Unit 9 Flashcards

1
Q

a homogeneous mixture of two or more aqueous compounds

A

solution

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2
Q

substance being dissolved

A

solute

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3
Q

substance doing the dissolving

A

solvent

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4
Q

a solution in which the particles of un-dissolved solute are so large that they settle out to the bottom of the container (ex. milk)

A

suspension

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5
Q

a solution in which the particles are so small that they do not settle out but you can see them floating around in the solution (ex. muddy water)

A

colloid

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6
Q

when you shine a light from a flashlight, search light or some sort of beam of light (sun) through a colloid, you can see the beam because it bounces off of the particles in the colloid. If it is a solution, no beam will be seen. (ex. lights at night in a swimming pool)

A

The Tyndall Effect

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7
Q

What is the most common solvent?

A

Water

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8
Q

the molecule is asymmetrical, and the charges are separated

A

Polar

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9
Q

the molecule is symmetrical and will not dissolve in water (ex. gasoline, waxes, oil, etc.)

A

Nonpolar

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10
Q

If two substances will dissolve in each other (oil and gasoline), they are considered ________.

A

Miscible

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11
Q

If two substances will not dissolve in each other

A

Immiscible

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12
Q

when a solution breaks apart into ions and conducts an electric current, like table salt or sulfuric acid

A

Electrolytes

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13
Q

What are three ways to dissolve a solute?

A
  1. Agitate the mixture by stirring or some other mechanical method
  2. Heat the solvent
  3. Increase the surface area of the solute
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14
Q

very little solute, lots of solvent

A

unsaturated

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15
Q

almost equal amounts of solute and solvent, a little solute can be seen at the bottom of the container after stirring

A

saturated

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16
Q

so much solute that there is a lot at the bottom after a lot of stirring/heating

A

supersaturated

17
Q

the amount of solute that will dissolve in a given amount of solute in a given amount of solvent at a specific temperature. (MOST of the time, heating the solvent increases solubility but there are times when heating actually decreases solubility. )

A

Solubility

18
Q

When you increase the pressure on a gas above a liquid, you increase the solubility of that gas in that liquid. When you increase the temperature, the gas escapes (molecules pull away from each other) ex. carbonated beverages

A

Henry’s Law

19
Q

the rapid escape of a gas from a liquid in which it has been dissolved

A

Effervescence

20
Q

the attraction of the surface of a liquid to the surface of a solid. This occurs in plants.

A

Capillary Action

21
Q

a force that tends to pull adjacent parts of a liquid’s surface together, decreasing the surface area (allows water bugs to walk on water)

A

Surface Tension

22
Q

states that a system of equilibrium, when subjected to a stress, shifts in a direction that will relieve the stress on the system. Stress to a system includes changing the temperature, adding or removing reactant or product, etc. (shaking a coke and opening the bottle)

A

LeChatelier’s Principle

23
Q

the change in phase from a sold directly to a gas without going through the liquid phase (ex. dry ice)

A

Sublimation

24
Q

when like molecules are attracted to each other (ex. mercury/aluminum coins floating on water)

A

Cohesion

25
Q

when molecules that are not alike come in contact with each other

A

Adhesion

26
Q

moles of solute per kilogram of solvent (m)

A

Molality

27
Q

moles of solute per Liter of solution (M)

A

Molarity

28
Q

properties depending only on the amount of the solute, not the identity of the solute

A

Colligative Properties

29
Q

solutes that do not affect the boiling or freezing point of the solution because they leave the solution

A

Volatile solutes

30
Q

Boiling point always goes __ and freezing point always goes ____ when a solute dissolves in a pure solvent.

A

up, down