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Chemistry 30S > Solutions > Flashcards

Solutions Flashcards

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1
Q

Pressure

A

Increases the solubility of gas in a solvent.

Forces particles together

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2
Q

Temperature (solubility)

A

Increases the solubility of solids in a solvent.

Decreases solubility of gases in a solvent.

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3
Q

Agitate (stir) the mixture

A

Adding energy from stirring dissolves it faster

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4
Q

Surface Area (crushing)

A

Dissolves faster with increased surface area

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5
Q

Homogeneous Mixtures

A

Particles are evenly distributed

Ex. salt water

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6
Q

Things that look homogenous but is really heterogenous

A 
Blood
Milk
Mayonnaise
Whip cream
Jelly
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7
Q

Colloids/Gels

A

Larger molecules suspended in liquid.
Are usually opaque/translucent.
Not easily filtered and do not settle out.

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8
Q

Emulsion

A

Heterogeneous mix of two or more liquids.
If you let me sit they will separate
(Ex. Oil and water)

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9
Q

Saturated Solution

A

Max amount dissolved at that temperature.

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10
Q

Unsaturated Solution

A

Solvent is able to dissolve more at that temperature.

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11
Q

Supersaturated

A

Solvent is holding more solute that normally can at that temperature.
Very unstable.

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12
Q

Saturated solution

A

Amount of solute needed to make a saturated solution.

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13
Q

Suspension

A

Heterogeneous mix of solid in liquid.
Use filters to separate components.
(Ex. sand in water)

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14
Q

Heterogeneous mixtures

A

Uneven distribution.
Particles in mixture can be identified.
(Ex. sand and water)

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15
Q

Aqueous Solution

A

Solutions with water as the solvent.

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16
Q

Solute

A

The dissolved substance.

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17
Q

Nature of the solvent and solute

A

Like dissolves like

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18
Q

Types of solutions

A

Saturated
Unsaturated
Supersaturated

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19
Q

Dissociating

A

The process of separating into charged parts when dissolving.
Only ionic and very polar covalent compounds will dissociate.

20
Q

Electrolytes

A

Charged particles in a solution can conduct an electrical current.
If it dissociates it creates electrolytes.

21
Q

Uncharged Particles (non-polar)

A

Are only soluble in uncharged solvents.

22
Q

If a solute is attracted to water will it dissolve.

A

When water is the solvent- hydration

23
Q

Solvent

A

Substance that does the dissolving.

24
Q

3 steps in the dissolving process

A

1) solute particles must break apart.
•requires energy
2) solvent particles spread apart to make room
•requires energy
3) solute and solvent particles come together •release energy

25
Q

Ionic

A

Give/take of electrons between metals and non metals
Creates charged ions
Really big Electronegativity difference

26
Q

Non polar covalent

A

Equal sharing of bonding electrons
No dipoles-no permanent charge
Small Electronegativity difference
Diatomic and coin pounds of c and h are non polar

27
Q

Solubility

A

The amount of solute that can dissolve in a give. Volume of solvent to form a solution.

28
Q

Soluble

A

Dissolves in a solvent (solution)

29
Q

Insoluble

A

Does not dissolve (suspension)

30
Q

Alloys

A

Solutions of two or more metals.

Ex. Steel- iron and carbon

31
Q

Very Polar

A

Dissociates

Ex. HCl=>H+Cl

32
Q

Polar Covalent

A

Unequal sharing of bonding electrons.
Creates positive and negative dipoles to opposite parts of compound.
Bigger Electronegativity difference.

33
Q

Electronegativity

A

The attraction an atom has for the shared pair of electrons in a bond.

34
Q

Immiscible

A

Liquids do not mix (emulsion)

35
Q

Solution

A

Mixture where all substance are distributed as individual molecules or ions
Solution do not settle
Solutions cannot be filtered

36
Q

Spectator Ions

A

Do not participate, remain moving freely in a solution.

37
Q

Miscible

A

Liquids mix in each other

38
Q

Precipitation (ppt) reaction

A

Formation of an ionic compound that is not soluble in current solvent.

39
Q

Homogeneous mixtures

A

Particles are evenly distributed.
Difficult to separate.
(Ex. Salt in water)

40
Q

Factors that affect solubility

A 
Nature of the solvent and solute
Surface area
Agitate (stir)
Temperature
Pressure (only gases)
41
Q

Some molecules can contain ____ but because of the ____ they are considered to be a ____.

A

Polar bonds
Shape
Non-polar molecules

42
Q

All gas mixtures are ____ and ____.

A

Solutions

Homogeneous

43
Q

The most electronegative element is ____ with ____.

A

Fluorine

4.0

44
Q

The least electronegative element is ____ with ____.

A

Cesium

0.7

45
Q

In a compound, the atom with the ____ Electronegativity pulls the ____ electrons ____.

A

Higher
Shared
Closer

46
Q

In a mixture of the same states (bother liquids), the ____ is the substance present in the ____.

A

Solvent

Larger amount

47
Q

A solution is made up with ____ and ____.

A

Solute

Solvent

Chemistry 30S (2 decks)

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