CHM 1046

Review Test 3

 

 

  1. Terminology i.e. equilibrium, equilibrium constants, LeChatelier's Principle, acids (strong/weak), bases (strong/weak), salts, buffers, etc.

 

 

  1. Chemical Equilibria

 

    1. Equilibrium expression as a function of concentration & pressure 
    2. Equilibrium constants expressions and balanced reactions
    3. Heterogeneous and homogeneous equilibria
    4.  Relationship  between Kp and Kc:      Kp = Kc(RT)Dn 
    5. Le Chatelier's Principle and concentration, pressure, temperature changes
    6. Finding K from equilibrium concentrations values
    7. Finding equilibrium values knowing Keq via 3 approaches using  i c e methods: neglecting x if  K allows it, perfect squares method and quadratic expression
    8. Thermo and K:    DG= - RTlnK
    9. Van't Hoff equation  ln K2/K1= DH/R(1/T1 - 1/T2)

 

3.   Acid-Base Equilibria in aqueous solutions general concepts

        a.    Autoionization of water Kw = [H3O+] [OH-] = 1 x 10-14

        b.    pH and pOH

        c.    Classification of substances as acids (strong & weak) bases and salts

        d.    Effects of pH in solutions of strong acids or bases

        e.    Effects of pH in weak acidic or basic solutions; % ionization; Ka and Kb

        f.     Polyprotic acids Ka1, Ka2, etc (compare this case to weak monoprotic acid ionization)

        g.    Buffers and buffer action (addition of strong acids or base to buffers)

                [H+]= a/s x K;      [OH-]=b/s x K

                For a quick presentation/review of the last 4 topics click below  ( hydrolysis is no longer part of test 3 but will be in test 4)   Equilibria