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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.
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http://www.csun.edu/~hcchm 001/FreshChemHandouts.html
(s, l, g, aq). Balance this equation. Most of these kinds of equations are double displacement reactions: AX + BY 6 AY + BX
(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)
(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
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
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) ---->
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
Reaction of hydrobromic acid and ammonium carbonate in aqueous solution
Reaction of sodium sulfite with hydrochloric acid in aqueous solution