Solutions Chapter 15 Question Preview (ID: 1730)
Solutions, Molarity, Molality, Mole Fractions.
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Why can water dissolve NaCl, where as hexane cannot?
a) As a polar solvent, water is attracted to both anions and cations.
b) Hexane is attracted to the sodium ions, but not to the chlorine atoms.
c) Both water and salt are inorganic and hexane is organic.
d) water can form hydrogen bonds with NaCl.
The extent to which a solute dissolves in a solvent is determined by all of the following except
a) ambient pressure.
b) temperature.
c) stirring the mixture.
d) the type of intermolecular forces in the solute and solvent.
How do yu prepare a supersaturated solution?
a) Heat the solution and then add excess solute.
b) Choose a solute and a solvent with similar molecular structures.
c) Cool the solution quickly.
d) Heat the solution to the supersaturation point.
The rate at which a solid solute can be dissolved in a liquid solvent can be increased by
a) grinding the solute into small pieces.
b) lowering the temperature of the solvent.
c) increasing the air pressure on the liquid.
d) lowering the temperature of the solute.
All of the following are colligative properties except
a) chemical solubility.
b) boiling point elevation.
c) freezing point depression.
d) vapor pressure reduction.
Colligative properties of solutions depend on the
a) concentration of solute molecules dissolved.
b) chemical nature of the solute.
c) physical nature of the solute.
d) number of moles of solvent.
Which concentration unit is used when calculating colligative properties relating to boiling point elevation?
a) molality
b) molarity
c) mole fraction
d) weight percent
Receiving an injection of pure water would be painful because
a) osmotic pressure would cause cells to swell and burst.
b) the water would prevent blood from reaching cells.
c) water would leak out of the cells and cause them to wrinkle and die.
d) water is more concentrated than cell cytoplasm and would cause local weight increase.
Compared to the pure solvent, the boiling point of a solution is
a) increased because of the lowered vapor pressure of the solution.
b) increased because the solution has a higher osmotic pressure.
c) decreased because the solute boils at a higher temperature than the solvent.
d) decreased because the dissolved solute raises the vapor pressure of the solution over that of the solvent.
The molal freezing point constant, K,
a) is a specific effect of a solute on a given solvent.
b) varies with temperature and pressure.
c) has the same value as the boiling point constant.
d) is independent of the solute used in making the solution.
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