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100 mL of a 1.0 M sugar solution. When thesystem comes to equilibrium,1.all of the water will be in the sugar solu-tion.2.the beaker with the sugar solution willhave a larger volume.correct3.the beaker with the salt solution will havea larger volume.4.the two beakers will have identical vol-umes.5.all of the water will be in the salt solu-tion.Explanation:Both liquids will evaporate and condensefrom each beaker.The chamber will cometo equilibrium when the two beakers havethe same concentration (same vapor pres-sure).The salt solution will become moreconcentrated (lower volume) and the sugar so-lution will become less concentrated (highervolume).01610.0 points
gonzales (pag757) – Homework #2 – Holcombe – (52460)5Which of the following two solutions willachieve the greatest boiling point increase andwhat will the new temperature be?AssumethatKb= 0.52◦C/m for water.Explanation:First calculate the molality of each solution,which is mol solute per kg solvent.To dothis, you will need to convert from mass tomols, using molar mass. Remember also thati= 2 for NaCl andi= 1 for sucrose. UsingΔT=imKbyou will find that ΔT= 0.32◦Cfor the sucrose solution and 1.25 for the saltsolution, which means the boiling point of thesalt solution will be 101.25◦C.01710.0 points30.2 g of glycerine (C3H8O3) are dissolved in150 g of water. What is the boiling point ofthe solution? (◦C.What is the molality of the solution? Assumethat there is no dissociation of the solute andthatkfis 1.68 K·kg/mol.3.3.44m4.0.995m5.0.497mcorrectExplanation:01910.0 pointsAnaqueoussolutionfreezesat-5.44