Ethylene glycol (OH—CH2—CH2—OH) is used as an antifreeze. (Its boiling point is 197 ◦C and freezing point is –17.4 ◦C.)(a) Look up the density of ethylene glycol in the CRC Handbook or other tables and write a general formula for the freezing point of a mixture of X mL of ethylene glycol in 1.00 L of water for X in the range 0–100 mL.(b) If the lowest expected temperature is about –10 ◦C, what is the minimum amount of ethylene glycol (milliliters ethylene glycol per liter of H2O) you need in your coolant?(c) What is the boiling point of the coolant that contains 300 mL of ethylene glycol per liter of water?

Straightforward questions answered in the powerpoint slidesreaction: heating the starting materials under refluxwhat does it mean to heat under reflux? why do we choose water as the reflux solvent? what are boiling chips used for? why do we put a condenser on top of the reaction? why do we add heat and let the reaction stir for 30 minutes? why do we add sulfuric acid to the reaction after it cools as opposed to when it’s still hot? separation: filtration of precipitatewhy don’t we do an aqueous and organic extraction in the separatory funnel? why do you rinse the salicylic acid on the filter with ice cold water? purification: recrystallization of salicylic acid (no hot filtration needed)what is the difference in the amount of room temperature water vs. boiling water needed to dissolve the salicylic acid (assume a 1.2 gram yield of salicylic acid)? remember, in the lab if you need x ml of boiling water to dissolve a solid, then you should add a little more (definitely no more than 1.5 times the theoretical amount) to ensure it doesn’t recrystallize prematurely.analysis: melting point of salicylic acidwhat can you conclude if the melting point of the salicylic acid you just synthesized is 152-155oc and the 1: 1 mix of your product and “synthetic” salicylic acid is 151-154oc?