Why does the conductivity of a solution decrease with dilution?
The variation of conductivity with dilution can be explained on the basis of number of ions in solution.
In case of weak electrolyte, the number of ions furnished by an electrolyte in solution depends upon the degree of dissociation with dilution. With the increase in dilution, the degree of dissociation increases, as a result the molar conductance increases.
But for strong electrolyte, there is no increase in the number of ions with dilution because strong electrolytes are completely ionized in solution at all concentrations. However, in concentrated solutions of strong electrolytes there are strong forces of attraction between the ions of opposite charges called Interionic Forces. Due to these interionic forces the conducting ability of the ions is less in concentrated solutions. With dilution, the ions becomes far apart from each other and interionic forces decreases. As a result, molar conductance increases with dilution.
The reaction between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table:
| Experiment |
A/ mol L - 1 |
B/ mol L - 1 |
Initial rate/mol L - 1 min - 1 |
| I | 0.1 | 0.1 |
2.0 × 10 - 2 |
| II | -- | 0.2 |
4.0 × 10 - 2 |
| III | 0.4 | 0.4 | -- |
| IV | -- | 0.2 |
2.0 × 10 - 2 |
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The variation of conductivity with dilution can be explained on the basis of number of ions in solution.
In case of weak electrolyte, the number of ions furnished by an electrolyte in solution depends upon the degree ...
Step-by-step explanation:
• The variation of conductivity with dilution can be explained on the basis of number of ions in solution
•
•
• In case of weak electrolyte, the number of ions furnished by an electrolyte in solution depends upon the degree of dissociation with dilution
• With the increase in dilution, the degree of dissociation increases, as a result the molar conductance increases
Students often lose marks by skipping steps, writing incomplete explanations, or misunderstanding keywords used in the question.
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