Advertisements
Advertisements
Question
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 ____________.
Options
2.88 S cm2 mol−1
11.52 S cm2 mol−1
0.086 S cm2 mol−1
28.8 S cm2 mol−1
Advertisements
Solution
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 11.52 S cm2 mol−1.
Explanation:
Λ = `"κ"/"M" xx 10^-3 "mol"^-1 "m"^3`
= `(5.76 xx 10^-3 xx "S cm"^-1 xx 10^-3)/0.5` mol−1 m3
= `(5.76 xx 10^-3 xx 10^-3 xx 10^6)/0.5` S cm−1 mol−1 cm3
= 11.52 S cm2 mol−1
APPEARS IN
RELATED QUESTIONS
The number of electrons that have a total charge of 9650 coulombs is ____________.
Faradays constant is defined as ____________.
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.
Why does the conductivity of a solution decrease on dilution of the solution?
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.
Ionic conductance at infinite dilution of Al3+ and \[\ce{SO^{2-}_4}\] are 189 and 160 mho cm2 equiv−1. Calculate the equivalent and molar conductance of the electrolyte Al2(SO4)3 at infinite dilution.
