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प्रश्न
Why does the conductivity of a solution decrease on dilution of the solution?
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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 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.
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 ____________.
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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
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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
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