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Chemistry > Unit Seven > Flashcards

Unit Seven Flashcards

1
Q

Heterogeneous mixture

A

Do not have uniform composition (can see different parts)

Ex sand and water

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2
Q

Homogeneous mixture

A

Have uniform composition throughout (can’t see different parts)
Another name for a homogeneous mixture is a solution
Ex sugar and water

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3
Q

Aqueous

A

When substances are in a solution with water

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4
Q

Universal solvent

A

Water is the most common solvent used in the world, referred to as universal solvent

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5
Q

Distillation

A

Separates liquids based on boiling points

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6
Q

Centrifuge

A

Rapid spinning of a mixture to separate particles by density

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7
Q

Decant

A

Pouring a liquid off a solid

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8
Q

Filtration

A

Using a porous barrier to separate components of a mixture

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9
Q

Chromatography

A

Ability to run across a surface

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10
Q

Suspension

A

A dispersion of large particles that are temporarily suspended and settle out naturally over time
Ex orange juice with pulp

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11
Q

Colloid

A

Consists of two phases of matter and are only heterogeneous on a microscopic level (can’t see different parts with naked eye)
Cloudy
Ex milk

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12
Q

Major differences between suspension and colloids

A

Suspension do not have uniform composition, colloids have uniform composition
Colloids have much smaller particles than suspensions do
Because colloids don’t settle out, they are considered stable, suspensions are not stable because over time the parts of the mixture will separate

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13
Q

Solute

A

The substance that is being dissolved

Ex salt in salt and water

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14
Q

Solvent

A

The substance doing the dissolving

Ex water in salt and water

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15
Q

How to tell apart colloids and solutions

A

Colloids are cloudy

Solutions are clear

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16
Q

Solubility

A

The amount of solute that dissolves in a given amount of solvent

17
Q

Factors affecting solubility (dissolving a solid solute in a liquid solvent)

A

Temperature: increasing the temperature will increase solubility
Agitation: stirring the solution helps increase the solubility
Surface area: the smaller the particles the more quickly they will dissolve

18
Q

Saturated solution

A

Contains the maximum amount of solute for a given amount of solvent at a constant temperature

19
Q

Unsaturated solution

A

Contains less solute than a given amount of solvent can dissolve

20
Q

Supersaturated solution

A

Contains more than the maximum amount of solute that a given amount of solvent can dissolve

21
Q

How can you make a supersaturated solution?

A

Create a saturated solution
Heat up the solution
Add more solute
Cool to room temperature

22
Q

Above line
On line
Below line

A

Supersaturated
Saturated
Undersaturated

23
Q

Mixture

A

Two or more pure substances physically combined, components retain properties

24
Q

Soluble/insoluble

A

Used to describe when a solid/gas solute does/does not dissolve

25
Q

Miscible

A

Two liquids that can dissolve in one another
Ex water and ethanol
For liquids only

26
Q

Immiscible

A

Two liquids that cannot dissolve one another
Ex oil and water
Only for liquids

27
Q

Factors affecting solubility of gases

A

Agitation up, solubility down
Temperature up, solubility down
Pressure up, solubility up

28
Q

Solubility rule

A

Like dissolves like

Polar substances dissolve other polar substances, nonpolar substances dissolve other nonpolar substances

29
Q

Solvation

A

The surrounding of solute particles by solvent particles (dissolving)
Ionic compounds dissociate or break apart in water. Water molecules are attracted to ions on the surface of the crystal. Gradually, the water molecules surround each individual ion. This reduces the attraction of the ions for each other, and they are no longer held in the crystalline structure. The ions gradually break apart and move into solution.

30
Q

Electrolytes

A

Solutions that have the ability to conduct electricity

31
Q

PRACTICE WITH SOLUBILITY CURVES GRAPH ON P3 OF CLASSWORK

32
Q

Concentration

A

A measure of the amount of solute that is dissolved in a given amount of solvent

33
Q

Dissociate

A

When ionic compounds break apart in water

34
Q

Diluted solution

A

Contains a low ratio of solute to solution (small concentration of solute)

35
Q

Concentrated solution

A

Contains a high ratio of solute to solution (high concentration of solute)

36
Q

Molarity (M)

A

The number of moles of solute dissolved per liter of solution
Say a solution is molar (ex 0.5 molar)
Most important unit of concentration in chemistry

37
Q

Molarity equation

A

M = moles/liters = n/L = mol/L

38
Q

In diluting solutions, the concentration is

A

Lowered

However, the total number of moles of solute remains unchanged

39
Q

Dilution/concentration equation

A

M1V1 = M2V2

Chemistry (12 decks)

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