Define or describe:
(a) Amorphous solid (k) Molality
(b) Colligative property (l) Molarity
(c) Colloid (m) Nonelectrolyte
(d) Condensation (n) Phase
(e) Critical point (o) Strong electrolyte
(f) Critical pressure (p) Sublimation
(g) Crystalline solid (q) Surface tension
(h) Electrolyte (r) Triple point
(i) Fluid (s) Vapor pressure
(j) Ionization (t) Weak electrolyte
What rule is used to predict the solubility of materials?
Explain how and why the presence of a solute affects the boiling point of a solvent.
Calculate the mass percent solute in a solution of 12.6 grams of NaNO3 in 450 grams of water.
Show the calculation of the molality of a solution made by dissolving 12.6 grams of NaNO3 in 200 grams of water.
Show the calculation of the molarity of a solution made by dissolving 12.6 grams of NaNO3 to make 200 ml of solution.
Show the calculation of the mass of NaNO3 needed to make 450 ml of a 0.356 M solution.
Show the calculation of the volume of 0.987 M solution which can be prepared using 24.6 grams of NaNO3.
Show the calculation of the freezing point of a solution made by dissolving 12.6 grams of the nonelectrolyte C2H5OH in 200 grams of water. Kf for water is 1.86, FP of pure water is 0oC.
Show the calculation of the freezing point of a solution made by dissolving 12.6 grams of the electrolyte NaNO3 in 200 grams of water. Kf for water is 1.86 and the FP of pure water is 0oC.
Show the calculation of the molar mass (molecular weight) of a solute if a solution of 5.8 grams of the solute in 100 grams of water has a freezing point of -1.20oC. Kf for water is 1.86 and the FP of pure water is 0oC.
How would the FP of 0.100 m solutions of the following ionic electrolytes compare? Rank from lowest FP to highest FP.
AlCl3, Ca3(PO4)2, KCl, CaCl2