Advertisements
Advertisements
प्रश्न
Calculate molar conductivity for 0.5 M BaCl2 if its conductivity at 298K is 0.01 Ω–1 cm–1.
Advertisements
उत्तर
Given: c = 0.5 M, k = 0.01 Ω–1 cm–1, Λ = ?
Formula: Λ = `(1000k)/c`
∴ Λ = `(1000 xx 0.01)/0.5`
= 20 Ω–1 cm2 mol–1
APPEARS IN
संबंधित प्रश्न
0.05 M NaOH solution offered a resistance of 31.6 Ω in a conductivity cell at 298 K. If the cell constant of the cell is 0.367 cm-1, calculate the molar conductivity of NaOH solution.
The molar conductivity of 0.05 M BaCl2 solution at 25° C is 223Ω-1 cm2 mol-1. What is its conductivity?
What is a cell constant? What are its units? How is it determined experimentally?
Answer the following in brief.
Explain the effect of dilution of the solution on conductivity.
Answer the following:
What is Kohlrausch law of independent migration of ions? How is it useful in obtaining molar conductivity at zero concentration of a weak electrolyte? Explain with an example.
Kohlrausch law is applicable for the solution _______.
SI unit of conductivity is _______.
Write an equation that shows the relationship between molar conductivity and degree of dissociation of weak electrolyte.
Calculate molar conductivities at zero concentration for CaCl2 and NaCl.
Given: molar ionic conductivities of Ca2+, Cl–, Na+ ions are respectively, 104, 76.4, 50.1 Ω–1 cm–2 mol–1
Molar conductance of BaCl2, H2SO4 and HCl at infinite dilution are X1, X2 and X3 respectively. Molar conductance of BaSO4 at infinite dilution is ____________.
The molar conductances at infinite dilution `(∧_0)` for electrolytes B+A− and C+A− are 140 and 120 S cm2 mol−1. The molar conductance at infinite dilution for B+X− is 198 S cm2 mol−1. The `∧_0` (in S cm2 mol−1) of C+X− is __________.
The resistance of `1/10`M solution is 2.5 × 103 ohm. What is the molar conductivity of solution? (cell constant = 1.25 cm-1).
A conductivity cell having cell constant 8.76 cm−1, placed in 0.01 M solution of an electrolyte offered a resistance of 1000 ohms. What is the specific conductance of electrolytes?
Conductivity of KCI solution is 0.0027 Ω−1 m−1 at 25°C. The resistance of the solution is 82.4 Ω. The cell constant is ____________ m−1.
The molar conductivities at zero concentration for Ca2+ and CaCl2 are 104 and 256.8 Ω−1 cm2 mol−1 respectively. The molar conductivity at zero concentration for Cl− is ____________.
The SI unit of resistivity and molar conductivity are respectively ____________.
Which of the following graph represents the variation of `∧` with `sqrt"c"` for acetic acid solution?
What is the relation between cell constant, conductivity and electrical resistance?
What is the unit of electrical conductance?
If the conductivity of 0.08 M KCl solution is 2 × 10-2 Ω-1, what is the molar conductivity of the solution?
If the resistivity of 0.1 M KCI solution is 50 Ω cm, what is it's molar conductivity?
The value of [H3O+] in mol lit–1 of 0.001 M acetic acid solution (Ka = 1.8 × 10–5) is ______.
Which of the following has least conductivity in aqueous solution?
What is the SI unit of molar conductivity?
Explain the determination of molar conductivity of a weak electrolyte at infinite dilution or zero concentration using Kohlrausch's law.
