Chem.I Worksheet: Ionic Reactions. Block: ____ Name: ____________________________
Solubility Rules.
1. All salts containing ions of Group IA, NH4+, NO3-, C2H3O2- (acetate ion), or ClO3- ARE SOLUBLE.
2. Salts of Cl-, Br-, or I- ARE SOLUBLE, EXCEPT with Ag+, Cu+, Hg22+, or Pb2+.
3. Salts of SO42- ARE SOLUBLE, EXCEPT with Pb2+, Ca2+, Sr2+, Ba2+, or Ra2+.
4. Salts of OH- and S2- ARE NOT SOLUBLE, EXCEPT for Rule 1, or Ca2+, Sr2+, Ba2+ or Ra2+.
5. Salts of O2-, CO32-, PO43-, SO32-, CrO42-, and SiO42- ARE, NOT SOLUBLE,, EXCEPT for Rule I.
1. Based upon the above rules, predict whether each of the compounds listed is soluble (aq) or insoluble (s).
a. K2CO3 ____ b. CaSO4 ______ c. AgNO3 ______ d. MnPO4 _____ e. PbI2 ______ f. (NH4)2SO3 _____
g. Ca(OH)2 _____ h. Pb(C2H3O2)2 _____ i. AgI _____ j. Na2SiO4 _____ k. FeSO4 _____ m. WC14 _____
2. When the following ionic substances dissolve (however little) in water, into what ions will they dissociate?
a. NH4Cl =>__________________ b. K2CrO4 =>__________________ c. Fe(OH)2 =>_________________
d. Co(C2H302)2 =>__________________ e. SnSO4 =>__________________
f. CaCl2 =>__________________ g. KSCN =>__________________ h. NaOH =>__________________
3. For each of the following double replacement reactions occurring in water solution, write 3 balanced
equations: one in “molecular” form , one in ionic form and one in net (ionic equation) form (leaving out
spectator ions). Remember that in ionic forms insoluble materials (precipitates) must be written in molecular
form. For example:
Molecular: 1 NaCl (aq) + 1 AgNO3 (aq) => 1 NaNO3 (aq) + 1 AgCl(s) (See solubility rules for why AgCl is (s))
Ionic: 1 Na+(aq) + 1 Cl-(aq) + 1 Ag+(aq) + 1 NO3-(aq) => 1 AgCl (s) + 1 Na+(aq) + 1NO3-(aq)
Net Ionic: 1 Ag+(aq) + 1 Cl-(aq) => 1 AgCl (s)
a.
KI
+
b.
CaCl2
c.
Fe2(SO4)3
Pb(Cl03)2
+
=>
(NH4)3PO4
+
Ba(OH)2
=>
=>