Chemistry: Water and Solution, Chemistry 1 homework help

QUESTION 1

When you accidentally overfill a water glass, the water takes on a dome-like or convex shape, but a half-filled water glass takes on a concave shape, in which the water is higher at the sides of the glass. This is because:

Within the glass, adhesive forces dominate, and on top of the glass, cohesive forces dominate.

Within the glass, water tries to maximize its surface area, and on top of the glass, water tries to minimize its surface area.

Water’s surface tension is greater inside the glass than on top of the glass.

Adhesive forces between water and the glass get weaker with height.

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QUESTION 2

Water’s ability to dissolve many ionic and covalent substances is based on water’s:

melting point

electrical conductivity

molecular shape and polarity

surface tension

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QUESTION 3

The phrase that best describes the solution process is:

‘opposites attract’

‘like dissolves like’

‘water dissolves everything’

‘when in doubt, stir it about’

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QUESTION 4

For which of the following solutions would an increase in pressure result in an increase in solubility of a solute?

gas

liquid

solid

gases, liquids and solids

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QUESTION 5

If two solutions have the same solvent, concentration, pressure, temperature, and molecular polarity, then:

The solubility of the two solutions are identical as well.

The solution with the smaller particle size is generally more soluble.

The identities of the solutes are not relevant.

Their solubility will remain the same under all conditions.

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QUESTION 6

Match each example to the type of solution.

supersaturated solution

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unsaturated solution

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saturated solution

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Answer

A.

An Dissolving 37 grams of sodium chloride in 100 grams of water, at 25 degrees Celsius, when the maximum sodium chloride soluble at that temperature is 37 grams.

B.

The percentage of salt in ocean water.

C.

Carbon dioxide dissolved in a can of soda.

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QUESTION 7

When the compound, Na2S, is mixed with water, the Na2S is:

soluble because all Na+1 compounds are soluble in water

insoluble because most Na+1 compounds are insoluble in water

soluble because all S−2 compounds are soluble in water

insoluble because there are no water soluble S−2 compounds

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QUESTION 8

When the compound, PbCl2, is mixed with water, the PbCl2 is:

soluble because all Cl− compounds are soluble in water

insoluble because most compounds are insoluble in water

soluble because all Pb+2 compounds are soluble in water

insoluble because when Pb+2 and Cl− combine, the resultant compound is insoluble

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QUESTION 9

In the reaction between CaS (aq) and LiNO3 (aq), will a precipitate form?

No. This reaction produces no insoluble products.

Yes. Ca(NO3)2 will precipitate.

Yes. The Li2S will precipitate.

Yes. Both the Ca(NO3)2 and the Li2S will precipitate.

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QUESTION 10

In the double replacement reaction between K2CO3 (aq) and NiCl2 (aq), will a precipitate form?

No. All products are soluble.

Yes. The KCl will form a precipitate.

Yes. The NiCO3 will form a precipitate.

Yes. Both the KCl and the NiCO3 will form precipitates.

1. If 2.0 moles of a substance are dissolved in 2.0 liters of solution, then the molarity of this solution is:
   

   		0.5 M
   		1.0 M
   		1.5 M
   		2.0 M

3 points

QUESTION 2

1. Vinegar is commonly sold as a 5 percent (v/v) solution of acetic acid in water. This measurement means which of the following?
   

   		5 grams of acetic acid/100 grams of solution
   		5 grams of acetic acid/100 grams of water
   		5 mL of acetic acid/100 mL of solution
   		5 mL of acetic acid/100 mL of water

3 points

QUESTION 3

1. If a given solution has a 30 percent solute concentration, and more solute is added to the solution, the new solute concentration could be:
   

   		50%
   		25%
   		10%
   		5%

3 points

QUESTION 4

1. A common stain remover is sold in concentrated form as 1.8M sodium hypochlorite (NaOCl). For everyday use, you create 2.2 liter of a more dilute solution by dissolving 0.015 liters of the 1.8M solution in water. What is the concentration of this new solution?
   

   		0.012M
   		0.18M
   		1.4M
   		2.64M

3 points

QUESTION 5

1. Properties of a solution that depend only on the ratio of the number of particles of solute and solvent in the solution are known as:
   

   		intensive properties
   		extensive properties
   		colligative properties
   		chemical properties

3 points

QUESTION 6

1. How does adding a non-volatile solute to a pure solvent affect the freezing point of the pure solvent?
   

   		The solvent will have a lower freezing point.
   		The solvent will have a higher freezing point.
   		The solvent’s freezing point will not be affected.
   		The solvent’s freezing point will most likely change, but not in a predictable way.

3 points

QUESTION 7

1. Why are concentration units of mole fraction used in some colligative properties calculations?
   

   		Mole fraction expresses concentration more accurately than molarity.
   		Mole fraction does not depend on the chemical identity of the solute.
   		Mole fraction is easier to measure in the laboratory than molarity or molality.
   		Mole fraction is not affected by changes in temperature.

3 points

QUESTION 8

1. What is the molality of an aqueous sucrose solution that boils at 102.0 degrees Celsius? The boiling point elevation constant for water is 0.512 degrees Celsius per mole.
   

   		1.02 m
   		2.00 m
   		2.51 m
   		3.91 m

3 points

QUESTION 9

1. What would be the freezing point for a 2.6 mole aqueous sucrose solution? The freezing point depression constant for water = 1.86 °C/m.
   

   		4.8 °C
   		– 1.4 °C
   		0.72 °C
   		– 4.8 °C

3 points

QUESTION 10

1. A 300 gram sample of pure water exerts a vapor pressure of 750 millimeters of mercury on the walls of its container. If 0.27 moles of glucose (C₆H₁₂O₆) is added to the water, what will be the vapor pressure of the resulting solution?
   

   		0.984 mm Hg
   		12.1 mm Hg
   		738 mm Hg
   		748 mm Hg