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Chem 20 > Unit 3: Solutions and Mixtures > Flashcards

Unit 3: Solutions and Mixtures Flashcards

1
Q

What is a solution

A

Homogeneous mixture of a substance, composed of at least 1 solute and 1 solvent

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2
Q

What is a Solute?

A

the substance that is dissolved.

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3
Q

What is a solvent?

A

Medium in which the solute is dissolved; more of it; often water (universal solvent)

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4
Q

what is a homogeneous mixture?

A

Theoretically - uniform at the atomic and molecular level.

Where most liquid and gas state solutions are transparent

However, there are solutions that are colored as well (mostly with solids/metals)

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5
Q

what is a heterogeneous mixtures?

A

contain undissolved particles, are opaque or translucent.

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6
Q

add chart on phone

A
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7
Q

What does all aqueous solutions have? (three things)

A

They have water as a solvent

they may be coloured or colourless (Most useless piece of information but oh well)

are electrolytes (can conduct electricity

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8
Q

Recall: molecular and ionic compounds, and acids… are they electrolytes?

A 
ionic = yes
molecular = mostly no
acids = yes
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9
Q

How to test the conductivity of electrolytes or solutions?

A

Ohmmeter

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10
Q

what are electrolytes?

A

Conduct electricity in aqueous form.

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11
Q

What is litmus paper used for?

A

To classify solutes as acids, bases or neutral substances.

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12
Q

What does the subscript (alc) mean?

A

Dissolved in alcohol (any alcohol)

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13
Q

what did Svante Arrhenius do 1887?

A

explain electrolytes

proposed that when a substance dissolves, particles separate and disperse.

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14
Q

What makes ionic compounds electrolytes?

A

Because they are electrolytes, they have electrically charged particles that split away from each other when it dissociates.

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15
Q

what do non-electrolytes do in a solution?

A

They stay in the same compound and won’t go into Ions.

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16
Q

Define dissociation?

A

The separation of ions occurs when an IONIC compound dissolves in water.

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16
Q

Define dissociation?

A

The separation of ions occurs when an IONIC compound dissolves in water.

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17
Q

What is dissolving?

A

the process where a polar solute (any state or type) dissolved in a solvent to form a solution

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18
Q

What is low solubility?

A

Non-polar molecules or low soluble ionic compounds that have a low solubility.

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19
Q

What is ionization?

A

the process by which an acid produces h+(aq) and an anion

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20
Q

What does acids do in Arrhenius’ Theory

A

Ionize to produce H ions that react with OH ions to produce water

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21
Q

What do biases do in Arrhenius’ Hypothesis

A

Ionic hydroxides (OH) dissociate and then reacts with H ions to produce water

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22
Q

What is the definition of endothermic?

A

Absorbing energy from surroundings

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23
Q

What is the definition of exothermic?

A

Release energy from to the surroundings

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24
Q

Does breaking bonds or forming bonds release or require energy

A

Breaking bonds = uses energy.

Forming bonds = releases energy.

25
Q

What is concentration?

A

The ratio of solute to solvent

26
Q

What is the definition of a dilute solution?

A

Has a relatively small quantity of solute per unit volume of solvent

27
Q

What is the definition of a concentrated solution?

A

Has a relatively large quantity of solute per unit volume of solvent.

28
Q

How to do volume by volume concentration

A

V solute.
*100% = V%
V solution

Make sure you say v/v at the end

Make sure the units are the same

29
Q

How to do % concentration mass by volume?

A

M solute
*100 = concentration
V solution

Make sure you say m/v at the end

Make sure that the units are the same

30
Q

How to do concentration mass by mass

A

M solute
*100 = concentration
M solvent

Make sure units are the same

31
Q

What is molarity of a solution?

A

M/L

Always in moles per litre.

32
Q

What does M mean?

A

Moles per litre.

33
Q

How to do parts per million concentration

A

(Miligram)/kg = ppm

Miligram/L = ppm

34
Q

What is parts per billion and parts per trillion ratio

A

1 : 10 to the nine

1 : 10 to the twelve

35
Q

How can solutions be prepared?

A 
Solid solute 
Dilution method (oj from frozen concentrate)
36
Q

What is a standard solution?

A

Solution of accurate concentration

used in and prepared for labs and industry

37
Q

What are the two pieces of equipment necessary to prepare a solution from a solid?

A

Electronic balances, volumetric flasks

38
Q

How to prepare a dilution solution

A

Start with the stock solution (concentrated samples taken for dilution)

Then decide if you want it to be dilute (less than 0.1 mol/L) or concentrated (more than 1 mol/L)

Add solvent

39
Q

What is the solution formula?

A

CV = C2V2

Where C is the concentration
And V is volume (V can be any unit as long as it’s the same)

40
Q

Why should you dilute a solution?

A

To slow down a reaction

41
Q

What is the equipment necessary to dilute a solution?

A

Graduated pipette, and volumetric pipette, volumetric flask

42
Q

What type of relationship does concentration and volume

A

A INVERSE RELATIONSHIP!

43
Q

What is Ion concentration?

What is a mole ratio?

A

of ions in a solution as a ratio

One mol of [CaCl2]

Equals one mol of [Ca 2+]

And two mol of [Cl -]

to create a 1:1:2 ratio (compound, cation, anion)

44
Q

How to find ion concentration

A

Concentration • number of ion mol’s / number of mol’s in solution

Ex
0.500mol/L of CaCl2 • 2/1 = 1mol/L of Cl2

45
Q

What is an unsaturated solution?

A

More solute can be added.

Test by adding more solute

46
Q

What is a saturated solution?

A

Max amount of solute in a given temp.

Test by adding more solute and it will not dissolve

47
Q

What is a supersaturated solution?

A

More than the max amount of solute is dissolved at given conditions (by heating and cooling it)

The test is adding more solute and the solution crystalizes

48
Q

What is dynamic equilibrium?

A

When two opposite processes happen at the same rate.

Ex

The rate of dissolving is equal to the crystallization process.

49
Q

What is BCE?

A

Balanced chemical equation

50
Q

What is TIE?

A

Total ionic equation

51
Q

What is NIE?

A

Net ionic equation

52
Q

What is a ppt?

A

Precipitate

53
Q

What is a spectator ion?

A

an ion that exists as a reactant and a product in a chemical equation.

Removed for the NIE

54
Q

When are solids more soluble in water?

A

When the water temp. Is higher

55
Q

When are gasses more soluble in water

A

Lower temp, higher pressure.

56
Q

What is the relationship between the solubility of gas as temp increases

A

AN INVERSE RELATIONSHIP

57
Q

What increases the solubility of polar substances?

A

Higher temp.

58
Q

What happens if you try to dissolve any amount of polar molecules with h bonding?

A

ALL OF IT gets dissolved. (Can NEVER become a saturated solution)

59
Q

Do elements dissolve?

What are the edge cases?

What reacts with water?

A

No

Halogens and oxygen gas

(Halogens and alkali metals)

Chem 20 (6 decks)

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