Help with Solubility questions, please!

How would you use the solubility rules to separate the following pairs of ions? In each ease indicate what reagent you would add and write the net ionic equation for the precipitation reaction: (a) lead(II) and copper(II) ions; (b) ammonium and magnesium ions. (c) barium and mercury(I) ions; (d) silver and zinc ions


I appreciate any and all help!
Also, if you have a chance, if you wouldn't mind looking at my other chem question involving Avogadro's constant and moles and whatnot. Please and thank you! :
http://answers.yahoo.com/question/index;_ylt=AvfWnW.NXwbrvyJleAZGoRvty6IX;_ylv=3?qid=20110822144035AARP4TQ

How would you use the solubility rules to separate the following pairs of ions? In each ease indicate what reagent you would add and write the net ionic equation for the precipitation reaction:

http://www.files.chem.vt.edu/RVGS/ACT/no…

1. All common compounds of Group I and ammonium ions are soluble.
2. All nitrates, acetates, and chlorates are soluble.
3. All binary compounds of the halogens (other than F) with metals are soluble, except those of Ag, Hg(I), and Pb. Pb halides are soluble in hot water.)
4. All sulfates are soluble, except those of barium, strontium, calcium, lead, silver, and mercury (I). The latter three are slightly soluble.
5. Except for rule 1, carbonates, hydroxides, oxides, silicates, and phosphates are insoluble.
6. Sulfides are insoluble except for calcium, barium, strontium, magnesium, sodium, potassium, and ammonium.


To separate the ions, one of the ions must form a precipitate with the solution which is added. All nitrates are soluble, so the initial solutions are metallic nitrates.


(a) lead(II) and copper(II) ions; #3 add NaCl to precipitate PbCl2
2 NaCl + Pb(NO3)2 → 2 NaNO3 + PbCl2 ↓

(b) ammonium and magnesium ions. #5 add NaOH to precipitate Mg(OH)2
NaOH + Mg(NO3)2 → 2 NaNO3 + Mg(OH)2 ↓