1. Bronsted-Lowry, HA = H⁺ + A^- (conjugate base)

2. K_a = [H⁺] [A^-] / [HA]

   1. For K_a < 1, compound mostly associated

   2. For K_a > 1, compound mostly disassociated into proton (hydronium in water) and conjugate base

3. For H⁺ + A^- = HA, K = [HA] / ([H⁺] [A^-]) = 1/K_a

4. pK_a = -log (K_a), K_a = 10^-pKa (anti log of pK_a)

   1. lower pK_a, more acidic compound, less basic conjugate base

   2. higher pK_a, less acidic compound, more basic conjugate base

   3. pK_a of water = -log([H⁺] [^-OH] / 56) = -log((10^-7) (10^-7) / 56) = 7 + 7 + log(56) = 15.7

5. pH = -log[H⁺]

6. K_a = 10^-pKa = (x) (x) / (I-x), compound of initial concentration I disassociates into [H⁺] = [A^-] = x

   1. K_a (I-x) = x²

   2. x² +K_a x -I K_a = 0

   3. [H⁺] = x = (-K_a + Ö(K_a²+4 I K_a)) / 2, negative answer does not make sense

   4. pH = -log(x)

7. For HA + B^- = A^- + HB, K = K_f K_b

   1. Where HA = H⁺ + A^-, K_f = K_af

   2. Where H⁺ + B^- = HB, K_b = 1/K_ab

   3. K = (10^-pKaf) (10^--pKab) = 10^(-pKaf ^{+ pK}ab)

   4. If -pK_af + pK_ab > 0, pK_af < pK_ab, equilibrium favored towards the right, products

   5. If -pK_af + pK_ab < 0, pK_af > pK_ab, equilibrium favored towards the left, reactants

   6. A mixture of HA and B- with initial concentrations I₁ and I₂, respectively, has a final concentration of A- and HB of:

      1. K =  10^(-pK_af ^{+ pK}_ab⁾ = (x) (x) / ((I₁-x) ((I₂-x))

      2. K (I₁-x) ((I₂-x) = x²

      3. K (I₁I₂ - (I₁+I₂) x + x²) = x²

      4. (K-1) x² -K (I₁+I₂) x + K I₁ I₂ = 0

      5. x = (K (I₁+I₂) ± Ö((K (I₁+I₂))²-4 (K-1) K I ₁ I₂ )/(2 (K - 1)), check that the solution is positive.

      6. The percentage of HA that is disassociated is x / I₁ 100 %

      7. The final ratio of [A^-]/[HA] = x / (I₁-x)

8. Lewis Acids and Bases

9. Nucleophiles and Electrophiles

10. Reasons why some compounds are more acidic than others

    1. Electronegativity, examples: CH₄, NH₃, H₂O, HF

    2. Hybridization: sp³, sp², sp

    3. Delocalization, Resonance effect, examples: carboxylic acids and phenols

    4. Inductive effect, examples: halo substituted carboxylic acids

    5. Sterics, examples: amines

    6. Hard (ionic) and Soft (covalent)

pK_a values