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Inorganic and Organic Chemistry > Solution and Colligative Properties > Flashcards

Solution and Colligative Properties Flashcards

1
Q

Matter exists in two types

A

pure substances
mixtures

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2
Q

have fixed composition such as elements and compounds

A

pure substances

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3
Q

have variable composition

A

mixtures

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4
Q

Two types of mixture:

A

homogenous
heterogenous

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5
Q

have a single phase and are same in appearance throughout

A

homogenous mixture

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6
Q

mixture that have two or more distinct phases

A

heterogeneous mixture

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7
Q

homogenous mixtures that consists of solute and solvent

A

solution

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8
Q

substance that is dissolved

A

solute

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9
Q

dissolving agent

A

solvent

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10
Q

Solution may be classified according to the state of matter (solid, liquid, or gas) of the solvent and the solute such as:

A

liquid-liquid soln
liquid-solid soln
liquid-gas soln
solid-solid soln
solid-gas soln
gas-gas soln

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11
Q

contains less amount of solvent

A

concentrated soln

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12
Q

contains more solvent

A

dilute solution

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13
Q

maximum amount of solute dissolved by a given amount of solvent at a definite temperature

A

solubility

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14
Q

Temperature dependent

A

solubility

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15
Q

contains less solute and completely dissolves in a given amount of solvent, at a particular temperature

A

unsaturated

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16
Q

the solvent contains the maximum amount of solute at a particular temperature

A

saturated

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17
Q

contains the maximum amount of solute at a higher temperature

A

supersaturated

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18
Q

The solubility of a particular solute in a given solvent is affected by several factors which includes the following

A

particle size
temperature
nature of solute and solvent
pressure

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19
Q

smaller particle size has larger surface area, thus, there is more points of interactions between the solute and solvent molecules. T
Therefore, smaller particle size favors a _____ rate of dissolution

A

faster

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20
Q

in general, a higher temperature (increases/decreases) the solubility of solid solute in liquid. The opposite is true for gases which becomes (more/less) soluble in liquid as temperature increases

A

increases, less

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21
Q

solubility follows the rule β€œlike ____like”.

A

dissolves

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22
Q

Polar solutes dissolve in polar/nonpolar solvent while nonpolar solute dissolves in nonpolar/polar solvent

A

polar
nonpolar

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23
Q

this applies only to gaseous solute in liquid. An increase in pressure ____the rate of the solubility of gas

A

increases

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24
Q

as the temperature increases, solubility _____ (in most cases) except in gases (more heat, (more/less) gas dissolves)

A

increases
less

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25
Q

as the pressure _____ , solubility _____

A

increases

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26
Q

the _____ the surface area, the faster it dissolves

A

larger

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27
Q

quantitative way of such description

A

concentration units

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28
Q

common concentration units

A

% by mass
% by volume
% by mass-volume
molarity
molality
mole fraction
parts per unit (ppm, ppb, ppt)

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29
Q

formula by % by mass

A

mass of solute / mass of solution * 100

30
Q

formula of % by volume

A

volume of solute / volume of solution * 100

31
Q

formula of % by mass volume

A

mass of solute (g) / volume of solution (mL) *100

32
Q

formula of density

A

mass/volume

33
Q

formula of mass

A

(density)(volume)

34
Q

formula of volume

A

mass/density

35
Q

Acetone, C3H6O, is the main ingredient in nail polish remover. A solution is made up by adding 35.0 mL of acetone (d= 0.790 g/mL) to 50.0 mL of ethyl alcohol, C2H6O (d=0.789 g/mL). Assuming volumes are additive, calculate the following:

the mass percent of acetone in the solution

36
Q

Acetone, C3H6O, is the main ingredient in nail polish remover. A solution is made up by adding 35.0 mL of acetone (d= 0.790 g/mL) to 50.0 mL of ethyl alcohol, C2H6O (d=0.789 g/mL). Assuming volumes are additive, calculate the following:

b. the volume percent of ethyl alcohol in the solution

37
Q

formula for molarity

A

moles solute / volume of soln (L)

38
Q

formula for molality

A

moles solute / mass (kg) solvent

39
Q

mole fraction formula

A

number of moles solute / total number of moles soln

40
Q

Calculate the molarity, molality, and mole fraction of NH3 for a solution of 30.0g of NH3 in 70.0g of water. The density of the solution is 0.982 g/mL.

A

molarity =17.3𝑀
molality = 25.1π‘š
mole fraction = 0.312

41
Q

Reagent grade nitric acid is 71.0% nitric acid by mass and has a density of 1.418 g/mL. calculate the molarity, molality, and mole fraction of nitric acid in the solution.

A

molarity = 16.0 𝑀 𝐻𝑁𝑂3
molality = 39.0 π‘š 𝐻𝑁𝑂3
mole fraction = 0.412

42
Q

ppm units

A

mg/L or mg/kg

43
Q

ppb units

A

ΞΌg/L or ΞΌg/kg

44
Q

ppt units

A

ng/L or ng/kg

45
Q

A 2.6g sample of plant tissue was analyzed and found to contain 3.6ΞΌg zinc, what is the concentration of zinc in the plant sample in ppm and ppb

A

ppm = 1.4 ppm Zn
ppb = 1385 ppb Zn

46
Q

process of preparing a less concentrated solution from a more concentrated one

47
Q

to carry out proper dilution, it is important to calculate the needed amount of concentrate for dilution into specific concentration unit,

give the formula that describes the unit of a concentrated solution and its volume to a less concentrated solution and its volume

A

𝐢1𝑉1= 𝐢2𝑉2

48
Q

Describe how you would prepare 500.0 mL 0.150 M NaOH solution from stock solution of 2.50 M NaOH.

A

30.0 π‘šπΏ

49
Q

stepwise dilution process using a certain dilution factor

A

serial dilution

50
Q

HCl comes in 10mL bottles of 1M concentration. You serially dilute it 3 times, diluting the solution by Β½ each time. What is the concentration of the HCl at the end.

A

first dilution = 0.5 M
second dilution = 0.25 M
third dilution = 0.125 M

51
Q

are those dependent only on the amount of solute and not only on its nature

A

colligative properties

52
Q

Four specific colligative properties

A

freezing point depression
boiling point elevation
vapor pressure lowering
osmotic pressure

53
Q

whenever this is placed in car radiators, boiling point elevation is applied

54
Q

When a solute is dissolved in the solvent the freezing point of the resulting solution is ___ than the freezing point of the pure solvent.

55
Q

the boiling point of the solution is ___ compared to that of the pure solvent.

56
Q

Formula for freezing point depression

A

π›₯𝑇𝑓= π‘˜π‘“π‘š

57
Q

π›₯𝑇𝑓= π‘˜π‘“π‘š

Kf = ?
m = ?

A

kf = freezing point depression constant
m = molality

58
Q

formula for boiling point depression

A

π›₯𝑇𝑏= π‘˜π‘π‘š

59
Q

π›₯𝑇𝑏= π‘˜π‘π‘š

Ξ”Tb = ?
Kb = ?
m = ?

A

Ξ”Tb = boiling point elevation
Kb = boiling point elevation constant
m = molality

60
Q

Calculate the boiling point and freezing point of a solution containing 478 g of ethylene glycol in 3202 g of water. Molar mass of ethylene glycol is 62.07 g/mole. Use data from table 3.1.

Kf = 1.86π‘œπΆ/π‘š
Kb = 0.51π‘œπΆ/m
freezing point of water = 0.0^oC
boiling point of water = 101.2^oC

A

π›₯𝑇𝑓= -4.46^oC
Ξ”Tb = 100.0oC

61
Q

movement of solute molecules from an area of higher concentration to an area of lower concentration

62
Q

is the diffusion of solvent across a membrane, the movement of the solvent molecules from a region of lower solute concentration to a region of higher solute concentration

63
Q

process of separating molecules in solution by the difference in their rates of diffusion through a semipermeable membrane

64
Q

can be used to determine the molar mass of certain compounds

A

osmotic pressure

65
Q

A 202-mL benzene solution containing 2.47g of an organic polymer has an osmotic pressure of 8.63 mmHg at 21oC. calculate the molar mass of the polymer.

1 atm = 760mmHg
C + 273 = Kelvin

A

2.59π‘₯104 𝑔/π‘šπ‘œπ‘™π‘’

66
Q

when a solute is added the vapor pressure above the solution becomes lower compared to that of a pure solvent

A

vapor pressure lowering

67
Q

formula for vapor pressure lowering

A

π›₯𝑃= 𝑋2𝑃1π‘œ

68
Q

Complete the following table for aqueous solutions of potassium hydroxide. Show complete solution. Molar mass KOH = 56.11 g/mole; H2O = 18.02g/mole.

refer to the ppt slide

A

grade yourself accordingly

69
Q

Complete the following table for aqueous solution of potassium hydroxide. Show complete solution. Molar mass KOH = 56.11 g/mole ; H2O = 18.02 g/mole

refer to ppt slide

A

grade yourself accordingly

70
Q

Complete the following table for aqueous solutions of potassium hydroxide. Show complete solution. Molar mass of KOH = 56.11 g/mole; H2O = 18.02 g/mole

refer to ppt slide

A

grade yourself accordingly

71
Q

A solution is prepared by dissolving 396g of sucrose (C12H22O11) in 624g of water. What is the vapor pressure of this solution at 30oC (the vapor pressure of water is 31.8 mmHg at 30oC)

  • Mass of sucrose = 396g
  • Mass of water = 624g
  • Vapor pressure of water at 30oC = 31.8mmHg
A

1.03π‘šπ‘šπ»π‘”

Inorganic and Organic Chemistry (19 decks)

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