The freezing point depression of a solvent is directly proportional to the molality of the solute. Therefore, the number of moles of the solute required to achieve the same freezing point lowering as 5.0 mol of ethylene glycol in 1 kg of water is 5.0 mol.
Thus, 5.0 moles of CH3−OH and 5.0 moles of KNO3 are needed to give the same freezing point lowering as 5.0 mol of ethylene glycol in 1 kg of water.
How many moles of each of the following are needed to give the same freezing point lowering as 5.0mol of the nonelectrolyte ethylene glycol in 1 kg of waterCH3−OH, a non electrolyte,KNO3, a strong electrolyte
I am so lost with what they exactly want for this?
1 answer
1 answer