WRITING TOTAL AND NET IONIC EQUATIONS
1. Write the overall equation including the correct designations for the physical state of the substances
(s, l, g, aq). Balance this equation. Most of these kinds of equations are double displacement
reactions: AX + BY 6 AY + BX
2. For the total ionic equations, write strong electrolytes in solution in the form of aqueous ions.
(a) Strong acids. The common strong acids and their aqueous ions are:
HI
HBr
HCl
HNO3
HClO4
H2 SO4
Hydroiodic acid
Hydrobromic acid
Hydrochloric acid
Nitric acid
Perchloric acid
Sulfuric acid
H+ (aq) + I-(aq)
H+ (aq) + Br-(aq)
H+ (aq) + Cl-(aq)
H+(aq) + NO3 -(aq)
H+ (aq) + ClO4 -(aq)
2 H+ (aq) + SO4 -2 (aq)
(b) Strong bases. Strong bases are the hydroxides of the alkali (Group IA) and
alkaline earth (Group IIA) metals ions which are sufficiently soluble. The
common strong bases and their aqueous ions are:
LiOH
NaOH
KOH
Sr(OH)2
Ba(OH)2
Lithium hydroxide
Sodium hydroxide
Potassium hydroxide
Strontium hydroxide
Barium hydroxide
Li+(aq) + OH-(aq)
Na+ (aq) + OH-(aq)
K+ (aq) + OH-(aq)
Sr+2(aq) + 2 OH-(aq)
Ba+2(aq) + 2 OH-(aq)
(c) Soluble salts. Determinations of the solubility of a salt may be made by
reference to SOLUBILITIES OF IONIC COMPOUNDS. Soluble salts are
written as their aqueous ions:
NaCl(aq)
K2 SO4 (aq)
Li2 CO3 (aq)
Na3 PO4 (aq)
(NH4 )2 SO4 (aq)
Sodium chloride
Potassium sulfate
Lithium carbonate
Sodium phosphate
Ammonium sulfate
Na+(aq) + Cl-(aq)
2 K+ (aq) + SO4 -2 (aq)
2 Li+ (aq) + CO3-2 (aq)
3 Na+ (aq) + PO4 -3 (aq)
2 NH4 + (aq) + SO4 -2 (aq)
3. For the total ionic equations, write the weak electrolytes in solution as their (predominantly)
molecular form. Weak electrolytes, or un-ionized substances, include (with examples):
(a) weak acids
HC2 H3 O2 (aq)
HCN(aq)
(b) weak bases
NH3 (aq)
(NH4OH written as NH3(aq) + H2O(l)
(c)
water
H2 O(l)
4. For the total ionic equations, write insoluble substances as the total compound (in their
molecular form). Unstable substances are written in their decomposed forms. These substances
include (with examples):
(a) precipitates or insoluble reactants (b) gases
(c) derived from unstable substances
CaCO3 (s)
CO2 (g)
If NH4 OH, write NH3 (aq) + H2 O(l)
Zn(OH)2 (s)
SO2 (g)
If H2 CO3 , write CO2 (g) + H2 O(l)
Mg(OH)2 (s)
SO3 (g)
If H2 SO3 , write SO2 (g) + H2 O(l)
Ca(OH)2(s)
O2(g), N2(g)
5. For the net ionic equations, cancel any substances or ions that appear on both sides of the equation. WRITING TOTAL AND NET IONIC EQUATIONS
EXAMPLES
Reaction of hydrobromic acid and ammonium carbonate in aqueous solution
(a) Overall equation:
2 HBr(aq) +
strong
acid
(NH4)2CO3(aq) ----->
soluble
salt
2 NH4Br(aq) + H2CO3(aq)
soluble
unstable
salt
substance
(b) Total ionic equation:
2 H+ (aq)
+
2 Br-(aq)
spectator
ion
+
2 NH4 + (aq)
spectator
ion
+
CO3 -2 (aq)
----->
2 NH4 + (aq) +
spectator
ion
2 Br-(aq)
spectator
ion
+
CO2 (g) +
H2 O(l)
(c) Net ionic equation:
2 H+ (aq)
charge: +2
+
CO32-(aq)
-2 = 0
---->
CO2 (g) +
0
H2O(l)
0
Reaction of sodium sulfite with hydrochloric acid in aqueous solution
(a) Overall equation:
Na2 SO3 (aq)
soluble
salt
+
2 HCl(aq) 6
strong
acid
Ð[H2 SO3 (aq)]Ð unstable substance
H2 O(l) + SO2 (g) + 2 NaCl(aq)
soluble
salt
(b) Total ionic equation:
2 Na+ (aq)
spectator
ion
+
SO3 -2 (aq)
+
2 H+ (aq)
H2 O(l) +
+
2 Cl-(aq)
spectator
ion
---->
SO2 (g) +
2 Na+ (aq)
spectator
ion
+
H2 O(l) +
0
SO2 (g)
0
(c) Net ionic equation:
SO3 -2 (aq)
charge: -2
+
2 H+ (aq)
+2 = 0
---->
2 Cl-(aq)
spectator
ion
Writing Total and Net Ionic Equations
of 2
Report
Tell us what’s wrong with it:
Thanks, got it!
We will moderate it soon!
Free up your schedule!
Our EduBirdie Experts Are Here for You 24/7! Just fill out a form and let us know how we can assist you.
Take 5 seconds to unlock
Enter your email below and get instant access to your document