Chemistry review

Chapter 14: Solution
Henry's Law: C = k P, where c is solubility, k is constant and P is pressure. Therefore, if pressure of solution increase, solubility increase.
Osmotic pressure = iMRT, where i is Van't Hoff's factor, M is molarity, R is 0.08206 and T is temperature in Kelvin.
Raoult's Law: Vapor pressure, PA = XA PA*, if add solutes to solution, vapor pressure decreases.
Freezing point depression: delta T = -KfM
Boiling point elevation: delta T = KbM

Chapter 16: Chemical Equlibrium
Kp = Kc (RT)^delta n
If Qc = 0 : equlibrium
If Qc < 0 : too much reactant, move to right
If Qc > 0 : too much product, move to left

Chapter 17: Acids and Bases
Kw = [H3O+][OH-] = KaKb = 1.0 x 10^(-14)
pH = -log[H3O+]
pOH = -log[OH-]
pKw = pH + pOH = 14

The stronger an acid, the weaker its conjugate base.
Eg: HF is acidic, therefore its conjugate ion, F- is basic.
Note: ion of strong acid and base is neutral.
Eg: Na+ is neutral (Bacause NaOH is strong base).

What makes an ion more acidic?
1. If conjugate is delocalized - more stable - ion more acidic.
2. More eletronegative - more stable - more stable.
3. Have a resonance structure - more delocalized - more stable.

Lewis theory:
Acid: electron pair acceptor
Base: electron pair donor

Wah.. i finish reading 3 chapters already!! :D Tmr is presidential day holiday! Can do practice tests.. good luck to everyone!! Jia you!!