Colligative Properties - CORRECT ANSWER-properties of solution, such as freezing
point and boiling point, which depend on the concentration of solute
... [Show More] particles dissolved
in the solvent
Freezing Point Depression Equation - CORRECT ANSWERMolality - CORRECT ANSWER-moles of solute per kg of solvent
Molality= - CORRECT ANSWERWhat is the definition of colligative properties? (Antifreeze) - CORRECT ANSWERproperties of a solution that depend on the concentration of solute dissolved in the
solvent
What is the difference between solute and solvent? (Antifreeze) - CORRECT ANSWERThe solute is what is dissolved, and the solvent is what is doing the dissolving.
What is the difference between molality and molarity? (Antifreeze) - CORRECT
ANSWER-molality=mol/kg
molarity=mol/L
What is the difference between freezing point and melting point? (Antifreeze) -
CORRECT ANSWER-There is no difference between the melting point and boiling
point. The freezing point and boiling point depends on the direction of the reaction --
whether a solid or liquid is being formed.
An antifreeze solution contains 25 mL of ethylene glycol and 75 mL of water. What is
the molality of the solution? (density of H2O = 1.00 g/mL and density of C2H4(OH)2 =
1.11 g/mL) (Antifreeze) - CORRECT ANSWER-5.96 m
What will be the freezing point of the antifreeze solution in the question above?
(Antifreeze)
V of C2H4(OH)2 (mL): 25 mL
V of H2O (mL): 75 mL
Density of H2O (g/mL): 1.00 g/mL
Density of C2H4(OH)2 (g/mL): 1.11 g/mL
Kf of H2O: 1.86 *C/m
Tf of H2O: 0 *C - CORRECT ANSWER--11.09 *C
A different antifreeze solution contains 45 mL of ethylene glycol and 55 mL of water.
What will be the freezing point of this new solution? (Antifreeze)
Density of H2O (g/mL): 1.00 g/mL
Density of C2H4(OH)2 (g/mL): 1.11 g/mL
Kf of H2O: 1.86 *C/m
Tf of H2O: 0 *C - CORRECT ANSWER--27 *C
Based on your results, which of the following antifreeze solutions will be the best at
protecting your radiator from freezing? (Antifreeze)
A. 100% water
B. 2 m ethylene glycol
C. 12 m ethylene glycol
D. pure ethylene glycol - CORRECT ANSWER-C. 12 m ethylene glycol
Some students mislabeled their test tubes. The test tube really contained 2.5 mL of
ethylene glycol instead of 2.0 mL. Will this affect the observed experimental melting
point? If so, will this melting point be higher or lower than expected? Explain your
answer. (Antifreeze) - CORRECT ANSWER-If the test tube contained 2.5 mL of
ethylene glycol instead of 2.0 mL, the melting point will be lower than expected because
the more concentrated the ethylene glycol solution is, the lower the melting point of the
solution.
Regular thermometers are filled with mercury. Mercury freezes at -39 *C. Can regular
thermometers be used for this experiment? Explain your answer. (Antifreeze) -
CORRECT ANSWER-Regular thermometers could not be used for this experiment [Show Less]