Depression of Freezing Point — MCQ Practice

A solution is prepared by dissolving $1.8,\text{g}$ of glucose (molar mass $180,\text{g/mol}$) in $100,\text{g}$ of water. The cryoscopic constant for water ($K_f$) is $1.86,\text{K kg/mol}$. What is the depression in freezing point of the solution?

Which of the following $0.1,\text{m}$ aqueous solutions will have the lowest freezing point? (Assume complete dissociation for electrolytes)

An aqueous solution freezes at $-0.372^circ C$. If $K_f$ for water is $1.86,\text{K kg/mol}$, what is the molality of the solution?

A $5$ (w/w) aqueous solution of a non-electrolyte has a freezing point of $-1.0^circ C$. If $K_f$ for water is $1.86,\text{K kg/mol}$, what is the molar mass of the solute?

Which of the following statements about depression of freezing point is INCORRECT?

What is the freezing point of a solution containing $10.0,\text{g}$ of MgCl$_2$ (molar mass $95.2,\text{g/mol}$) in $200,\text{g}$ of water? Assume complete dissociation and $K_f$ for water is $1.86,\text{K kg/mol}$.