1. Weak electrolyte Weak electrolytes are not fully ionized in solution, such as weak acids and bases. Degree of ionization (α): defined as the ratio of the amount of ions being formed in the solution and the amount of electrolyte added to the solution. For the acid HA at a molar concentration c, [H 3 O + ] = αc, [A - ] = αc, [HA] = c –αc Since only fraction, α, of electrolyte is actually presents as ions, the measure conductivity Λ m, is given by: Λ m = αΛ 0 m

2. Ostwald’s dilution law

3. 24.7 The mobility of ions Drift speed: the terminal speed reached when the accelerating force is balanced by the viscous drag. Accelerating force induced by a uniform electric field (E = Δø/ l ): F = z e E = z e Δø/ l Friction force F fric = (6πηa)s, a is the hydrodynamic radius Mobility of an ion:

4. Mobility and conductivity For the solution: Λ 0 m = (z + u + v + + z - u - v - ) F

5. Transport numbers The fraction of total current carried by the ions of a specified type. The limiting transport number, t 0 ±,

6. Conductivities and ion-ion interactions

7. 24.8 The thermodynamic view of diffusion The maximum amount of work can be done when moving a substance from local x to x+dx is: When expressed with an opposite force: dw = - F dx Then one gets: Therefore: The slope of the chemical potential can be interpreted as an effect force, thermodynamic force. This force represents the spontaneous tendency of the molecules to disperse.

8. Since μ = μ ө + RTlnα One get Using concentrations to replace the activity: Recall Fick’s first law of diffusion: Connections between the thermodynamic force and the concentration gradient

9. 24.9 The diffusion equation

10. Derivation of the diffusion equation The amount of particles enter the slab in the time interval dt equals: JAdt, where J is the matter flux The increase in molar concentration inside the slab is: JAdt / (A l t) = J/ l Consider the outflow through the right-hand side: -JAdt / (A l t) = J/ l The net change is: Then

11. Designing electrochemical cells Example 1: 5Zn + 2MnO 4 - + 16H + → 5Zn 2+ + 2Mn 2+ + 8H 2 O Example 2: Pt | H 2 (g) | HCl (aq), AgCl(s) | Ag(s) Example 3: Zn(s) | ZnCl 2 (aq) | KCl(aq) | CuCl 2 | Cu(s)

12. Highlights of Chapter 9 Extent of the reaction. Reaction Gibbs energy. The relationship between the reaction Gibbs energy and chemical potential. The relationship between the reaction Gibbs energy and chemical equilibrium. Expressing equilibrium constant in terms of the standard reaction Gibbs energy. Calculations of the reaction Gibbs energy. Le Chatelier’s principle. Van’t Hoff equation. Changes of pH during the titration of weak acids (at the beginning, in the process, at the stoichiometric point, beyond the ending point).

13. Highlights from Chapter 10 Standard enthalpy and Gibbs energy of formation for ions. Thermodynamic cycle. The standard enthalpy and Gibbs energy of formation of H + is used as the reference for other ions. Activity coefficient. Debye-Huckel theory to calculate the mean activity coefficient. Galvanic cell and electrolytic cell. Electrodes and half reactions. Cell potentials. Calculations of the standard cell potential. Applications of the standard potential. Temperature coefficient of cell potential.

14. Highlights from Chapter 24 Kinetic theory. Flux of matter. Flux of energy. Flux of momentum. Effusion. Collision flux, collision frequency, and their connection with the measurement of vapor pressure. Molar conductivity for electrolytes. Molar conductivity of individual ions. Kohlrausch’s law. Ostwald’s dilution law. Thermodynamic view of diffusion.