Chapter 7 Chemistry Notes

H 2 naaq cl aq or o nacls h 2 naclaq means same

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Unformatted text preview: me thing) ! If an ionic substance dissolves, it dissociates into solvated ions. Precipitate Formation CaCO3(s) does not dissolve to a significant extent. Observation: some ionic solids do not dissolve significantly in water. Would this “shell solution” conduct electricity? Why or why not? ________________________________________________ The white solid Pb(NO3)2 and the white solid KI are substances that dissolve to give clear colorless solutions. Pb(NO3)2(s) Pb2+(aq) + 2 NO3-(aq) KI(s) K+(aq) + I-(aq) When you add a seashell (98%, CaCO3) to water, what happens? Think about what you have already seen: But remember what happened when mixed? A yellow solid (PbI2) formed. Such solid forming reactions are call precipitation reactions. Pb(NO3)2(aq) + 2 KI(aq) 2 KNO3 (aq)+ 2 PbI2(s) What if we add PbI2 and KNO3 water? 2 KNO3 (aq)+ 2 PbI2(s) no reaction It seems to be “in the nature” of the PbI2. ionic substances have to dissolve in order to form an electrolyte. Solubility Guidelines (“usually soluble”) Compounds containing the following ions are generally soluble Exceptions (when combined with ions on the left the compound is insoluble) Li+, Na+, K+, NH4+ –, none – NO3 C2H3O2 Cl–, Br–, I– 2– SO4 none Ag+, Hg22+, Pb2+ Ca2+, Sr2+, Ba2+, Solubility Rules: (“usually insoluble”) Compounds containing the following ions are generally insoluble OH– [Li+, Na+, K+, NH4+,]** Ca2+, Sr2+, Ba2+ [Li+, Na+, K+, NH4+,] ** Ca2+, Sr2+, Ba2+ [Li+, Na+, K+, NH4+] ** S2– Pb2+ For example, KI, Pb(NO3)2 , and FeSO4 are soluble, but PbI2, CaSO4 , and AgBr are insoluble. memorize these! CO32–, PO43– **Already Exceptions (when combined with ions on the left the compound is soluble or slightly soluble) known case from prior usually soluble” rules. memorize these! Which Compounds are Soluble in Water? Chapter 7 to do list Read Chapter 7 Finish MC6 homework, due Monday @11:59PM. KOH Pb(NO3)2 Finish up MC7- prep due Wed. @ 11:59PM. BaSO4 Practice Balancing Reactions CdS CuSO4 CaS Soluble Li+, Na+, K+, NH4+ NO3-, C2H3O2Cl-, Br-, I- (except Hg22+, Ag+, Pb2+) SO42(except Group 2A & Pb2+) Mostly Insoluble (Except Li+, Na+, K+, NH4+, H+) CO32- , PO43OH- (slightly soluble Group 2A) S2- (except Group 2A) 3 9/27/2013 Which Compounds are Soluble in Water? Co3PO4 PbSO4 Insoluble Mn(OH)2 Insoluble ZnS Insoluble (NH4)2S Soluble Chapter 7B - Chemical Reactions Insoluble Soluble Li+, Na+, K+, NH4+ NO3-, C2H3O2Cl-, Br-, I- (except Hg22+, Ag+, Pb2+) SO42(except Group 2A & Pb2+) Mostly Insoluble Soluble and insoluble ionic compounds Precipitation reactions/double displacement reactions Complete and net ionic reactions Acid-Base reactions (Except Li+, Na+, K+, NH4+, H+) OH- (slightly soluble Group 2A) S2- (except Group 2A) Writing acid-base reactions Acid-base gas forming reactions CO32- , PO43- Chapter Outline • • • • • • • • Solubility Guidelines (“usually soluble”) Chemical Equations: Chemical change & balance √ Solubility and electrolytes √ Types of Reactions: (by types of chemistry) Precipitation & Solubility ◄ Acid-Base (H+, OH-) Gas Evolution (Bubbles) Oxidation-Reduction (Redox, electrons) • • • Exceptions (when combined with ions on the left the compound is insoluble) Li+, Na+, K+, NH4+ –, none – NO3 C2H3O2 Cl–, Types of Reactions: (by atom exchange pattern) • Compounds containing the following ions are generally soluble Double Displacement (AB + CD AD + CB) ◄ Synthesis (Mak...
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This note was uploaded on 02/04/2014 for the course CHEM 004:007 taught by Professor Russellarsen during the Fall '13 term at University of Iowa.

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