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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 ____________.
| 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.
Faradays constant is defined as ____________.
Which of the following electrolytic solution has the least specific conductance?
The equivalent conductance of `"M"/36` solution of a weak monobasic acid is 6 mho cm2 equivalent−1 and at infinite dilution is 400 mho cm2 equivalent−1. The dissociation constant of this acid 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.
