt of silver oxide is formed which on further addition of ammonia dissolves to form a complex of silver amine