CHM142 Questions And Answers Latest Top Score.
Fog
Lemonade with Pulp
Salt water
A cup of hot tea - correct answer. There are three types of mixtures that involve a solute dissolving into a solvent: solutions, colloids, and suspensions.
The size of the solute, or the p...
A cup of hot tea - correct answer. There are three types of mixtures that involve a
solute dissolving into a solvent: solutions, colloids, and suspensions.
The size of the solute, or the particle being dissolved, determines whether the resulting
mixture is a solution, colloid, or suspension.
Which of the following is an example of a colloid?
20 g
5g
10 g
30 g - correct answer. The solubility of solids is affected by temperature while the
solubility of gases is affected by both temperature and pressure.
The Solubility of Solids
The solubility of a solid solute increases with increasing temperature because the
thermal energy helps to overcome the attractions between solute molecules in the solid.
The Solubility of Gases
The solubility of a gaseous solute decreases with increasing temperature because the
thermal energy helps to overcome the attractions between solute and solvent
molecules. The solubility of a gaseous solute increases as pressure of the solute gas
, above the solution is increased because a higher pressure means that more gas
molecules are present near the surface of the solution and able to dissolve.
How much KNO3 can dissolve in 50 g of water at 10 °C?
CH3OH (methanol, polar)
BF3 (Boron trifluoride, nonpolar)
CCl4 (carbon tetrachloride, nonpolar)
C4H10 (butane, nonpolar) - correct answer. There must be a strong attraction
between the solute and the solvent molecules in order for the solute to dissolve in the
solvent allowing a solution to form.
Which substance will dissolve in water, a polar substance?
8.84 g glucose/108.84 g solution
8.84 g glucose/91.16 g solution
8.84 g glucose/100 g solution
8.84 g glucose/100 g water - correct answer. Which expression is equivalent to
8.84% (m/m) glucose?
3.6 °C
-3.6 °C
10.1 °C
-10.1 °C - correct answer. Colligative properties of solutions depend only on the
number of particles dissolved in a solvent. The higher the number of dissolved solute
particles, the larger the effect on the boiling point, melting point, vapor pressure, and
osmotic pressure.
What is the freezing point of 0.500 m I2 in cyclohexane (normal freezing point = 6.55
°C)? Kf,cyclohexane = 20.2 °C/m
0.690
0.310
0.136
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