Frequently Asked Questions
What is a net ionic equation?
A net ionic equation shows only the species that actually participate in a reaction - the spectator ions are removed. For AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq), the complete ionic equation splits all aqueous electrolytes: Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) -> AgCl(s) + Na+(aq) + NO3-(aq). Removing Na+ and NO3- (spectators) gives the net ionic equation: Ag+(aq) + Cl-(aq) -> AgCl(s).
What are spectator ions?
Spectator ions are dissolved ions that appear on both sides of the complete ionic equation unchanged. They do not participate in the reaction but are present as counter-ions to balance charge. In the reaction between AgNO3 and NaCl solutions, Na+ and NO3- are spectator ions because they remain in solution throughout. Only Ag+ and Cl- combine to form the precipitate.
How do I know which compounds are soluble (aq) vs. insoluble (s)?
Use the solubility rules. Generally soluble: all nitrates, all sodium/potassium/ammonium salts, most chlorides (except Ag, Pb, Hg), most sulfates (except Ba, Pb, Ca). Generally insoluble: most carbonates, phosphates, hydroxides, and sulfides (except Group 1 and NH4+ salts). Memorizing these rules is essential for predicting precipitation reactions.
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