CHM 1046

Review Test 4

 

 

1. Terminology i.e. equilibrium, hydrolysis reactions, salts, anion,   cations, types of salts (acidic salts, basic salts, neutral) acid-base  titrations, molar solubility, electrochemistry, oxidizing agents, reducing agents, voltaic cells, electrolytic cells, anode, cathode, salt bridge, reduction potentials at standard and non-standard conditions, etc.

 

 

2. Salt Hydrolysis Equilibria

 

1. Soluble salts (100% ionization) vs. insoluble salts. 
2. Types of salts: acidic, basic, neutral.
3. Conjugate acid and bases, hydrolysis reactions.
4. Hydrolysis constants calculations.
5. pH calculations.

 

                For a quick presentation/review of the last  topic click equilibria  

 

3.   Acid-Base Titrations in aqueous solutions: types and general concepts

        a.    pH calculations at different points of the titration of strong acid and strong bases

        b.    pH calculations at different points of the titration of strong acid and weak bases

        c.    pH calculations at different points of the titration of weak acid and strong bases

     

                For a quick presentation/review of the last  topic click    titration  

 

4.   Solubility product constant, Ksp and molar solubility, x

        a.  Give Ksp expressions for different salts

        b.  Given Ksp calculate molar solubility and vice versa

        c.   The common ion effect and solubility

 

5.  Electrochemistry: types of cells and characteristics of each

        a.  Voltaic cells and reduction potentials at standard conditions

        b.  Nernst Equation:   E = E^o - 0.0592/n log Q

        c.  Relationships between electrochemistry, thermo and equilibrium          DG = -nFE  ;  E^o  =  0.0592/n log K

        d.  Electrolytic cells: anode, cathode reactions; calculations using          electrolytic cells