II Types of Electrolytes A Strong Electrolytes zcompletely

Types of Strong Electrolytes z. Soluble salts z. Strong acids: HCl, HI, HBr, HNO

II. Types of Electrolytes B. Weak Electrolytes z. Only some dissociation z. Most remains

Types of Weak Electrolytes z. Weak acids: ex. HF, CH 3 CO 2 H

II. Types of Electrolytes z. C. Non- Electrolytes zdissolve in water but don’t form

III. When Do Exchange Rx Occur? z. A water insoluble product forms (a precipitation

IV. Precipitation Rx z. A type of exchange reaction zsoluble reactants form insoluble product

3 Ways to Write Equations: z. Overall eq Ag. NO 3(aq) + KBr(aq) Ag.

How do you know when a solid forms? *Understand concepts and memorize rules! *Solids

Predict the Solubility z. KCl z. Mg. CO 3 z. Ni. O z. Ca.

What Possible Solids Could Form in a Reaction? z. Exchange anions and use solubility

Pb(NO 3)2(aq) + K 2 Cr. O 4(aq) ? For practice, write the overall,

Pb(NO 3)2(aq) + K 2 Cr. O 4(aq) Overall: Pb(NO 3)2(aq) + K 2

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II. Types of Electrolytes A. Strong Electrolytes zcompletely ionize in water

II. Types of Electrolytes A. Strong Electrolytes zcompletely ionize in water zconduct electricity well (bright light) AB + H 2 O A+(aq) + B-(aq)

Types of Strong Electrolytes z. Soluble salts z. Strong acids: HCl, HI, HBr, HNO 3, H 2 SO 4, HCl. O 4 HCl + H 2 O H +(aq) + Cl-(aq) H 2 SO 4 + H 2 O H +(aq) + HSO 4 -(aq) z. Strong bases: KOH, Na. OH, Ba(OH)2, Ca(OH)2 KOH + H 2 O K +(aq) + OH-(aq)

II. Types of Electrolytes B. Weak Electrolytes z. Only some dissociation z. Most remains intact in water z. Don’t conduct electricity well (dim light)

Types of Weak Electrolytes z. Weak acids: ex. HF, CH 3 CO 2 H and H 3 PO 4 CH 3 CO 2 H CH 3 CO 2 -(aq) + H+(aq) z. Weak bases: ex. Ammonia NH 3 + H 2 O NH 4+(aq) + OH-(aq)

II. Types of Electrolytes z. C. Non- Electrolytes zdissolve in water but don’t form ions zdo not conduct electricity (no light) zpolar, non-ion forming compounds zex. Sugar, ethanol

III. When Do Exchange Rx Occur? z. A water insoluble product forms (a precipitation rx) z. A stable molecule forms and removes ions from solution (ex. Neutralization rx-more details in chapt 11) z. A gas is produced

IV. Precipitation Rx z. A type of exchange reaction zsoluble reactants form insoluble product

3 Ways to Write Equations: z. Overall eq Ag. NO 3(aq) + KBr(aq) Ag. Br(s) + KNO 3(aq) z. Complete ionic Ag+ (aq) + NO 3 - (aq) + K+ (aq) + Br- (aq) Ag. Br(s) + K+ (aq) + NO 3 -(aq) z. Net ionic Ag+ (aq) + Br-(aq) Ag. Br(s) cancel ions

How do you know when a solid forms? *Understand concepts and memorize rules! *Solids must have a net charge of zero-2 cations can’t form a solid.

Solubility Rules (memorize)

Predict the Solubility z. KCl z. Mg. CO 3 z. Ni. O z. Ca. I 2

Predict the Solubility z. KCl z. Mg. CO 3 z. Ni. O z. Ca. I 2 soluble insoluble

What Possible Solids Could Form in a Reaction? z. Exchange anions and use solubility rules to see if products are solid or aqueous. z. If both are aqueous there is no reaction.

Pb(NO 3)2(aq) + K 2 Cr. O 4(aq) ? For practice, write the overall, complete ionic and net ionic equations for this reaction.

Pb(NO 3)2(aq) + K 2 Cr. O 4(aq) Overall: Pb(NO 3)2(aq) + K 2 Cr. O 4(aq) Decide if any product is solid. Balance!!! ? Pb. Cr. O 4(s) + 2 KNO 3(aq)

Pb(NO 3)2(aq) + K 2 Cr. O 4(aq) Overall: Pb(NO 3)2(aq) + K 2 Cr. O 4(aq) ? Pb. Cr. O 4(s) + 2 KNO 3(aq) To do complete ionic, write aqueous species as separate ions. Complete ionic: Pb 2+ (aq) + 2 NO 3 - (aq) + 2 K+ + Cr. O 42 -(aq) Pb. Cr. O 4 (s) + 2 K+ (aq) + 2 NO 3 - (aq)

Pb(NO 3)2(aq) + K 2 Cr. O 4(aq) Overall: Pb(NO 3)2(aq) + K 2 Cr. O 4(aq) Pb. Cr. O 4(s) + 2 KNO 3(aq) Complete ionic: Pb 2+ (aq) + 2 NO 3 - (aq) + 2 K+ + Cr. O 42 -(aq) Pb. Cr. O 4 (s) + 2 K+ (aq) + 2 NO 3 - (aq) Net ionic: Pb 2+ (aq) + Cr. O 42 -(aq) ? Pb. Cr. O 4 (s)