Exams › NEET › Chemistry

Given specific conductance of the solution (κ) = 0.012 ohm⁻¹ cm⁻¹ and resistance (R) = 55 ohm. We know that cell constant = Specific conductance × Observed resistance = 0.012 × 55 = 0.66 cm⁻¹.

1. λ°Na⁺ + λ°Cl⁻ = 126.45
2. λ°Na⁺ + λ°Cl⁻ = 426.16
3. λ°CH₃COO⁻ + λ°Na⁺ = 91
4. λ°CH₃COONa = 390.71 ohm⁻¹ cm²

Correct answer: λ°CH₃COONa = 390.71 ohm⁻¹ cm²

Solution

The cell constant is calculated correctly as 0.66 cm⁻¹, and the given data aligns with the molar conductivity of CH₃COONa. Option D is consistent with the provided values.

Related NEET Chemistry questions

• Assertion: When an electric current is passed through the copper sulphate electrolyte, the impure copper anode gradually dissolve and pure copper is deposited on the cathode. Reason: Pure metals are deposited in electroplating techniques.
• What is the electric current required to deposit 0.972 g of chromium in three hours? (E.C.E. of chromium is 0.00018 g/c)
• Which of the following statement (s) differentiate between electrochemical cell and electrolytic cell? This question has multiple correct options
• Among the following, the couple with most positive reduction potential is :
• The resistance of \( 1 \mathrm{N} \) solution of acetic acid is \( 250 \Omega \) when measured in a cell having a cell constant of \( 1.15 \mathrm{cm}^{-1} . \) The equivalent conduction (in oh \( m^{-1} c m^{2} e q u i v^{-1} \) ) of \( 1 N \) acetic acid is
• If \( 9 g m H_{2} O \) is electrolysed completely with the current of \( 50 \% \) efficiency then :

⚔️ Practice NEET Chemistry free + battle 1v1 →