Final Exam Review Section 3 Flashcards
% Composition Equation
(Molar mass of X)/Total Mass *100
Molarity Equation
M = moles / Liters
Dilution Equation
M1V1 = M2V2
Group 1 compounds solubility
Li +, Na +, K +, Rb +, Cs +
soluble no exceptions
ammonium ion solubility
NH4+
Soluble no exceptions
Halides solubility
Cl -, Br -, I -
Soluble
exceptions are Ag+, Hg2 2+, Pb 2+
Nitrate solubility
NO3 -
Soluble no exceptions
Perchlorate solubility
ClO4 -
Soluble no exceptions
Acetate solubility
CH3CO2 -
Soluble no exceptions
Sulfate solubility
SO4 2-
Soluble
exceptions: Ca 2+, Sr 2+, Ba 2+, Hg2 2+, Pb 2+
Carbonate solubility
CO3 2-
Insoluble
Exceptions: Cations of 1A & NH4 +
Sulfide solubility
S 2-
Insoluble
Exceptions: Cations of 1A, NH4 +, Ca 2+, Sr 2+, Ba 2+
Phosphate solubility
PO4 3-
Insoluble
Exceptions: Cations of 1A & NH4 +
Hydroxide solubility
OH -
Insoluble
Exceptions: Cations of 1A, NH4 +, Ca 2+, Sr 2+, Ba 2+
Reduction
Gain of electrons; more (-) charge
Oxidizing agent
Oxidation
Loss of electrons; more (+) charge
Reducing Agent
Non-Electrolytes
Compounds that dissolve in water but do not Ionize completely when dissolved in water
Strong Electrolytes
Assumed to ionize completely when dissolved in water
-Soluble via solubility rules, strong acids, strong bases
Weak Electrolytes
Assumed to ionize minimally when dissolved in water
-insoluble via solubility rules, weak acids, weak bases
Strong Acids
HCL, HBr, HI, HClO4, HNO3, H2SO4
Strong Bases
LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
Weak Acids and Bases
Anything that is not a strong acid or base
