CHEMICAL AND IONIC EQUILIBRIUM

1. Equilibrium in Water : 
   
   • Equilibrium Constant , K = 
     [C]^c[D]^d[A]^a[B]^b
      = 
     k_forwardk_backward
      = K_C
   • In terms of partial pressure
     Equilibrium Constant , K_p = 
     p_C^c p_D^dp_A^a p_B^b
      = K_c (RT)^Δn_g       [Δn_g = n_p - n_r]
2. Van't Hoff Equation : 
   
3. Gibb's Free Energy 
   ΔG = Δ - TΔS
   ΔG_o = - 2.303 RT log₁₀K
4. Buffer : 
   pH = pK_a + log 
   [conjugate base][acid]
   
   pOH = pK_b + log 
   [conjugate acid][base]
   
   Mixture of weak acids = ( k₁c₁ +k₂c₂ )^1/2
   α = 
   % conjugation100
   
   
   ∴ K_sp = [A^y+] ^x [B^x-] ^y
5. Arrhenius Concept : 
   Substance which give H⁺ ions when dissolved in water are called acids , while gives OH^- ions are called bases.
6. Bronsted Lowry Concept : 
   Acid donates proton , base accepts ptoton.
7. Ostwald's Dilution Law : 
   α = ( K / C)^1/2
   K = dissociation constant of weak electrolyte
   C = Concerntatation
   α = degree of dissociation
   K_W = [H⁺ ][OH^- ]
8. Hydrolysis Constant : 
   K_h = 
   h²C1 - h
   
   h = 
   amount of salt hydrolysedTotal salt taken
9.