The specific conductance of 0.01 M aqueous solution of acetic acid is 1. 63 x10-2 S m-1 and the molar conductance at infinite dilution is 390.7x10-4 S m2 mol-1.Calculate the degree of dissociation of the acetic acid solution?
The specific conductance of 0.01 M aqueous solution of acetic acid is 1. 63 x10-2 S m-1 and the molar conductance at infinite dilution is 390.7x10-4 S m2 mol-1.Calculate the degree of dissociation of the acetic acid solution?
0.4
0.239
0.0417
0.0239
The Correct Option is C
Solution and Explanation
To calculate the degree of dissociation (α) of the acetic acid solution, we'll follow these steps:
1. Given Data:
- Specific conductance (κ) = 1.63 × 10-2 S m-1
- Molar concentration (c) = 0.01 M = 0.01 × 103 mol m-3 = 10 mol m-3
- Molar conductance at infinite dilution (Λ0) = 390.7 × 10-4 S m2 mol-1
2. Calculate Molar Conductance (Λm):
Molar conductance is given by:
Λm = κ / c
= (1.63 × 10-2 S m-1) / (10 mol m-3)
= 1.63 × 10-3 S m2 mol-1
3. Calculate Degree of Dissociation (α):
The degree of dissociation is given by:
α = Λm / Λ0
= (1.63 × 10-3 S m2 mol-1) / (390.7 × 10-4 S m2 mol-1)
= (1.63 × 10-3) / (3.907 × 10-2)
= 0.0417 or 4.17%
4. Interpretation:
The low degree of dissociation (4.17%) indicates that acetic acid is a weak electrolyte, as expected, with only a small fraction of molecules dissociated into ions at this concentration.
Final Answer:
The degree of dissociation of the 0.01 M acetic acid solution is 0.0417 (or 4.17%).
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Concepts Used:
Electrochemical Cells
An electrochemical cell is a device that is used to create electrical energy through the chemical reactions which are involved in it. The electrical energy supplied to electrochemical cells is used to smooth the chemical reactions. In the electrochemical cell, the involved devices have the ability to convert the chemical energy to electrical energy or vice-versa.
Classification of Electrochemical Cell:
Cathode
- Denoted by a positive sign since electrons are consumed here
- A reduction reaction occurs in the cathode of an electrochemical cell
- Electrons move into the cathode
Anode
- Denoted by a negative sign since electrons are liberated here
- An oxidation reaction occurs here
- Electrons move out of the anode
Types of Electrochemical Cells:
Galvanic cells (also known as Voltaic cells)
- Chemical energy is transformed into electrical energy.
- The redox reactions are spontaneous in nature.
- The anode is negatively charged and the cathode is positively charged.
- The electrons originate from the species that undergo oxidation.
Electrolytic cells
- Electrical energy is transformed into chemical energy.
- The redox reactions are non-spontaneous.
- These cells are positively charged anode and negatively charged cathode.
- Electrons originate from an external source.