lab2 - Introduction To determine the electrical...

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Introduction: To determine the electrical conductivity and the limiting conductivity of a strong electrolyte (KCl) and a weak electrolyte (acetic acid) and also to determine the dissociation constant of acetic acid. Electrolytes conduct electricity by the dissociation into ions and this conductivity increase with increasing the ions concentration and the degree of dissociation. Κ = G . (L/A) K is the electrical conductance, G is the conductance which is the reciprocal of the resistance. We also define the molar conductivity Λ = k/c .This molar conductivity approaches a limiting value called the limiting molar conductivity in infinite dilution i.e when c goes to zero .This value is the sum of the limiting molar conductivities of each ion. For strong electrolyte the dissociation is complete and they obey the following equation: Λ = Λ o – a * C After measuring “k “ and “c” experimentally the “ Λ o “ can be determined by extrapolating the curve. In the case of weak electrolyte we define a term called the dissociation factor which is defined as : α = Λ / Λ o The equilibrium constant of weak electrolyte is: Ka = (c α ^ 2 ) / ( 1- α ) From this equation we got the relation:
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This note was uploaded on 04/13/2011 for the course CHEM 311 taught by Professor Alial-habib during the Fall '09 term at King Fahd University of Petroleum & Minerals.

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lab2 - Introduction To determine the electrical...

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