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pre ap chemistry 1 > solutions > Flashcards

solutions Flashcards

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1
Q

mixture

A

two or more substances physically combined

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2
Q

homogenous

A

a mixture that is uniform throughout (solution)

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3
Q

heterogenenous

A

a mixture that is not uniform throughout

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4
Q

soluble

A

a substance that is dissolved (aqueous)

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5
Q

insoluble

A

a substance that does not dissolve (a precipitate)

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6
Q

solution

A

a homogenous mixture that contains a solute that is fully dissolved in a solvent

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7
Q

solution examples

A

steel, sugar water, air

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8
Q

solute

A

substance that dissolves in .a solvent

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9
Q

solvent

A

substance that dissolves a solute

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10
Q

what does the solvent do in a solution

A

pulls the solute apart and distributes the particles

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11
Q

saturated

A

solution that can not dissolve any more solute at a given temperature and pressure

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12
Q

unsaturated

A

a solution that can dissolve more solute at a given temperature and pressure

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13
Q

supersaturated

A

a solution in which excess solute precipitates out of the solution at a given temperature and pressure q

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14
Q

what is solubility

A

maximum amount of a solute that will dissolve in a given amount of solvent at a specific temperature and pressure

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15
Q

precipitate

A

forms if the substance is insoluble

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16
Q

substance is aqueous

A

if the substance is soluble

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17
Q

non polar covalent bond

A

bond in which electrons are equally shared

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18
Q

polar covalent bond

A

electrons not equally shared
-one element is more electronegative, so electrons more attracted to more electronegative element, creating a partial charge

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19
Q

nonpolar dissolves in

A

nonpolar

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20
Q

polar dissolves in

A

polar

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21
Q

miscible

A

two liquids are soluble in each other

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22
Q

immiscible

A

two liquids are not soluble in each other

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23
Q

what factors affect the rate of solubility

A

surface area
temperature
pressure of gas

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24
Q

how does temp affect solubility

A
  • increased temp of a solid to increase solubility

- decrease temp of a liquid or gas to increase solubility

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25
Q

how does surface area affect solubility

A

agitation (stirring) allows smaller particles to contact the solute

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26
Q

how does pressure of a gas increase solubility

A

increasing the pressure of a gas increases the solubility

27
Q

what does a solubility graph show

A

shows how temperature affects solubility

28
Q

indentify the species of the graph

A

unsaturated: below the curve
saturated: on the curve
supersaturated: above the curve

29
Q

what is a stock solution

A
  • called standard solution

- solution whose concentration is known

30
Q

concentrated

A

if a solute contains a large amount of product

31
Q

dilute

A

if it contains a small amount of solute

32
Q

concentration

A

a measure of how much solute is dissolved in a solvent

33
Q

molarity

A

measure of concentration of a solute

unit M or moles/litres

34
Q

molarity formula

A

moles of a solute /litres of solution

35
Q

dilution

A

used to dilute a stock solution

remember significant figures

36
Q

dilution formula

A

m1 x v1 = m2 x v2

37
Q

how to prepare a standard solution

A
  1. mass the solute
  2. add the solute and deionized water
  3. swirl solution and dissolve solute
  4. add deionized water to the mark
38
Q

water

A
  • the most common solvent

- H and O held together by polar covalent bonds

39
Q

charges of water

A
  • partial positive charge around both hydrogens

- partial negative charge around the oxygen

40
Q

shape of water

A

bent shape because the two unshared electrons pairs require more space

41
Q

what are the properties of water (non -high ones)

A
  • unequal distribution of electrons
  • soluble because of polarity
  • dissolve nonpolar molecules like alcohols and sugars
42
Q

properties of water (high ones)

A
  • high heat of vaporization
  • high specific heat
  • high cohesive forces
  • high adhesive forces
43
Q

heat of vaporization

A

heat required to change 1 g of H2O to gas

44
Q

specific heat

A

heat required to change 1 g of H2O to 1 degree

45
Q

cohesive force

A

attraction between like molecules

46
Q

adhesive forces

A

attraction between unlike molecules

47
Q

solid water

A

arranged in orderly, open framework result in a less dense substance

48
Q

liquid water

A

move and allow opposing forces to come between the molecules, results in a denser substance

49
Q

intramolecular forces

A

forces that hold atoms together within a molecule

stronger than intermolecular forces

50
Q

types of intramolecular forces

A

ionic bond

covalent bond

51
Q

intermolecular forces

A

forces that hold two or more molecules together

52
Q

types of intermolecular forces

A

dipole-dipole
hydrogen bond
london dispersion force

53
Q

dipole-dipole

A

an attraction between oppositely charger regions of polar molecules

54
Q

hydrogen bond

A

a type of dipole-dipole force in which a H in one molecule bonds with a F, O , or N in another molecule (is very strong)

55
Q

landon dispersion force

A

type of van der Waal force that occurs between non polar molecules in which electrons shift positions (very weak)

56
Q

what is an electrolyte

A

an ionic compound whose solution conducts electricity because it dissociates

57
Q

strong electrolyte

A

a strong acid and strong base, completely dissociates

58
Q

weak electrolyte

A

weak acid and weak base, does not completely dissociate

59
Q

non electrolyte

A

a compound whose solution does not conduct electricity because it does not dissociate

60
Q

what dissociate

A

ionic compounds, breaks into the individual atoms

61
Q

does not dissociate

A

does not break into individual atoms, breaks into individual molecules

62
Q

examples of non electrolytes

A

water, sugar, alcohol

63
Q

is water polar

A

yes

pre ap chemistry 1 (12 decks)

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