Question

Why is the freezing point depression of 0.1 M KCl solution nearly twice that

of 0.1 M sucrose solution?​

Answer 1

Answer:

0.1M NaCl and0. 1M glucose solution means that 0.1 moles of solute dissolve in 1L of solvent. ... The depression in freezingpoint is inversly proprotional to molar mass of solute thus more is molar mass of solute lesser is the depression in freezing point .

Explanation:

hope it helps you

Answer 2

Answer:

The freezing point depression of $0.1 M KCl$ solution is nearly twice that of $0.1 M sucrose$ solution because the concentration after dissociation of $KCl$ in solution is twice the concentration of sucrose in solution. 

Explanation:

Given,

The molarity of $KCl$ = $0.1 M$

The molarity of sucrose = $0.1 M$

As we know,

• In an aqueous solution, $KCl$ dissociates:
• $KCl \rightarrow K^{+} + Cl^{-}$
• $0.1 M$    $0.1M$   $0.1M$

Therefore, the total concentration of $KCl$ (aq)  = $0.1 + 0.1$ = $0.2 M$

But,

• In an aqueous solution, sucrose does not dissociate:
• $sucrose \rightarrow sucrose (aq)$
• $0.1M$          $0.1M$

Therefore, the total concentration of $sucrose (aq)$ = $0.1M$

Thus, the molarity of the aqueous solution of $KCl$ is twice the molarity of the aqueous solution of sucrose.

As we know,

• The freezing point depression is directly proportional to the molarity of the solution.

Therefore,

• The freezing point depression of $0.1 M KCl$ solution is nearly twice that of $0.1 M sucrose$ solution.