Q.What are the factors that affects electrolytic conductance ?

Electrolytic conductance is governed by how many ions are present and how freely they can move, so it depends on the nature and concentration of the electrolyte, temperature, solvent, and ionic mobility.

Factors affecting electrolytic conductance:

1. Nature of the electrolyte. Strong electrolytes (e.g. $KCl$, $NaOH$) are almost completely ionised in solution and so conduct much better than weak electrolytes (e.g. $CH_3COOH$, $NH_4OH$), which ionise only partially.

2. Concentration (dilution). Specific conductance ($\kappa$) decreases on dilution, because the number of ions per unit volume decreases; however, molar conductance ($\Lambda_m$) increases on dilution, because for a weak electrolyte the degree of dissociation increases, and even for a strong electrolyte interionic attractions decrease, allowing ions to move more freely.

3. Temperature. Conductance increases with increasing temperature, because the viscosity of the solvent decreases (ions move more freely) and, for weak electrolytes, the degree of dissociation also increases.

4. Nature of the solvent. A solvent with a high dielectric constant (like water) promotes greater ionisation of the electrolyte, and lower solvent viscosity allows faster ionic movement, both increasing conductance.

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