Calculate the freezing point of a solution when 31 gram of Ethylene glycol is dissolved in 500 gram of water. (

Kf for water=1.86 k kg /mol

Q. The freezing point of a solution containing 28.335 $c{m}^3$ of ethylene glycol in 50 g water is found to be $–{34}^{\circ }$ C. Assuming ideal behaviour, calculate the density of ethylene glycol. $K_f$ for water 1.86 K kg $mo{l}^{-1}$.___

Q. Value of kf of water is 1.86 k g mole ^-1 if your vehicles radiator can accommodate 1kg of water then how many grams of ethylene glycol can be dissolved in it so that freezing point of solution becomes -2.8 degree Celsius

Q. $K_f$ for water is $1.86Kkgmo{l}^{-1}$. Your automobile radiator holds 1.0 kg of water, how many grams of ethylene glycol $\left(C_2{H}_6{O}_2\right)$ must you add to get the freezing point of the solution lowered to $-{2.8}^{o}C$?

Q. Ethylene glycol is used as an antifreeze in a cold climate. Mass of ethylene glycol which should be added to 4 kg of water to prevent it from freezing at $-6^{o}C$ will be $(K_f$ for water $=1.86Kkg$ $mo{l}^{-1}$, and molar mass of ethylene glycol $=62gmo{l}^{-1}$)

Q. $45$g of ethylene glycol $\left(C_2{H}_6{O}_2\right)$ is mixed with $600$g of water. The freezing point of the solution is ($K_f$ for water is $1.86$K kg $mo{l}^{-1}$).