7-2
Remember that strong acids and bases are considered to be strong electrolytes, so would be
shown in the complete ionic equation in their dissociated ionic form. Weak acids are weak
electrolytes so should be written in molecular form.
The third way to write a double displacement reaction is called the net ionic equation. In this
form, only reacting ions and their product(s) are written exactly how they appear in the complete
ionic equation. Spectator ions are any ions that do not change throughout the course of the
reaction. These are not shown in the net ionic equation as they were not involved in the actual
reaction. The net ionic equation can be seen in Eqn. 4.
Mg
2+
(aq) + CO
3
2-
(aq) → MgCO
3
(s) Eqn. 4
The net ionic equation shows clearly that a reaction has occurred but does not indicate any
context. All three equations are needed to express a single double displacement reaction as each
tells a different layer of information.
If either product (AX or BY) from a double displacement reaction forms an insoluble precipitate,
the reaction is additionally classified as a precipitation reaction. The solid is called the precipitate
and the solution is the supernatant. A clear solution is one that does not contain any precipitate.
A colorless solution is a solution that is absent of color. The color of the precipitate may be
different than the color of the supernatant. Eqn. 4 indicates that the reaction between Mg(NO
3
)
2
and K
2
CO
3
is a precipitation reaction since MgCO
3
(s) is formed. The solubility of some ionic
compounds in aqueous solution is expressed in Table 1.
If either product (AX or BY) is a gas, it is called a gas evolution reaction. The most common gases
produced in gas evolution and double displacement reactions are CO
2
(g), SO
2
(g), NH
3
(g), and
H
2
S(g). The first three are produced via the immediate breakdown of gas evolution intermediates,
or compounds that, when formed via a double displacement reaction, undergo an immediate
second decomposition reaction. These are seen in Eqns. 5-7. Hydrogen sulfide (H
2
S(g)) is
naturally a gas in normal conditions.
H
2
CO
3
(aq) → H
2
O(l) + CO
2
(g) Eqn. 5
H
2
SO
3
(aq) → H
2
O(l) + SO
2
(g) Eqn. 6
NH
4
OH(aq) → H
2
O(l) + NH
3
(g) Eqn. 7
If the reaction produces heat (is exothermic) and a weak electrolyte, it is an acid-base
neutralization. Acids are compounds that release H
+
in aqueous solution and bases release OH
-
.
When combined, H
+
and OH
-
neutralize one another to make H
2
O(l), as in Eqn. 8. Since the
production of H
2
O(l) in aqueous solution cannot be easily observed, an increase in solution
temperature indicating an exothermic reaction will instead be used as evidence for a successful
acid-base neutralization.
H
+
(aq) + OH
-
(aq) → H
2
O(l) Eqn. 8
If both products (AY and BX) are soluble, then no reaction is said to have occurred and no net
ionic equation can be written as all ions will be spectators.