1. Describe the process by which Ag+ ions are precipitated out of solution. 2. A

Question

1. Describe the process by which Ag+ ions are precipitated out of solution.
2. A disproportion reaction occurs when NH3 solution reacts with Hg2Cl2. Write a balancedreaction equation for this event.
3. Write half-reactions that show how H2O2 can act as either an oxidizing agent or a reducingagent, and describe where each of these situations occurred in your testing.
4. In your testing, several precipitates are formed, and then dissolved as complexes. Select threeof these situations for which to write a balanced reaction equation.
5. When Mn2+ ions are separated from the mixture, they go through a series of oxidizing andreducing steps. Write the reaction equations that describe this process.
6. The NH3 solution is used, in three separate instances, to separate two ions. In each of thesecases, one ion forms a precipitate and the other ion remains in solution as a complex.Describe each of these instances, using reaction equations.
7. Al3+ and Zn2+ ions are amphoteric. Describe how the amphoteric nature of these ions isshown in your testing.

Explanation / Answer

1. Ag+ can be precipitated out by adding chloride (Cl-) ions to the solution. We can add NaCl soultion to the Ag+ solution. A precipitate of AgC will be formed by this

Ag+ + NaCl --> AgCl (s) + Na+

2. When Hg2Cl2 is treated with aqueous NH3 disproportionation occurs:

Hg2Cl2 first dissociate into HCl2 and Hg metal
Hg2Cl2 ? HgCl2 + Hg

Then Hg2Cl2 reacts with ammonia:
HgCl2 + 2NH3 ? [Hg(NH3)2Cl2]

Which dissociate as
[Hg(NH3)2Cl2] ? [Hg(NH2)Cl] + NH4Cl

The salt may further react with water to give

[Hg(NH2)Cl] + H2O ? [Hg2NCl (H2O)] + NH4Cl

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