What is the freezing point of a 1 molal aque | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(D) The depression in freezing point is given by the formula: $\Delta T_{f} = K_{f} \cdot m$ Substituting the given values: $\Delta T_{f} = 1.86 \ K \

Vedclass · Accepted Answer

$-1.86$

Vedclass · Answer

(D) The depression in freezing point is given by the formula: $\Delta T_{f} = K_{f} \cdot m$ Substituting the given values: $\Delta T_{f} = 1.86 \ K \ kg \ mol^{-1} 	imes 1 \ mol \ kg^{-1} = 1.86 \ K$ Since the change in temperature in Celsius is the same as in Kelvin,$\Delta T_{f} = 1.86^{\circ} C$ The freezing point of the solution is calculated as: $T_{f} = T_{f}^{\circ} - \Delta T_{f}$ $T_{f} = 0^{\circ} C - 1.86^{\circ} C = -1.86^{\circ} C$

What is the freezing point of a $1 \ molal$ aqueous solution of a non-volatile solute (in $^{\circ} C$)? $(K_{f} = 1.86 \ K \ kg \ mol^{-1}, T_{f}^{\circ} \text{ for water } = 0^{\circ} C)$

Similar Questions

Which of the following has the minimum freezing point?

$50 \ g$ of antifreeze (ethylene glycol) is added to $200 \ g$ of water. What amount of ice will separate out at $-9.3 \ ^oC$? $(K_f = 1.86 \ K \ kg \ mol^{-1})$

Calculate the molar mass of a nonvolatile solute when $1.5 \ g$ of it is dissolved in $90 \ g$ of solvent,decreasing its freezing point by $0.25 \ K$. Given: $K_{f} = 1.2 \ K \ kg \ mol^{-1}$.

When a solution containing a non-volatile solute freezes,which equilibrium exists?

At $1 \ atm$ pressure,which of the following solutions will have the highest freezing point?

Vedclass Test Series

Exam Paper Generator

Online Exam Module