Chapter 4.3 Precipitation Reactions

Question 1

Soluble Ionic Compounds Rules (4)

Answer 1

1. All common compounds of Group 1A ions and Ammonium ion are soluble
2. All common Nitrates, Acetates, and most Perchlorates are soluble (NO3^-, CH3COO^-, ClO4^-
3. All common Chlorides, Bromides, and Iodides are soluble EXCEPT those of Ag+, Pb+2, Cu+, and Hg2^+2 (Silver, Lead, Copper, and Mercury)
4. All common sulfates (SO4^-2) are soluble, EXCEPT those of Ca+2, Sr+2, Ba+2, Ag+2, and Pb+2 (Calcium, Strontium, Barium, Silver, and Lead)

Question 2

Insoluble Ionic Compounds Rules (3)

Answer 2

1. All common metal hydroxides are insoluble EXCEPT those of Group 1A and the larger members of Group 2A (beginning a/ Ca+)
2. All common carbonates (CO3^-2) and phosphates (PO4^3) are insoluble, EXCEPT those of Group 1A and NH4^+
3. All common sulfides are insoluble EXCEPT those of Group 1A, Group 2A and NH4^+)

Question 3

Steps to predict if a precipitate will form when mixing two aqueous ionic solutions (3)

Answer 3

1. Note the ions in the reactants
2. Consider all possible Cation-Anion combinations
3. Decide whether any combination is insoluble

Question 4

Metathesis (Double-Displacement Reactions)

Answer 4

reactions that show the ions exchanging partners