Solution and Colligative Properties

Question 1

Matter exists in two types

Answer 1

pure substances
mixtures

Question 2

have fixed composition such as elements and compounds

Answer 2

pure substances

Question 3

have variable composition

Answer 3

mixtures

Question 4

Two types of mixture:

Answer 4

homogenous
heterogenous

Question 5

have a single phase and are same in appearance throughout

Answer 5

homogenous mixture

Question 6

mixture that have two or more distinct phases

Answer 6

heterogeneous mixture

Question 7

homogenous mixtures that consists of solute and solvent

Answer 7

solution

Question 8

substance that is dissolved

Answer 8

solute

Question 9

dissolving agent

Answer 9

solvent

Question 10

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

Answer 10

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

Question 11

contains less amount of solvent

Answer 11

concentrated soln

Question 12

contains more solvent

Answer 12

dilute solution

Question 13

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

Answer 13

solubility

Question 14

Temperature dependent

Answer 14

solubility

Question 15

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

Answer 15

unsaturated

Question 16

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

Answer 16

saturated

Question 17

contains the maximum amount of solute at a higher temperature

Answer 17

supersaturated

Question 18

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

Answer 18

particle size
temperature
nature of solute and solvent
pressure

Question 19

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

Answer 19

faster

Question 20

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

Answer 20

increases, less

Question 21

solubility follows the rule “like ____like”.

Answer 21

dissolves

Question 22

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

Answer 22

polar
nonpolar

Question 23

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

Answer 23

increases

Question 24

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

Answer 24

increases
less

Question 25

as the pressure _____ , solubility _____

Answer 25

increases

Question 26

the _____ the surface area, the faster it dissolves

Answer 26

larger

Question 27

quantitative way of such description

Answer 27

concentration units

Question 28

common concentration units

Answer 28

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

Question 29

formula by % by mass

Answer 29

mass of solute / mass of solution * 100

Question 30

formula of % by volume

Answer 30

volume of solute / volume of solution * 100

Question 31

formula of % by mass volume

Answer 31

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

Question 32

formula of density

Answer 32

mass/volume

Question 33

formula of mass

Answer 33

(density)(volume)

Question 34

formula of volume

Answer 34

mass/density

Question 35

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

Answer 35

=41.2%

Question 36

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

Answer 36

41.2%

Question 37

formula for molarity

Answer 37

moles solute / volume of soln (L)

Question 38

formula for molality

Answer 38

moles solute / mass (kg) solvent

Question 39

mole fraction formula

Answer 39

number of moles solute / total number of moles soln

Question 40

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.

Answer 40

molarity =17.3𝑀 molality = 25.1𝑚 mole fraction = 0.312

Question 41

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.

Answer 41

molarity = 16.0 𝑀 𝐻𝑁𝑂3 molality = 39.0 𝑚 𝐻𝑁𝑂3 mole fraction = 0.412

Question 42

ppm units

Answer 42

mg/L or mg/kg

Question 43

ppb units

Answer 43

μg/L or μg/kg

Question 44

ppt units

Answer 44

ng/L or ng/kg

Question 45

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

Answer 45

ppm = 1.4 ppm Zn ppb = 1385 ppb Zn

Question 46

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

Answer 46

dilution

Question 47

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

Answer 47

𝐶1𝑉1= 𝐶2𝑉2

Question 48

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

Answer 48

30.0 𝑚𝐿

Question 49

stepwise dilution process using a certain dilution factor

Answer 49

serial dilution

Question 50

HCl comes in 10mL bottles of 1M concentration. You serially dilute it 3 times, diluting the solution by ½ each time. What is the concentration of the HCl at the end.

Answer 50

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

Question 51

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

Answer 51

colligative properties

Question 52

Four specific colligative properties

Answer 52

freezing point depression boiling point elevation vapor pressure lowering osmotic pressure

Question 53

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

Answer 53

coolant

Question 54

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

Answer 54

lower

Question 55

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

Answer 55

higher

Question 56

Formula for freezing point depression

Answer 56

𝛥𝑇𝑓= 𝑘𝑓𝑚

Question 57

𝛥𝑇𝑓= 𝑘𝑓𝑚 Kf = ? m = ?

Answer 57

kf = freezing point depression constant m = molality

Question 58

formula for boiling point depression

Answer 58

𝛥𝑇𝑏= 𝑘𝑏𝑚

Question 59

𝛥𝑇𝑏= 𝑘𝑏𝑚 ΔTb = ? Kb = ? m = ?

Answer 59

ΔTb = boiling point elevation Kb = boiling point elevation constant m = molality

Question 60

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 = 1.86𝑜𝐶/𝑚 Kb = 0.51𝑜𝐶/m freezing point of water = 0.0^oC boiling point of water = 101.2^oC

Answer 60

𝛥𝑇𝑓= -4.46^oC ΔTb = 100.0oC

Question 61

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

Answer 61

diffusion

Question 62

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

Answer 62

osmosis

Question 63

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

Answer 63

dialysis

Question 64

can be used to determine the molar mass of certain compounds

Answer 64

osmotic pressure

Question 65

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

Answer 65

2.59𝑥104 𝑔/𝑚𝑜𝑙𝑒

Question 66

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

Answer 66

vapor pressure lowering

Question 67

formula for vapor pressure lowering

Answer 67

𝛥𝑃= 𝑋2𝑃1𝑜

Question 68

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

Answer 68

grade yourself accordingly

Question 69

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

Answer 69

grade yourself accordingly

Question 70

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

Answer 70

grade yourself accordingly

Question 71

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

Answer 71

1.03𝑚𝑚𝐻𝑔