lab2-chem311-1 - INTRODUCTION I-Objective :- To obtain the...

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INTRODUCTION I-Objective :- - To obtain the electrical conductivity of KCl and acetic acid solutions. - Finding out the limiting conductivity for the two solutions. - To find the dissociation constant of acetic acid. II-Theory :- Some substances that dissociate into ions by some suitable solvents can conduct electricity. Therefore, the conductance of these solutions depends on the degree of dissociation and the concentration of ions. The electrical conductivity, k , is the conductance of a cube of a solution which is contained between two parallel electrodes 1 cm square and 1 cm apart, and it can be found by: k G l A = (1) Where, G = the conductance, S l = the length of material, cm A = the cross-sectional area, cm 2 K = the electrical conductivity, S cm The molar conductivity, Λ , can be defined as, Λ = k c / (2) The importance of the molar conductivity is that it gives information about the conductivity of the ions produced in solution by 1 mol of a substance. Where, c = the concentration, mol/ cm 3 c = the concentration, mol/ cm 3 Λ = The molar conductivity, S cm 2 mol -1 In infinite dilution (c 0 ), we have the limiting molar conductivity Λ 0 , which can expressed as, Λ 0 = λ 0 + + λ 0 - (3) 2
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STRONG ELECTROLYTES KCl is a one of the strong electrolytes that occur almost as ions when they are in aqueous solution. . It does obey the Debye-Huckel- Onsager equation, Λ = Λ 0 - a c (4) Where, a is a constant. For strong electrolytes the molar conductivity falls only slightly as the
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lab2-chem311-1 - INTRODUCTION I-Objective :- To obtain the...

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