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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 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 ____________.
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 ____________.
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.
Which of 0.1 M HCl and 0.1 M KCl do you expect to have greater `Λ_"m"^∘` and why?
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.
