1. 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

2. 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!!!!!

3. 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)

4. 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

5. H+

6. 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

7. H –– Cl H+
Cl-

8. 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