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AP Chemistry > H Chemistry: Unit 7 > Flashcards

H Chemistry: Unit 7 Flashcards

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1
Q

solution

A

homogeneous mixture made of a solute and a solvent

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2
Q

solute

A

substance being dissolved

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3
Q

solvent

A

substance dissolving the solute

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4
Q

universal solvent

A

water

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5
Q

solutions can be

A

solids, liquids, and gases

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6
Q

solutions made with water are referred to as

A

aqueous

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7
Q

soluble

A

solutes ability to dissolve in a solvent

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8
Q

insoluble

A

inability for a solute to dissolve

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9
Q

miscible

A

the ability of two liquids to mix together

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10
Q

immiscible

A

the inability of two liquids to mix together

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11
Q

solvation

A

process of dissolving; opposite of crystallization

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12
Q

factors that increase solvation

A
  1. agitation
  2. increase the temperature
  3. increase the surface area of the solute
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13
Q

solvation>crystallization

A

unsaturated solution

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14
Q

solvation=crystallization

A

saturated solution

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15
Q

solvation<crystallization

A

precipitation(solid in solution)

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16
Q

supersaturated solution

A

solution that contains more solute than a saturated solution; unstable and crystallizes rapidly

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17
Q

how to make a supersaturated solution

A
  1. add solute slowly and heat a saturated soln
  2. stir slowly
  3. let it cool to room temperature
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18
Q

delta H of solution

A

change in energy when a solution is formed

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19
Q

solubility

A

maximum amount of solute that can be dissolved in 100 grams of solvent at STP

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20
Q

factors that affect solubility

A
  1. temperature
  2. pressure
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21
Q

concentration

A

expression of the ratio of solute to solvent

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22
Q

diluted solution

A

very little solute to solvent

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23
Q

concentrated solution

A

a lot of solute compared to solvent(saturated solution)

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24
Q

molarity

A

M; concentration of miles of solute per liter of solution

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25
Q

stock solution

A

solution that is concentrated from which diluted solutions can be made

26
Q

M1V1=

A

M2V2

27
Q

solubility rules 1

A

salts made with Group 1A elements and ammonium are soluble

28
Q

solubility rules 2

A

acetates, bicarbonates, chlorates, & nitrates are soluble

29
Q

solubility rules 3

A

salts made with Br, Cl, I are soluble except when bound to silver, mercury, or lead

30
Q

solubility rules 4

A

sulfates are soluble except when bound to silver, mercury, lead, calcium, strontium, or barium

31
Q

solubility rules 5

A

carbonates, chromates, hydroxides, oxides, and phosphates are insoluble except for rule #1

32
Q

assumptions of ideal gases(5)

A
  1. gas particles are in constant random motion
  2. gas particles do not attract or repel each other
  3. gas particles are much smaller than the space between them
  4. gas particles do not lose kinetic energy when they collide with themselves or their container
  5. gas particles have the same kinetic energy at a given temperature
33
Q

4 properties if gases

A
  1. volume
  2. pressure
  3. temperature(K)
  4. amount(mol)
34
Q

Charles law

A

a volume of a specific amount of gas is directly proportional to its kelvin temperature at constant pressure

35
Q

charles law formula

A

V1/T1 = V2/T2

36
Q

Boyles Law

A

the pressure of a specific amount of gas is inversely related to volume at constant temperature

37
Q

boyles law formula

A

P1V1 = P2V2

38
Q

how many psi in 1 atm

A

14.7

39
Q

how many bar in 1 atm

A

1.01

40
Q

how many mmHg(torr) in 1 atm

A

760

41
Q

how many kPa in 1 atm

A

101.3

42
Q

Gay-Lussacs law

A

the pressure of a specific amount of gas is directly proportional to its Kelvin temperature at constant volume

43
Q

gay-lussacs law formula

A

P1/T1 = P2/T2

44
Q

combined gas law formula

A

P1V1/T1 = P2V2/T2

45
Q

combined gas law is used when

A

only miles are constant and 5 pieces of information are given and you must solve for the 6th; temp must be in K

46
Q

ideal gas law

A

used to solve for a property of a gas at a given moment

47
Q

ideal gas law formula

A

PV = nRT

48
Q

ideal gas constant

A

0.0821(Lxatm)/(molxK)

49
Q

vapor

A

gaseous substance that is a liquid or solid at room temperature

50
Q

vapor pressure

A

pressure exerted by a vapor; every liquid has vapor pressure; determined by molecular structure and mass

51
Q

boiling point

A

temperature at which the vapor pressure is equal to the atmospheric pressure

52
Q

partial pressure

A

pressure exerted by a single gas in a mixture

53
Q

Dalton’s law of partial pressure

A

the total pressure of a mixture is equal to the sun of the partial pressure of the gases that make up a mixture

54
Q

diffusion

A

movement of a gas from high concentration to low concentration

55
Q

effusion

A

movement of a gas through a small opening of hole

56
Q

KE=

A

1/2 mv^2

57
Q

the smaller the gas particle

A

the higher the velocity

58
Q

grahams law

A

the rate(velocity) of a gas particle is inversely related to the square root of its molar mass

59
Q

grahams law formula

A

Rate a/Rate b = (molar mass a/ molar mass b)^1/2

60
Q

Avagadros law

A

the volume at constant pressure is directly proportional to the number of gas particles at a given temperature

61
Q

avagadros law formula

A

V1/N1 = V2/N2

62
Q

standard volume of gas

A

one mole of gaseous particles at STP occupies 22.4 L of space regardless of identity

AP Chemistry (16 decks)

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