Categorize (1) milk, (2) whipped cream and (3) fog as emulsion, foam or aerosol.
Explain how and why the presence of a solute affects the freezing point of a solvent.
Rank and explain how the freezing point of 0.100 m solutions of the following ionic electrolytes compare. List from lowest freezing point to highest freezing point.
MgI2 ,AlCl3, Mg3(PO4)2, NaI
Show the calculation of the mass percent solute in a solution of 20.8 grams of Ba(NO3)2 in 400 grams of water. Report your answer to 3 significant figures.
Show the calculation of the molality of a solution made by dissolving 24.5 grams of C4H8O4 in 400 grams of water. Report your answer to 3 significant figures.
Show the calculation of the molarity of a solution made by dissolving 35.9 grams of Mg(NO3)2 to make 400 ml of solution. Report your answer to 3 significant figures.
Show the calculation of the mass of Ca3(PO4)2 needed to make 350 ml of a 0.150 M solution. Report your answer to 3 significant figures.
Show the calculation of the volume of 0.827 M solution which can be prepared using 26.4 grams of Ca3(PO4)2.
Show the calculation of the freezing point of a solution made by dissolving 15.6 grams of the nonelectrolyte C3H6O3 in 200 grams of water. Kf for water is 1.86, freezing point of pure water is 0oC. Calculate your answer to 0.01oC.
Show the calculation of the molar mass (molecular weight) of a solute if a solution of 14.6 grams of the solute in 200 grams of water has a freezing point of -1.35oC. Kf for water is 1.86 and the freezing point of pure water is 0oC. Calculate your answer to 0.1 g/mole.