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Writing Total and Net Ionic Equations for Chemical Reactions, Exams of Chemistry

Instructions and examples for writing total and net ionic equations for chemical reactions. It covers various types of substances, including strong and weak acids and bases, soluble and insoluble salts, and gases. The document also explains how to cancel spectator ions in net ionic equations.

Typology: Exams

2021/2022

Uploaded on 09/12/2022

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http://www .csun.edu /~hcchm 001/F reshChe mHa ndouts.htm l
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 Hydroiodic acid H (aq) + I (aq)
+-
HBr Hydrobromic acid H (aq) + Br (aq)
+-
HCl Hydrochloric acid H (aq) + Cl (aq)
+-
33
HNO Nitric acid H (aq) + NO (aq)
+-
44
HClO Perchloric acid H (aq) + ClO (aq)
+-
24 4
H SO Sulfuric acid 2 H (aq) + SO (aq)
+-2
(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 Lithium hydroxide Li (aq) + OH (aq)
+-
NaOH Sodium hydroxide Na (aq) + OH (aq)
+-
KOH Potassium hydroxide K (aq) + OH (aq)
+-
2
Sr(OH) Strontium hydroxide Sr (aq) + 2 OH (aq)
+2 -
2
Ba(OH) Barium hydroxide Ba (aq) + 2 OH (aq)
+2 -
(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) Sodium chloride Na (aq) + Cl (aq)
+-
24 4
K SO (aq) Potassium sulfate 2 K (aq) + SO (aq)
+-2
23 3
Li CO (aq) Lithium carbonate 2 Li (aq) + CO (aq)
+-2
34 4
Na PO (aq) Sodium phosphate 3 Na (aq) + PO (aq)
+-3
42 4 4 4
(NH ) SO (aq) Ammonium sulfate 2 NH (aq) + SO (aq)
+-2
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 (b) weak bases (c) water
232 3 2
HC H O (aq) NH (aq) H O(l)
432
HCN(aq) (NH OH written as NH (aq) + H 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
32432
CaCO (s) CO (g) If NH OH, write NH (aq) + H O(l)
222322
Zn(OH) (s) SO (g) If H CO , write CO (g) + H O(l)
232322
Mg(OH) (s) SO (g) If H SO , write SO (g) + H O(l)
222
Ca(OH) (s) O (g), N (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
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http://www.csun.edu/~hcchm 001/FreshChemHandouts.html

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

  1. 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 Hydroiodic acid H (aq) + I (aq)+^ - HBr Hydrobromic acid H (aq) + Br (aq)+^ - HCl Hydrochloric acid H (aq) + Cl (aq)+^ - HNO 3 Nitric acid H (aq) + NO (aq) 3

HClO 4 Perchloric acid H (aq) + ClO (aq) 4

H SO 2 4 Sulfuric acid 2 H (aq) + SO 4 (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 Lithium hydroxide Li (aq) + OH (aq)+^ - NaOH Sodium hydroxide Na (aq) + OH (aq)+^ - KOH Potassium hydroxide K (aq) + OH (aq)+^ - Sr(OH) 2 Strontium hydroxide Sr (aq) + 2 OH (aq) +2 - Ba(OH) 2 Barium hydroxide Ba (aq) + 2 OH (aq) +2 -

(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) Sodium chloride Na (aq) + Cl (aq)+^ - K SO (aq) 2 4 Potassium sulfate 2 K (aq) + SO 4 (aq)

Li CO (aq) 2 3 Lithium carbonate 2 Li (aq) + CO 3 (aq)

Na PO (aq) 3 4 Sodium phosphate 3 Na (aq) + PO 4 (aq)

(NH ) SO (aq) 4 2 4 Ammonium sulfate 2 NH 4 (aq) + SO 4 (aq)

  1. 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 (b) weak bases (c) water HC H O (aq) 2 3 2 NH (aq) 3 H O(l) 2 HCN(aq) (NH OH written as NH (aq) + H O(l) 4 3 2

  1. 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 CaCO (s) 3 CO (g) 2 If NH OH, write NH (aq) + H O(l) 4 3 2 Zn(OH) (s) 2 SO (g) 2 If H CO , write CO (g) + H O(l) 2 3 2 2 Mg(OH) (s) 2 SO (g) 3 If H SO , write SO (g) + H O(l) 2 3 2 2 Ca(OH) (s) 2 O (g), N (g) 2 2
  2. For the net ionic equations , cancel any substances or ions that appear on both sides of the equation.

WRITING TOTAL AND NET IONIC EQUATIONS

http://www.csun.edu/~hcchm 001/FreshChemHandouts.html

(a) Overall equation :

2 HBr(aq) + (NH ) CO (aq) -----> 4 2 3 2 NH Br(aq) + H CO 4 2 3(aq) strong soluble soluble unstable acid salt salt substance

(b) Total ionic equation :

2 H (aq) + 2 Br (aq) + 2 NH 4 (aq) + CO 3 (aq) ----->

spectator spectator ion ion

2 NH 4 (aq) + 2 Br (aq) + CO (g) + 2 H O(l) 2

spectator spectator ion ion (c) Net ionic equation :

2 H (aq) + CO 3 (aq) ----> CO (g) + 2 H O(l) 2

  • 2-

charge: +2 -2 = 0 0 0

(a) Overall equation :

- [H SO (aq)] 2 3 – unstable substance Na SO (aq) 2 3 + 2 HCl(aq) 6 H O(l) + 2 SO (g) + 2 2 NaCl(aq) soluble strong soluble salt acid salt

(b) Total ionic equation :

2 Na (aq) + SO 3 (aq) + 2 H (aq) + 2 Cl (aq) ---->

  • -2 + - spectator spectator ion ion

H O(l) + 2 SO (g) + 2 2 Na (aq) + 2 Cl (aq)

spectator spectator ion ion (c) Net ionic equation :

SO 3 (aq) + 2 H (aq) ----> H O(l) + 2 SO (g) 2 -2 +

charge: -2 +2 = 0 0 0

WRITING TOTAL AND NET IONIC EQUATIONS

EXAMPLES

Reaction of hydrobromic acid and ammonium carbonate in aqueous solution

Reaction of sodium sulfite with hydrochloric acid in aqueous solution