Problem Set – Solubility and Net Ionic Equations - #2
Name:
Chemistry
Period:
Date:
RF Mandes, PhD, NBCT
DIRECTIONS: Follow these steps and the example to complete #1-5.
1st
2nd
3rd
4th
5th
6th
Dissociate the reactants into individual ions (dissociate regardless of solubility, the goal is to create a vertical pair).
Switch partners, but keep them as ions. Do not change anything. Just write each cation with the other anion.
Write the new formulas.
Determine the solubility of the reactants and products, and circle the appropriate form – ions or empirical formula
Write a chemical equation with the reactants and products in their appropriate form (the one you circled)
Cancel any substances present as both a reactant and product (called spectator ions) and write what remains as the
net ionic equation
EXAMPLE
This example follows the general outline above, and steps #1-6 to complete problems #1-5
Steps 1st, 2nd, 3rd
Na2CO3
+

BaCl2
NaCl
1st
Na1+ + CO32-
+
+
BaCO3
3rd
Ba2+ + Cl1-
2nd
Na1+ + Cl1-
+
Ba2+ + CO32-
4th Determine the solubility - Na2CO3, BaCl2, and NaCl are determined to be soluble and so are written as ions;
BaCO3 is determined to be insoluble and so is written as an empirical formula.
5th ionic eq:
Na1+ + CO32- + Ba2+ + Cl1-  Na1+ + Cl1- + BaCO3
6th net ionic eq:
CO32- + Ba2+

BaCO3
DIRECTIONS: Accurately supply all missing information.
1.
CrBr3
+
K2S

1st
+
3rd
2nd
+
+
4th Determine the solubility of the reactants and products, and circle the appropriate form – ions or empirical formula
5th ionic eq:
6th net ionic eq:
2.
NaF
+
1
+
Mg(NO3)2

+
3rd
st
2nd
+
4th Determine the solubility of the reactants and products, and circle the appropriate form – ions or empirical formula
5th ionic eq:
6th net ionic eq:
Problem Set – Solubility and Net Ionic Equations - #2
3.
(NH4)2SO4
+
1
Ca(OH)2

+
3rd
st
2nd
+
+
4th Determine the solubility of the reactants and products, and circle the appropriate form – ions or empirical formula
5th ionic eq:
6th net ionic eq:
4.
K2C2O4
+
Ni(NO3)3

1st
+
3rd
2nd
+
+
4th Determine the solubility of the reactants and products, and circle the appropriate form – ions or empirical formula
5th ionic eq:
6th net ionic eq:
5.
AgNO3
+
CuCl2

1st
+
+
3rd
2nd
+
4th Determine the solubility of the reactants and products, and circle the appropriate form – ions or empirical formula
5th ionic eq:
6th net ionic eq:
Problem Set – Solubility and Net Ionic Equations - #2
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 rules written for cations instead of anoins.
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 COMPOUNDS
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:
Compounds of NH41+ and the alkali metal cations*.
carbonate, CO32phosphate, 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+