Statement-1 : The difference in the boiling points of equimolar solution of HCl and HF decreases as their molarity is decreased.Statement-2 : The extent of dissociation decreases steadily with increasing dilution.a)Statement-1 is True, Statement-2 is True; Statement-2 is a correct explanation for Statement-1.b)Statement-1 is True, Statement-2 is True; Statement-2 is NOT a correct explanation for Statement-1c)Statement-1 is True, Statement-2 is Falsed)Statement-1 is False, Statement-2 is TrueCorrect answer is option 'C'. Can you explain this answer?

Question

Answer

Statement-1: The difference in the boiling points of equimolar solution of HCl and HF decreases as their molarity is decreased.
Statement-2: The extent of dissociation decreases steadily with increasing dilution.

Explanation:
To understand the relationship between the boiling points of equimolar solutions of HCl and HF, and their molarity, let's analyze the statements:

Statement-1: The difference in the boiling points of equimolar solution of HCl and HF decreases as their molarity is decreased.
The boiling point of a solution depends on the strength of the intermolecular forces between the solute particles. In the case of HCl and HF, both are polar covalent compounds, but HF has stronger intermolecular forces due to hydrogen bonding. As a result, HF has a higher boiling point than HCl.

When we prepare an equimolar solution of HCl and HF, the boiling point of the solution will be closer to the boiling point of HF due to its stronger intermolecular forces. However, as the molarity of the solution is decreased, the number of solute particles decreases, leading to a decrease in the strength of intermolecular forces. Consequently, the boiling point of the solution decreases.

Statement-2: The extent of dissociation decreases steadily with increasing dilution.
Dissociation refers to the process in which solute particles separate into ions in a solution. The extent of dissociation can be measured by the degree of ionization, which is the ratio of the number of dissociated particles to the total number of solute particles.

When a solution is diluted, the number of solute particles decreases while the volume of the solution increases. As a result, the concentration of the solute decreases, which leads to a decrease in the extent of dissociation. This decrease in dissociation is more prominent for weak electrolytes like HCl and HF, as they have a lower degree of ionization compared to strong electrolytes.

Explanation of the relationship between the two statements:
Statement-2 provides a logical explanation for Statement-1. As the molarity of the solution decreases, the extent of dissociation decreases, leading to a decrease in the number of solute particles and a decrease in intermolecular forces. This decrease in intermolecular forces ultimately results in a decrease in the boiling point of the solution.

Therefore, both Statement-1 and Statement-2 are true, and Statement-2 provides a correct explanation for Statement-1. Hence, the correct answer is option (a) Statement-1 is True, Statement-2 is True; Statement-2 is a correct explanation for Statement-1.

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