Advertisements
Advertisements
प्रश्न
Answer the following in brief.
Explain the effect of dilution of the solution on conductivity.
Advertisements
उत्तर
- The electrolytic conductivity is the electrical conductance of unit volume (1 cm3) of solution. It depends on the number of current-carrying ions present in unit volume of solution.
- On dilution total number of ions increases as a result of an increased degree of dissociation.
- An increase in the total number of ions is not in the proportion of dilution. Therefore, the number of ions per unit volume of solution decreases.
- This results in a decrease of conductivity with a decrease in the concentration of the solution.
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.
Choose the most correct option.
Two solutions have the ratio of their concentrations 0.4 and ratio of their conductivities 0.216. The ratio of their molar conductivities will be ______.
What is a cell constant? What are its units? How is it determined experimentally?
Answer the following in one or two sentences.
Write the relationship between conductivity and molar conductivity and hence unit of molar 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 _______.
The molar conductivity and conductivity of AgNO3 solution is 121.4 Ω–1 cm2 mol–1 and 2.428 × 10–3 Ω–1 cm–1 at 25 °C. What is molar concentration of AgNO3 solution?
Write applications of Kohlrausch’s Law.
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 CORRECT unit of molar conductivity is ____________.
The molar conductance of 0.001 M acetic acid is 50 ohm−1 cm2 mol−1. The limiting molar conductance is 250 ohm−1 cm2 mol−1. What is its degree of ionization?
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 SI unit of resistivity and molar conductivity are respectively ____________.
The resistance of a conductivity cell containing 0.001 M KCl solution at 298 K is 1500 Ω. What is the cell constant if conductivity of 0.001 M KCI solution at 298 K is 0.146 × 10−3 S cm−1?
The distance between electrodes of a conductivity cell is 0.98 cm and area of cross section is 1.96 cm2. What is the cell constant?
If the conductivity of 0.08 M KCl solution is 2 × 10-2 Ω-1, what is the molar conductivity of the solution?
A conductivity cell dipped in 0.5 M KCl gives a resistance of 250 ohms. If the conductivity of KC I solution is 6.68 × 10-3 S cm-1, what is the cell constant?
Which of the following has least conductivity in aqueous solution?
Explain the determination of molar conductivity of a weak electrolyte at infinite dilution or zero concentration using Kohlrausch's law.
Define the term cell constant.
Write the relation between molar conductivity and molar ionic conductivities for the electrolytes:
- Na2SO4
- AlCl3
