Question:
The molar conductance of NaCl, HCl and CH3COONa at infinite dilution are 126.45, 426.16 and 91.0 S cm2 mol−1 respectively. The molar conductance of CH3COOH at infinite dilution is. Choose the right option for your answer
The molar conductance of NaCl, HCl and CH3COONa at infinite dilution are 126.45, 426.16 and 91.0 S cm2 mol−1 respectively. The molar conductance of CH3COOH at infinite dilution is. Choose the right option for your answer
Updated On: May 5, 2024
540.48 S cm2 mol−1
201.28 S cm2 mol−1
390.71 S cm2 mol−1
698.28 S cm2 mol−1
Hide Solution
Verified By Collegedunia
The Correct Option is C
Solution and Explanation
The correct answer is option (C): 390.71 S cm2 mol−1
Was this answer helpful?
0
0
Top Questions on Electrochemistry
- Consider the concentration cell \[ \text{Pt} | \text{H}_2 (1 \, \text{bar}) | \text{HCl} (a_1) || \text{HCl} (a_2) | \text{H}_2 (1 \, \text{bar}) | \text{Pt} \] In concentration cells, the magnitude of liquid junction potential depends upon the transport number of cations and anions. For cells with \( a_2^+ \text{HCl} > a_1^+ \text{HCl} \), then the value of \( E_{ij} \) is negative when:
- CUET (PG) - 2025
- Chemistry
- Electrochemistry
- According to the moving boundary method, the transport number of the cation \( t_{\text{+}} \) of the principle electrolyte is calculated using the formula Given: \( l \) is the length by which the boundary has moved. The electrolyte of concentration \( c \) is kept in a long vertical tube with area of cross section \( A \).
- CUET (PG) - 2025
- Chemistry
- Electrochemistry
- Assertion (A): Electrolysis of aqueous NaCl gives H$_2$ at cathode and Cl$_2$ at anode.
Reason (R): Chlorine has higher oxidation potential than H$_2$O.- CBSE CLASS XII - 2025
- Chemistry
- Electrochemistry
- Calculate \( E_{\text{cell}} \) of a galvanic cell in which the following reaction takes place at 25°C:
\[ \text{Zn(s)} + \text{Pb}^{2+}(0.02M) \longrightarrow \text{Zn}^{2+}(0.1M) + \text{Pb(s)} \quad \text{[Given: } E^0_{\text{Zn}^{2+}/\text{Zn}} = -0.76V, \; E^0_{\text{Pb}^{2+}/\text{Pb}} = -0.13V, \; \log 2 = 0.3010, \; \log 4 = 0.6021, \; \log 5 = 0.6990 \text{]} \]- CBSE CLASS XII - 2025
- Chemistry
- Electrochemistry
- What is the standard electrode potential of a half-reaction in which electrons are transferred from \(Ag^+\) to \(Ag\)?
- VITEEE - 2025
- Chemistry
- Electrochemistry
View More Questions
Concepts Used:
Electrolysis
Electrolysis:
Electrolysis is the process by which an element is decomposed and undergoes some chemical change under the influence of any electric current. The first-ever electrolysis was executed out by Sir Humphrey Davey in the year 1808. Electrolysis can occur in both Galvanic cells and Electrolytic cells.
Applications of Electrolysis:
- Electrolytic cells are used for the production of Hydrogen and Oxygen gas from water.
- They are used for the large-scale production of pure metals like sodium, copper, magnesium, etc.
- They are used to extract Aluminium from Bauxite.
- Electrolytic cells are used for electroplating, a process by which a thin protective layer of one metal is formed over another metal, mostly for protection.
- Electrolysis is used for the electrorefining of non-ferrous metals.
Read More: Products of Electrolysis