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प्रश्न
Why does the conductivity of a solution decrease on dilution of the solution?
उत्तर
Conductivity always decreases with a decrease in concentration (on dilution of the solution) both for weak as much as for strong electrolytes. It is because the number of ions per unit volume that carry the current in a solution decreases on dilution.
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संबंधित प्रश्न
The number of electrons that have a total charge of 9650 coulombs is ____________.
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Faradays constant is defined as ____________.
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A conductivity cell has been calibrated with a 0.01 M, 1 : 1 electrolytic solution (specific conductance (κ = 1.25 × 10−3 S cm−1) in the cell and the measured resistance was 800 Ω at 25°C. The cell constant is, ____________.
Conductivity of a saturated solution of a sparingly soluble salt AB (1 : 1 electrolyte) at 298 K is 1.85 × 10−5 S m−1. Solubility product of the salt AB at 298 K `(Λ_"m"^∘)_"AB"` = 14 × 10−3 S m2 mol−1.
The conductivity of a 0.01 M solution of a 1 : 1 weak electrolyte at 298 K is 1.5 × 10−4 S cm−1.
i) molar conductivity of the solution
ii) degree of dissociation and the dissociation constant of the weak electrolyte
Given that
\[\ce{λ^∘_{cation}}\] = 248.2 S cm2 mol−1
\[\ce{λ^∘_{anion}}\] = 51.8 S cm2 mol−1
Arrange the following solutions in the decreasing order of specific conductance.
i) 0.01 M KCl
ii) 0.005 M KCl
iii) 0.1 M KCl
iv) 0.25 M KCl
v) 0.5 M KCl
Why is AC current used instead of DC in measuring the electrolytic conductance?
0.1 M NaCl solution is placed in two different cells having cell constant 0.5 and 0.25 cm−1 respectively. Which of the two will have a greater value of specific conductance.
