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प्रश्न
Why does the conductivity of a solution decrease on dilution of the solution?
Why does the specific conductivity (κ) of a solution decrease on dilution?
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उत्तर
The specific conductivity (κ) of an electrolytic solution decreases during dilution because the number of ions present per unit volume of the solution decreases.
संबंधित प्रश्न
The number of electrons that have a total charge of 9650 coulombs is ____________.
The molar conductivity of a 0.5 mol dm−3 solution of AgNO3 with electrolytic conductivity of 5.76 × 10−3 S cm−1 at 298 K is ____________.
| Electrolyte | KCl | KNO3 | HCl | NaOAC | NaCl |
| Λ_ (S cm mol−1) |
149.9 | 145.0 | 426.2 | 91.0 | 126.5 |
Calculate \[\ce{Λ^∘_{HOAC}}\] using appropriate molar conductances of the electrolytes listed above at infinite dilution in water at 25°C.
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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, ____________.
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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
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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.
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