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Chem 20 > Chapter 12-14 > Flashcards

Chapter 12-14 Flashcards

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

A

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

23
Q

Dilute concentration

A

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

24
Q

Concentrated solution

A

Relatively large quantity of solute per unit volume of solution

25
Q

Concentration Equation

A

Concentration (c) = quantity of solute/ quantity of solution

26
Q

Percentage Equation

A

C= v solute/ v solution x 100%

27
Q

Percentage by weight volume

A

C= m solute/ v solution x 100%

28
Q

Percentage by mass

A

C= m solute/ m solution x 100%

29
Q

Parts per million

A 
C= m solute/ m solution x10^6 
= 
M solute (mg) / m solution (kg)
30
Q

Amount concentration

A

Chemical amount of solute dissolved in one litre of solution

Amount concentration= chemical amount of solute in moles/ volume of solution (in litres)

31
Q

Mass, volume and concentration calculations

A

n=Vc

m=nM

32
Q

Concentration of Ions

A

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
Q

Standard solutions

A

A solution with a concentration that is known with considerable certainty a solution of accurate concentration

34
Q

Dilution

A

Quick procedure that begins with a stock solution and to add a solvent (water) to decrease concentration to desired level

35
Q

Stock solution

A

Is an initial, concentrated solution from which samples are taken for a dilution

36
Q

Dilution/ Constant quantity solute Equation

A

V1C1=VfCf
Concentration is inversely related to solutions Volume
*as volume increases, concentration decreases

37
Q

Solutions make it easy to

A

Handle chemicals, complete reactions, control reactions

38
Q

Saturated solution

A

A solution in which no more solute will dissolve at a specified temperature (maximum solute concentration)
Dynamic equilibrium is reached

39
Q

Solubility

A

Is the concentration of a saturated solution, needs a temperature value

40
Q

Solids solubility in water

A

Solids have a higher solubility in water at higher temps

41
Q

Gases solubility in water

A

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
Q

Liquids solubility in water

A

Liquids: polar liquids in water solubility increases the with temp

43
Q

Immiscible in water

A

Non polar liquids do not dissolve and form a separate layer

44
Q

Miscible

A

Liquids with small polar molecules and hydrogen bonding dissolve completely in any proportion

45
Q

Elements solubility in water

A

Have low solubility in water

46
Q

Solubility table

A

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
Q

In equilibrium

A

Of solution is in a closed system (no substance can enter or leave), the observable properties become constant

48
Q

Dynamic equilibrium

A

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
Q

Precipitate

A

Insoluble product forms a solid

Reaction that forms a solid

50
Q

Factors that affect solubility

A

Temperature, pressure, nature of solute and solvent

51
Q

Supersaturated

A

A saturated solution may be heated to dissolve extra solute and then carefully cooled to the original temperature without the extra solute crystallizing

52
Q

Dissolving

A

When a solute dissolved in a solution, the solid particles move into the solvent to form ions

53
Q

Crystallization

A

At the same time, some of the dissolved ions crystallize to Become solid again

54
Q

Categories of solutions

A

What their solvent is
If they can conduct electricity
Acidity

Chem 20 (8 decks)

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