Question:
Molar conductivity ($\Lambda_{m}$) of aqueous solution of sodium stearate, which behaves as a strong electrolyte, is recorded at varying concentrations (c) of sodium stearate. Which one of the following plots provides the correct representation of micelle formation in the solution? (critical micelle concentration (CMC) is marked with an arrow in the figures)
Molar conductivity ($\Lambda_{m}$) of aqueous solution of sodium stearate, which behaves as a strong electrolyte, is recorded at varying concentrations (c) of sodium stearate. Which one of the following plots provides the correct representation of micelle formation in the solution? (critical micelle concentration (CMC) is marked with an arrow in the figures)
Updated On: Jun 14, 2022
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The Correct Option is C
Solution and Explanation
Sodium stearate $ \to CH_3(CH_2)_{16}COO^-Na^+$
At normal or low concentration, it behaves as strong electrolyte and for strong electrolyte, molar conductance $\left(\Lambda_{m}\right)$ decreases with increase in concentration.
But only above particular concentration sodium stearate forms aggregates that concentration is called as CMC. Since number of ions decreases, hence $\Lambda_{m}$ decreases.
At normal or low concentration, it behaves as strong electrolyte and for strong electrolyte, molar conductance $\left(\Lambda_{m}\right)$ decreases with increase in concentration.
But only above particular concentration sodium stearate forms aggregates that concentration is called as CMC. Since number of ions decreases, hence $\Lambda_{m}$ decreases.
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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.