Happy Birthday Jagdish Chandra Bose (1858-1937) Mastering Chemistry New assignment will be posted later today Due Tuesday by 11:59PM Reading Chapter 7, sections 5-10

THESE ONLY APPLY TO IONIC COMPOUNDS!!!!! Solubility Rules All ammonium and group 1 metal salts are SOLUBLE (no exceptions) All nitrate, chlorate, perchlorate, and acetate salts are SOLUBLE (no exceptions) Most chloride, bromide, and iodide salts are SOLUBLE. EXCEPTIONS! Compound containing silver, mercury (I), and lead (II) Most fluoride salts are SOLUBLE. EXCEPTIONS! Compounds containing magnesium, calcium, strontium, barium, and lead (II) Most sulfate salts are SOLUBLE. EXCEPTIONS! Compounds containing strontium, barium, mercury (I), and lead (II) Most sulfide and hydroxide salts are INSOLUBLE. EXCEPTIONS! Compounds containing calcium, strontium, and barium Most carbonate, phosphate, oxalate, and chromate salts are INSOLUBLE. THESE ONLY APPLY TO IONIC COMPOUNDS!!!!!

Solubility and Reactions Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s) Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s) Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s) Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s) Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s) 3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l) 3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l) 3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l) 3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l) 3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l) 2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s) 2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s) 2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s) 2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s) 2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s) 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g) K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g) K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g) K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g) K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g) K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g) 2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq) 2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq) 2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq) 2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq) 2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq)

Electrolytes What are they? Three types of electrolytes: Non-electrolytes Molecular compounds Do NOT form ions in water Weak electrolytes Weak acids Insoluble salts (insoluble ionic compounds) Form very VERY few ions in water

H+

Electrolytes What are they? Three types of electrolytes: Strong electrolytes Strong acids Soluble salts (soluble ionic compounds) Completely break apart into ions Called ionization when talking about acids Called disassociation when talking about salts

H –– Cl H+ Cl-

Electrolytes Strong acids? HCl(aq) HBr(aq) HI(aq) HNO3(aq) HClO4(aq) H2SO4(aq) ANY other acid is a weak acid (which makes it a weak electrolyte