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II. Conductometry

I = V / R. II. Conductometry. Dr. Hisham Ezzat Abdellatef. Introduction. Conductance: is the ability of the medium to carry the electric current. migration of positively charged species towards the cathode and negatively charged ones through the anode. ohm -1 (seimen).

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II. Conductometry

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  1. I = V / R II. Conductometry Dr. Hisham Ezzat Abdellatef

  2. Introduction • Conductance:is the ability of the medium to carry the electric current. • migration of positively charged species towards the cathode and negatively charged ones through the anode ohm-1(seimen) E is the potential difference, i is the current intensity. From Ohm low

  3. The conductance of the solution depends on: 1. Temperature: It is increased by increase of temperature. 2. Nature of ions size, molecular weight, number of charges the ion carries and other factors 3. The concentration of ions: As the number of ions increases the conductance of the solution increases. 4. The size of the electrodes L/A is cell constant K is the specific conductance or conductivity ohm-1cm-1 or seimen/cm.

  4. Equivalent conductance  It is defined as the conductance of one gram equivalent of solute contained between electrodes spaced one centimeter apart. Where C is the concentration in gram equivalent per liter. • Equivalent ionic conductance: • At infinite dilution, interactions become nil; the overall conductance of the solution consists of the sum of the individual equivalent ionic conductance • o = +o + -o

  5. Instrumentments • Two parts: • conductivity bridge. • Conductance cell

  6. Application of conductivity Direct or absolute measurments • checking purity of distilled water or other chemicals. • determination of physical constants such as ionization constant. 2. Conductometric titrations • Very dilute solutions. • Turbid and highly coloured solutions. • Reaction which is not complete and where there is no suitable indicator, e.g. reaction between weak acid and weak base.

  7. 1. Titration of strong acid with strong base: The reaction is represented by the following equations e.g. H+ + Cl- + Na+ + OH- H2O + Na+ + Cl-

  8. 2. Very weak acid with strong base or a very weak base with stronger acids

  9. Determination of mixture of hydrochloric acid (strong acid) and acetic acid (weak acid) with sodium hydroxide (strong base)

  10. 3. Precipitation and complex formation reaction Na+ + Cl- + Ag+ + NO3- AgCl + Na+ + NO3-

  11. Conductivity as a function of the volume of added standard solution in the titration of an approximately 0.1 molar acetic acid solution (V = 5 ml) with a sodium hydroxide solution (c = 0.1 mol · l-1)

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