Advertisements
Advertisements
प्रश्न
The molar conductivity of 0.025 mol L−1 methanoic acid is 46.1 S cm2 mol−1. Calculate its degree of dissociation and dissociation constant. Given \[\ce{λ^0_{(H^+)}}\] = 349.6 S cm2 mol−1 and \[\ce{λ^0_{(HCOO^-)}}\] = 54.6 S cm2 mol−1.
उत्तर
\[\ce{∧^0_{{m}(HCOOH)} = λ^0_{(H^+)} + λ^0_{(HCOO^-)}}\]
= 349.6 + 54.6
= 404.2 S cm2 mol−1
Given: \[\ce{∧_{{m}(HCOOH)}}\] = 46.1 S cm2 mol−1
Degree of dissociation, α = `∧_"m"/(∧_"m"^0)`
= `(46.1 "S cm"^2 "mol"^-1)/(404.2 "S cm"^2 "mol"^-1)`
= 0.114
\[\ce{HCOOH ⇌ HCOO^- + H^+}\]
| Initial concentration | c mol L−1 | 0 | 0 |
| Concentration at equilibrium | c(1 − α) | cα | cα |
∴ Kα = `("c"α . "c"α)/("c"(1 - α))`
= `("c"α^2)/(1 - α)`
= `(0.025 xx (0.114)^2)/(1 - 0.114)`
= 3.67 × 10−4
APPEARS IN
संबंधित प्रश्न
The conductivity of 0.20 M solution of KCl at 298 K is 0.025 S cm−1. Calculate its molar conductivity.
The conductivity of 0.001 mol L-1 solution of CH3COOH is 3.905× 10-5 S cm-1. Calculate its molar conductivity and degree of dissociation (α) Given λ°(H+)= 349.6 S cm2 mol-1 and λ°(CH3COO)= 40.9S cm2mol-1.
The conductivity of 0.02M AgNO3 at 25°C is 2.428 x 10-3 Ω-1 cm-1. What is its molar
conductivity?
Calculate the degree of dissociation (α) of acetic acid if its molar conductivity (Λm) is 39.05 S cm2 mol−1.
Given λ°(H+) = 349.6 S cm2 mol−1 and λ°(CH3COO−) = 40.9 S cm2 mol−1
A steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes FeSO4and ZnSO4 until 2.8g of Fe deposited at the cathode of cell X. How long did the current flow? Calculate the mass of Zn deposited at the cathode of cell Y.
(Molar mass: Fe=56g mol-1,Zn=65.3g mol-1,1F=96500C mol-1)
Conductivity always decreases with decrease in concentration both, for weak and strong electrolytes because of the fact that ____________.
Kohlrausch law of independent migration of ions states ____________.
Which of the statements about solutions of electrolytes is not correct?
When acidulated water (dil.H2SO4 solution) is electrolysed, will the pH of the solution be affected? Justify your answer.
Write the cell reaction of a lead storage battery when it is discharged. How does the density of the electrolyte change when the battery is discharged?
Why on dilution the m Λm of \[\ce{CH3COOH}\] increases very fast, while that of \[\ce{CH3COONa}\] increases gradually?
Assertion: `"E"_("Ag"^+ //"Ag")` increases with increase in concentration of Ag+ ions.
Reason: `"E"_("Ag"^+ //"Ag")` has a positive value.
Solutions of two electrolytes ‘A’ and ‘B’ are diluted. The Λm of ‘B’ increases 1.5 times while that of A increases 25 times. Which of the two is a strong electrolyte? Justify your answer. Graphically show the behavior of ‘A’ and ‘B’.
The limiting molar conductivities for Nacl, KBr and KCI are 126, 152 and 150 S cm2 mol–1 respectively. The limiting molar conductivity for Na Br is:-
Which of the following increases with the increase in the concentration of the solution?
The molar conductivity of 0.007 M acetic acid is 20 S cm2 mol−1. What is the dissociation constant of acetic acid? Choose the correct option.
`[(Λ_("H"^+)^ο = 350 "S" "cm"^2 "mol"^-1), (Λ_("CH"_3"COO"^-)^ο = 50 "S" "cm"^2 "mol"^-1)]`
The molar conductivity of CH3COOH at infinite dilution is 390 Scm2/mol. Using the graph and given information, the molar conductivity of CH3COOK will be:
The specific conductance of 2.5 × 10-4 M formic acid is 5.25 × 10-5 ohm-1 cm-1. Calculate its molar conductivity and degree of dissociation.
Given `λ°_("H"^+)` = 349.5 ohm-1 cm2 mol-1 and
`λ°_("HCOO"^-) = 50.5 " ohm"^-1 "cm"^2 "mol"^-1`
