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Chem 20 > Chapter 12-14 > Flashcards

Chapter 12-14 Flashcards

(54 cards)

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1
Q

Solutions

A

Homogeneous mixtures of substances composed of solutes and solvents

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2
Q

Solute

A

A substance that is dissolved (salt)

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3
Q

Solvent

A

Medium in which a solute is dissolved (ex: water)

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4
Q

Heterogeneous Mixture

A

Contains undissolved particles large enough to block or scatter light waves (milk)

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5
Q

Homogeneous Mixture

A

A clear substance, that when a chemical analysis of a sample is done you would find that the proportion of each chemical in the sample remains the same
*uniform mixtures of entities

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6
Q

Electrolytes

A

Compounds that their aqueous solutions conduct electricity

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7
Q

Non electrolytes

A 
Compounds that their aqueous solutions do not conduct electricity 
(Determine class of solute based on ohmmeter)
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8
Q

Electrolytes vs nonelectrolytes

A

Electrolytes are mostly highly soluble ionic compounds and bases (ionic hydroxides)
Nonelectrolytes are molecular compounds
Exception: acids conduct electricity

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9
Q

Dissociation

A

Describes the separation of ions that occurs when an ionic compound dissolves in water
*water is necessary, but is not consumed nor is a reactant

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10
Q

Ionization

A

Is the process by which a neutral atom or molecule is converted to an ion

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11
Q

Acids empirical definition

A

Forms solution that:

  • turn blue litmus red
  • are electrolytes
  • neutralize bases
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12
Q

Acids Arrhenius Theory

A

Hydrogen compounds to ionize to produce H+ (aq) ions, H+(aq) ions react with OH- (aq) ions to produce water

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13
Q

Bases Empirical Definition

A

Form solutions that:

  • turn red litmus blue
  • are electrolytes
  • neutralize acids
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14
Q

Bases Arrhenius theory

A

Ionic hydroxides dissociate to produce OH- (aq) ions, OH- (aq) ions react with H+ (aq) ions to produce water

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15
Q

Neutral Substances empirical definitions

A

Form solutions that:

  • do not affect litmus
  • some are electrolytes
  • some are non-electrolytes
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16
Q

Neutral Substances Arrhenius theory

A

No H+ (aq) or OH- (aq) ions are formed, some are ions in solution, some are molecules in solutions

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17
Q

Theoretical Principle of energy

A

Breaking existing bonds uses energy, forming new bonds release energy

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18
Q

Endothermic

A

More energy is absorbed than released

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19
Q

Exothermic

A

More energy is released than absorbed

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20
Q

Strong acids

A

Acids that are extremely good conductors

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21
Q

Weak acids

A

Most other common acids

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22
Q

Concentration

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A

Ratio that compares the quantity of solute to the quantity of the solution

23
Q

Dilute concentration

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A

If it has a relatively small quantity of solute per unit volume of solution

24
Q

Concentrated solution

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A

Relatively large quantity of solute per unit volume of solution

25
Concentration Equation
Concentration (c) = quantity of solute/ quantity of solution
26
Percentage Equation
C= v solute/ v solution x 100%
27
Percentage by weight volume
C= m solute/ v solution x 100%
28
Percentage by mass
C= m solute/ m solution x 100%
29
Parts per million
``` C= m solute/ m solution x10^6 = M solute (mg) / m solution (kg) ```
30
Amount concentration
Chemical amount of solute dissolved in one litre of solution | Amount concentration= chemical amount of solute in moles/ volume of solution (in litres)
31
Mass, volume and concentration calculations
n=Vc | m=nM
32
Concentration of Ions
Conductivity suggests the presence of ions in a solution, amount concentrations of the ions in a solution depend on the relative number of ions making up the compound.
33
Standard solutions
A solution with a concentration that is known with considerable certainty a solution of accurate concentration
34
Dilution
Quick procedure that begins with a stock solution and to add a solvent (water) to decrease concentration to desired level
35
Stock solution
Is an initial, concentrated solution from which samples are taken for a dilution
36
Dilution/ Constant quantity solute Equation
V1C1=VfCf Concentration is inversely related to solutions Volume *as volume increases, concentration decreases
37
Solutions make it easy to
Handle chemicals, complete reactions, control reactions
38
Saturated solution
A solution in which no more solute will dissolve at a specified temperature (maximum solute concentration) Dynamic equilibrium is reached
39
Solubility
Is the concentration of a saturated solution, needs a temperature value
40
Solids solubility in water
Solids have a higher solubility in water at higher temps
41
Gases solubility in water
Gases have a higher solubility in water at lower temps, solubility decreases as temp increases. Have a higher solubility in water at higher pressures
42
Liquids solubility in water
Liquids: polar liquids in water solubility increases the with temp
43
Immiscible in water
Non polar liquids do not dissolve and form a separate layer
44
Miscible
Liquids with small polar molecules and hydrogen bonding dissolve completely in any proportion
45
Elements solubility in water
Have low solubility in water
46
Solubility table
Of ionic compounds assumes that most substances dissolve in water to some extent, vary from very soluble to slightly soluble, allows to predict state of a compound formed in a reaction in aqueous solution *cutoff between very and slightly is 0.1 mol/L
47
In equilibrium
Of solution is in a closed system (no substance can enter or leave), the observable properties become constant
48
Dynamic equilibrium
The balance that exits when two opposing processes occur at the same rate, solubility Equilibrium must contain both dissolved and undissolved solute at the same time. Rate at which particles dissolves equals the rate at which particles crystallize
49
Precipitate
Insoluble product forms a solid | Reaction that forms a solid
50
Factors that affect solubility
Temperature, pressure, nature of solute and solvent
51
Supersaturated
A saturated solution may be heated to dissolve extra solute and then carefully cooled to the original temperature without the extra solute crystallizing
52
Dissolving
When a solute dissolved in a solution, the solid particles move into the solvent to form ions
53
Crystallization
At the same time, some of the dissolved ions crystallize to Become solid again
54
Categories of solutions
What their solvent is If they can conduct electricity Acidity

Chem 20 (8 decks)

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