Why is CH3COOH not conductive?
It is a weak electrolyte hence does not produce many ions on dissociation. So, it does not conduct electricity.
(a) The conductivity of 0.001 mol L−1 solution of CH3COOH is 3.905×10−5 Scm−1.
Description: Glacial acetic acid does not conduct electricity.
Glacial acetic acid does not dissociate enough to be able to conduct electricity.
Answer and Explanation: Acetic acid is a weak acid as suggested by its low dissociation constant. This low dissociation constant of acetic acid makes its ionization in an aqueous solution very limited. With this, it can be considered that acetic acid is a weak electrolyte.
Acetic acid (CH3COOH) ionises partially in water, hence, it is a weak acid. In other words, molecules of a weak acid ionises partially into corresponding ions, and the rest remain as simple acid molecules in water. The dissociation occurs as follows: CH3COOH(aq)⇋CH3COO−(aq)+H+(aq)
Yes, it does. Acetic acid disassociates into H+ and acetate ion in aqueous solution which are responsible for conducting electricity. Thanks!
A weak acid (e.g. CH3COOH) is in equilibrium with its ions in water and its conjugate (CH3COO–, a weak base) is also in equilibrium in water. For convenience the values are usually recorded as pKa or pKb values where pKa = -log Ka.
˄0m of Acetic acid (CH3COOH) can be calculated as. Q. The conductivity of 0.01 mol/dm3 aqueous acetic acid at 300 K is 19.5×10−5ohm−1cm−1 and the limiting molar conductivity of acetic acid at the same temperature is 390 ohm−1cm2mol−1.
Answer and Explanation: Based on the chemical equation, methanol can be classified as a non-electrolyte. It does not dissolve in aqueous solution to form ions. As a result, a solution of methanol does not conduct electricity.
Why limiting molar conductivity for CH3COOH Cannot be determined experimentally?
Why Limiting Molar Conductivity Of CH3COOH Cannot Be Determined Experimentally? The molar conductivity of CH3COOH cannot be determined experimentally because the molar conductivity of CH3COOH increases with the dilution. As dilution increases, obtaining a constant value becomes difficult.
The conductivity of dilute hydrochloric acid is greater than that of acetic acid. Acetic acid is weak electrolyte which dissociated partially whereas HCl is strong electrolyte which dissociates completely, therefore, HCl is better conductor compared to CH3COOH.