1. ACID-BASE NEUTRALIZATION REACTIONS: A special type of double-replacement reaction. An acid reacts with a base and neutralizes it. The equation will always be: Acid + Base  water + salt (salt being any ionic compound) For example: HCl + NaOH  H 2 O + NaCl

2. DISSOCIATION When compounds separate or split into smaller ions. If enough of the compound splits into ions, then the substance is considered an electrolyte because it can conduct electricity. Which substances have HIGH dissociation rates?

3. What compounds have high dissociation rates? All ionic compounds: –NaCl + H 2 O  Na + + Cl - + H 2 O Strong bases –NaOH + H 2 O  Na + + OH - + H 2 O Strong acids –HCl + H 2 O  H 3 O + + Cl - Covalent Compounds: Do not dissociate in water!

4. NET IONIC EQUATIONS: Spectator ions: ions that do not take part in the reaction- they sit in the stands and “watch” the action happen! Take them out of the equation and leave in only those ions that actually react: NaCl (aq) + AgNO 3(aq)  AgCl (s) + NaNO 3(aq) Ions in aqueous sol’ns are dissociated: Na + + Cl - +Ag + +NO 3 -  AgCl +Na + +NO 3 - Ag + + Cl -  AgCl (s) Total Ionic Equation