Problem Set – Solubility and Net Ionic Equations
Name:
Chemistry
Period:
Date:
PART I
RF Mandes, PhD, NBCT
SOLUBILITY RULES
Use the attached SOLUBILITY RULES to determine whether each compound is soluble or insoluble. Write
“S” for soluble or “I” for insoluble.
Compound
Solubility
Compound
1
AgNO3
26
LiCH3CO2
2
BaSO4
27
NH4NO3
3
NaCl
28
Mg(ClO3)2
4
K3PO4
29
Na2CO3
5
K2CO3
30
SrSO4
6
Fe(NO3)3
31
NH4Cl
7
K2SO4
32
Na2S
8
NaOH
33
Ca(OH)2
9
MgO
34
KNO3
10
KI
35
BaCO3
11
NaClO4
36
Mg(NO3)2
12
FeS
37
Na2O
13
AgCl
38
FeCO3
14
Na2SO4
39
NH4OH
15
Sn(NO3)2
40
CaPO4
16
MgBr2
41
KClO4
17
CuO
42
Li2SO4
18
NH4ClO3
43
NH4C2O4
19
KOH
44
AgBr
20
Mg(CH3CO2)2
45
K2CrO4
21
PbI2
46
Ba(OH)2
22
Li2CO3
47
CuNO3
23
CaSO4
48
PbSO4
24
Pb(NO3)2
49
CaCl2
25
Fe2O3
50
KClO3
Solubility
Problem Set – Solubility and Net Ionic Equations
PART II NET IONIC EQUATIONS
DIRECTIONS: Follow these steps and the example to complete #1-5.
1st
2nd
3rd
4th
5th
6th
generally
Dissociate (separate) the reactants into individual ions because they are dissolved in water.
Switch partners, but keep them as ions.
Write the new formulas.
U se the attached Solubility Rules to Determine which compounds are soluble or insoluble
Write soluble compounds as ions and insoluble as formulas in the ionic equations
Cancel any substances present as both a reactant and product and write what remains as the net ionic equation
A bB a
+
C dD c
→
A dD a
ê1st
Aa+ + Bb-
CbBc____
é3rd
Cc+ + Dd-
+
+
è2nd
Aa+ + Dd-
+
Cc+ + Bb-
This example follows the general outline above, and steps #1-6 to complete problems #1-5
example:
Na2CO3
+
BaCl2
→
NaCl
ê
Na1+ + CO32-
+
BaCO3
é
+
Ba2+ + Cl1-
è
Na1+ + Cl1-
+
Ba2+ + CO32-
Reactants and 1st product are determined to be soluble and so are written as ions.
2nd product is determined to be insoluble and so are written as an empirical formula
ionic eq:
Na1+ + CO32- + Ba2+ + Cl1- → Na1+ + Cl1- + BaCO3
net ionic eq:
CO32- + Ba2+
1.
+
AlBr3
K 2S
→
BaCO3
→
ê
+
é
+
è
+
→
+
ionic eq:
net ionic eq:
2.
FeCl3
+
AgNO3
ê
+
ionic eq:
net ionic eq:
é
è
+
Problem Set – Solubility and Net Ionic Equations
3.
(NH4)2SO4
+
Ca(OH)2
→
ê
+
é
+
è
+
→
+
ionic eq:
net ionic eq:
4.
CaCl2
+
K2CO3
ê
é
+
è
+
→
+
ionic eq:
net ionic eq:
5.
PbNO3
+
MgI2
ê
+
ionic eq:
net ionic eq:
é
è
+
Problem Set – Solubility and Net Ionic Equations
RULE 1: SOLUBLE COMPOUNDS
Soluble Compounds
Exceptions to the Rule
Compound with these anions are soluble and dissociate
into ions
These are exceptions to the rule. When these cations
are bonded to the selected anion the compound is
insoluble and is written as an empirical formula.
This is the only rule written for cations instead of anions.
Salts containing alkali metal ions and the ammonium ion,
NH41+, are soluble*.
Compounds with the anion:
nitrate, NO31chlorate, ClO31perchlorate, ClO41acetate, CH3CO21Compounds with the halides, Cl1-, Br1-, or I1-
Halides of Ag1+, Hg22+, and Pb2+
Compounds containing fluoride, F1-
Fluorides of Mg2+, Ca2+, Sr2+, Ba2+, and Pb2+
Compounds containing sulfate, SO42-
Sulfates of Ca2+, Sr2+, Ba2+, and Pb2+
RULE 2: INSOLUBLE COMPSOUNDS
Insoluble Compounds
Exceptions
Compounds with these anions are insoluble and so are
written as empirical formulas
These are exceptions to the rule. When these cations
are bonded to the selected anion the compound is
soluble and is dissociated into ions.
All compounds with the anion:
carbonate, CO32-
Compounds of NH41+ and the alkali metal cations*.
phosphate, PO43oxalate, C2O42chromate, CrO42Most metal sulfides, S2-
Compounds of NH41+ and the alkali metal cations*.
most metal hydroxides, OH1-, and oxides, O2-
Compounds of NH41+ and the alkali metal cations*.
*NOTE: The Alkali Metal Cations are the Group 1 elements with a 1+ charge: Li1+, Na1+, K1+, Rb1+, Cs1+