Handout-11 - Chemistry 111 Fall, 2005 Prof. Simpson...

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Chemistry 111 Fall, 2005 Prof. Simpson Chemistry 111 Handout #11 Solubility and Precipitation – Sample Problems Typical Net Ionic Equations: XY (s) X + (aq) + Y - (aq) XY (s) X 2+ (aq) + Y 2- (aq) X Y 2 (s) X 2+ (aq) + 2 Y (aq) for example… AgBr (s) Ag + (aq) + Br - (aq) C a S O 4 (s) Cu 2+ (aq) + SO 4 2- (aq) C a ( O H ) 2 Ca 2+ (aq) + 2 OH - (aq) Equilibrium Expressions: K sp = [X + ] [Y - ] … and so forth … Guideline to Soluble Compounds: (these are the ones you MUST know) Compound Solublity compounds with alkali metal ions all soluble compounds with ammonium ion (NH 4 + ) all soluble Nitrates (NO 3 - ), Chlorates (ClO 3 - ), all soluble EXCEPT KClO 4 P e r c h l o r a t e s ( C l O 4 - ), Acetates (CH 3 COO - ) & Be(CH 3 COO) 2 halides (Cl - , Br - , I - ) all soluble EXCEPT those with A g + , Hg 2 2+ and Pb 2+ sulfates (SO 4 2- ) all soluble EXCEPT those with A g + , Ca 2+ , Sr 2+ , Ba 2+ , Pb 2+ , H g
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Handout-11 - Chemistry 111 Fall, 2005 Prof. Simpson...

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