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Solutions Chapter 15
Test Description: Solutions, molarity, molality, mole fractions
Instructions: Answer all questions to get your test result.
1) Why can water dissolve NaCl, where as hexane cannot?
A
As a polar solvent, water is attracted to both anions and cations.
B
water can form hydrogen bonds with NaCl.
C
Both water and salt are inorganic and hexane is organic.
D
Hexane is attracted to the sodium ions, but not to the chlorine atoms.
2) The extent to which a solute dissolves in a solvent is determined by all of the following except
A
stirring the mixture.
B
ambient pressure.
C
the type of intermolecular forces in the solute and solvent.
D
temperature.
3) How do yu prepare a supersaturated solution?
A
Choose a solute and a solvent with similar molecular structures.
B
Heat the solution to the supersaturation point.
C
Heat the solution and then add excess solute.
D
Cool the solution quickly.
4) 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
increasing the air pressure on the liquid.
C
lowering the temperature of the solvent.
D
lowering the temperature of the solute.
5) All of the following are colligative properties except
A
boiling point elevation.
B
vapor pressure reduction.
C
chemical solubility.
D
freezing point depression.
6) Colligative properties of solutions depend on the
A
number of moles of solvent.
B
chemical nature of the solute.
C
physical nature of the solute.
D
concentration of solute molecules dissolved.
7) Which concentration unit is used when calculating colligative properties relating to boiling point elevation?
A
molarity
B
molality
C
mole fraction
D
weight percent
8) Receiving an injection of pure water would be painful because
A
the water would prevent blood from reaching cells.
B
osmotic pressure would cause cells to swell and burst.
C
water is more concentrated than cell cytoplasm and would cause local weight increase.
D
water would leak out of the cells and cause them to wrinkle and die.
9) Compared to the pure solvent, the boiling point of a solution is
A
decreased because the solute boils at a higher temperature than the solvent.
B
increased because of the lowered vapor pressure of the solution.
C
decreased because the dissolved solute raises the vapor pressure of the solution over that of the solvent.
D
increased because the solution has a higher osmotic pressure.
10) The molal freezing point constant, K,
A
is independent of the solute used in making the solution.
B
is a specific effect of a solute on a given solvent.
C
varies with temperature and pressure.
D
has the same value as the boiling point constant.
*select an answer for all questions
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