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Chemistry 400 > Chapter 13 solutions > Flashcards

Chapter 13 solutions Flashcards

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1
Q

Solution

A

A homogeneous mixture of two or more substances

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2
Q

Solvent

A

The component of a solution that is present in greatest amount

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3
Q

Solute

A

A component of a solution that is present in a lesser amount

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4
Q

Soluble

A

A compound is soluble if it dissolves in a solvent

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5
Q

Insoluble

A

A compound is insoluble if it does not dissolve in a solvent.

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6
Q

Miscible

A

Two substances that are soluble in all proportions are miscible

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7
Q

Dilute Solution

A

A solution that contains a low quantity of solute

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8
Q

Concentrated Solution

A

A solution that contains a high quantity of solute

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9
Q

Unsaturated solution

A

Solution that holds less than the maximum amount of solute possible

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10
Q

Saturated solution

A

Solution that holds the maximum amount of solute possible

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11
Q

Supersaturated solution

A

A solution that holds more than the amount of solute possible

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12
Q

Ion-Dipole Force

A

Intermolecular force between an ion and a polar molecule.

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13
Q

Henry’s law

A

Solubility of a gas is directly proportional to the pressure of the gas above the liquid

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14
Q

Like Dissolves Like

A

General rule to predict the solubility of molecular compounds. Polar solutes
dissolve in polar solvents, and non-polar solutes dissolve in non-polar solvents.

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15
Q

Concentration

A

Describes the amount of solute in a solution.

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16
Q

Molarity

A

The number of moles per liter of solvent. Often used as a conversion factor to convert
between volume and moles

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17
Q

Molality

A

The number of moles per kilogram of solvent

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18
Q

Mole fraction

A

The number of moles of a solute divided by the total number of moles in a solution

19
Q

Percent concentration

A

Solute divided by solution, multiplied by 100

20
Q

Parts per million (ppm)

A

Solute divided by solution, multiplied by 1 million (10^6)

21
Q

Parts per billion (ppb)

A

Solute divided by solution, multiplied by 1 billion (10^9)

22
Q

Dilution

A

The process of adding solvent to decrease the concentration of a solution

23
Q

Electrolyte solution

A

Solution that conducts electricity

24
Q

Electrolyte

A

A substance that conducts electricity when dissolved in water

25
Q

Non-Electrolyte

A

A substance that does not conduct electricity when dissolved in water

26
Q

Colligative properties

A

Properties that depend on the number of particles dissolved in a solution, and
not the identities of the particles themselves

27
Q

Ion pairing

A

Cations and anions get close enough to each other to effectively pair. This lowers the
concentration of particles below what is expected from the complete dissociation of ionic compounds

28
Q

van’t Hoff Factor

A

The ratio between the amount of particles produced and the amount of solute
dissolved. In this class, we assume all solutions are ideal solutions and ion pairing does not occur.

29
Q

Freezing Point Depression

A

Solutes cause the freezing point of a solution to be lower than that of the
pure solvent

30
Q

Boiling Point Elevation

A

Solutes cause the boiling point of a solution to be higher than that of the pure
solvent

31
Q

Osmosis

A

The flow of water toward a more concentrated solution through a semipermeable membrane

32
Q

Semipermeable Membrane

A

Membrane that allows water and other small molecules to pass through,
but blocks the passage of large molecules and ions

33
Q

Osmotic Pressure

A

The pressure required to stop osmosis

34
Q

Vapor Pressure

A

The partial pressure of a gas in dynamic equilibrium with its liquid

35
Q

Volatile

A

Something that vaporizes easily

36
Q

Non-Volatile

A

Something that does not vaporize easily

37
Q

Give an example of a solid in liquid solution

A

Saltwater - NaCl in water

38
Q

Give an example of a solid in solid solution

A

Brass - Alloy of copper and zinc

39
Q

Give an example of a gas in gas solution

A

Air - O2, CO2, Ar, and other gases in N2
Common Types of Solutions

40
Q

Name 3 solutes in a can of soda

A

Sugar, CO2, food coloring, …

41
Q

To answer the questions below, suppose a crystal of NaCl is dissolving in a beaker full of water.

a) What force is holding the atoms together in the NaCl crystal?

b) What force is holding the water molecules together in the beaker?

c) What force is causing the NaCl crystal to dissolve in the water?

A

a) Electrostatic attraction

b) Hydrogen bonding

c)The ion-dipole force

42
Q

In general, the solubility of solids ______ with increasing temperature

A

increase

43
Q

In general, the solubility of gases _______ with increasing temperature.

A

decreases

44
Q

According to Henry’s law, the solubility of gases ________ with increasing pressure

A

increases

Chemistry 400 (13 decks)

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