Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Grade 11 Chemistry > Unit 4 Test Notes > Flashcards

Unit 4 Test Notes Flashcards

1
Q

What is a solute?

A

A substance that is dissolved in a solvent (ex. salt)

Solutes can be solids, liquids, or gases that are present in a smaller amount compared to the solvent.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is a solvent?

A

The medium in which a solute is dissolved, often the liquid component of the solution (ex. water)

Solvents can be liquids, gases, or solids, but they are typically liquids.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Define a homogeneous mixture.

A

A uniform mixture of only one phase (looks the same throughout)

Examples include salt water and sugar water.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is a solution?

A

A homogeneous mixture of substances composed of at least one solute and one solvent

It appears uniform throughout and does not separate upon standing.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is a heterogeneous mixture?

A

A mixture where it is obvious that there is more than one substance present

Characteristics include being opaque, cloudy, and containing undissolved particles.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is an electrolyte?

A

A compound that, in an aqueous solution, conducts electricity

Electrolytes are often ionic compounds that dissociate into ions when dissolved.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is a nonelectrolyte solution?

A

A compound that, in an aqueous solution, does NOT conduct electricity

Nonelectrolytes are typically molecular compounds that do not dissociate into ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Fill in the blank: Acids form ______ solutions.

A

acidic

Acids increase the concentration of hydrogen ions (H+) in solution.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Fill in the blank: Bases form ______ solutions.

A

basic

Bases increase the concentration of hydroxide ions (OH-) in solution.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Fill in the blank: Water is known as the ______ solvent.

A

universal

Water’s ability to dissolve many substances is due to its polarity and ability to form hydrogen bonds.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is dissociation in the context of ionic compounds in water?

A

The separation of individual ions from an ionic compound as it dissolves in water

For example, NaCl dissociates into Na+ and Cl- ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What does ‘like dissolves like’ refer to?

A

Polar substances dissolve in polar solvents; non-polar substances dissolve in non-polar solvents

This principle explains solubility behaviors based on molecular polarity.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What are hydrogen bonds?

A

A very strong intermolecular force formed when water is the solvent and solutes have N, O, or F lone pairs or H-N, H-O, or H-F bonds

Hydrogen bonding significantly affects the solubility of substances in water.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is the role of London dispersion forces?

A

Weak intermolecular forces between non-polar substances that are responsible for dissolving non-polar solutes in non-polar solvents

These forces are significant in non-polar solute interactions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

True or False: Water is consumed during the dissociation of NaCl.

A

False

Water facilitates the dissociation process but remains unchanged in quantity.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is the difference between a total ionic equation and a net ionic equation?

A

Total ionic equation includes all dissociated ions, while net ionic equation includes only reacting entities.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is a total ionic equation?

A

A chemical equation in which all highly soluble ionic compounds are written as dissociated ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What criteria must a total ionic equation meet to be balanced?

A
  1. All entities on one side must be accounted for on the other side. 2. The net electrical charge must be the same on both sides.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Define spectator ions.

A

Ions that are not involved in a chemical reaction and do not react themselves.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

True or False: Spectator ions participate in the reaction.

A

False.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What is a formula equation?

A

A chemical equation in which all compounds are represented by their chemical formulas.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What does the solubility table predict?

A

The solubilities of many compounds and whether an ionic compound will dissolve into ions or remain a solid.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Fill in the blank: The greater the number of _________, the more reactions occur.

A

collisions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What happens when a solid dissolves into a solution?

A

It reduces into the smallest possible particles, creating a larger surface area and more collisions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What is a net ionic equation?

A

A chemical equation that includes only the entities that react during the reaction.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

List the types of equations discussed.

A
  • Formula Equation
  • Total Ionic Equation
  • Net Ionic Equation
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What must you refer to when writing total and net ionic equations for reactions?

A

The solubility table.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Sample Problem: Write the total ionic equation and net ionic equation for the reaction of lead(II) nitrate and potassium iodide.

A

Refer to the solubility table for the specific equations.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Sample Problem: Write the net ionic equation for aluminum metal in copper(II) chloride solution.

A

Refer to the solubility table for the specific equation.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What is a saturated solution?

A

A solution that contains the maximum quantity of solute at a given temperature and pressure.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

What defines an unsaturated solution?

A

A solution in which more solute can dissolve at a given temperature and pressure.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

What characterizes a supersaturated solution?

A

A solution that contains more than the maximum quantity of solute that it should at a given temperature and pressure.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

Define solubility.

A

The concentration of a saturated solution of a solute in a solvent at a specific temperature and pressure.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

What are the common units for expressing solubility?

A

Grams per 100 mL of solvent.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

What factors affect solubility?

A
  • Molecule size
  • Temperature
  • Pressure
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

How does temperature affect the solubility of solids?

A

Solids usually have a higher solubility in water at higher temperatures.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

What happens to the solubility of gases as temperature increases?

A

The solubility of gases decreases.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

What is a solubility curve?

A

A graph of the solubility of a given solute against temperature.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

What do points on the solubility curve represent?

A

Saturated solutions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

What do points below the solubility curve represent?

A

Unsaturated solutions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

What do points above the solubility curve indicate?

A

Supersaturated solutions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

What is crystallization?

A

A process that occurs when some of the solvent evaporates out of a solution.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

What characterizes high solubility?

A

A maximum concentration at SATP of greater than or equal to 0.1 mol/L.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

Define low solubility.

A

A maximum concentration at SATP of less than 0.1 mol/L.

45
Q

What does it mean if a substance is insoluble?

A

It has negligible solubility at SATP.

46
Q

Fill in the blank: The concentration of a saturated solution must be accompanied by a _______.

A

temperature.

47
Q

True or False: Polar liquids generally decrease in solubility as temperature increases.

A

False.

48
Q

What happens to gas molecules as temperature increases?

A

They regain some energy and come out of solution.

49
Q

What is the definition of concentration?

A

The quantity of a given solute in a solution.

50
Q

What does a dilute solution refer to?

A

Having a relatively small quantity of solute per unit volume of solution.

51
Q

What does a concentrated solution refer to?

A

Having a relatively large quantity of solute per unit volume of solution.

52
Q

How is concentration calculated?

A

Concentration = Quantity of solute / Quantity of solution.

53
Q

What does ‘C’ represent in molar concentration?

A

Molar concentration (mol/L).

54
Q

What does ‘n’ represent in the formula for molar concentration?

A

The amount of solute in moles (mol).

55
Q

What does ‘V’ represent in the formula for molar concentration?

A

The volume of solution in litres (L).

56
Q

What is molar concentration?

A

The amount of solute, in moles, dissolved in one litre of solution.

57
Q

If n = 0.186 mol and V = 0.250 L, what is the molar concentration C?

A

C = 0.744 mol/L.

58
Q

True or False: Molar concentration can be expressed as M.

A

True.

59
Q

Fill in the blank: To calculate molar concentration when given mass, you must first convert to _______.

A

moles.

60
Q

What is the molar concentration of sodium carbonate if 5.00g is dissolved in 250 mL?

A

Calculation needed based on molar mass.

61
Q

What is the amount concentration of a solution containing 63 g of phosphoric acid in 250 mL?

A

Calculation needed based on molar mass.

62
Q

What pages should be read for further understanding of molar concentrations?

A

Pages 397-401.

63
Q

Where can you find practice questions related to molar concentration?

A

Questions on page 402 #3-7.

64
Q

What type of calculations are used to determine molar concentration?

A

Stoichiometric calculations.

65
Q

What is the formula for calculating concentration?

A

Concentration = Quantity of solute / Quantity of solution

66
Q

What does % v/v stand for?

A

% v/v means percentage volume by volume

67
Q

If vinegar is labeled as 5% acetic acid, how many mL of pure acetic acid are in 100 mL of vinegar solution?

A

5 mL

68
Q

What is the percentage by volume concentration of acetic acid in a solution containing 140 mL of acetic acid in a 500 mL bottle?

A

28% v/v

69
Q

What does W/V stand for in concentration measurements?

A

W/V stands for percentage weight by volume

70
Q

What does a 3% W/V concentration of hydrogen peroxide indicate?

A

3 g of hydrogen peroxide in every 100 mL of solution

71
Q

What is the percentage weight by weight concentration of silver in a sterling silver ring that has 11.1 g of pure silver and a total mass of 12.0 g?

A

92.5% w/w

72
Q

What units are commonly used for very low concentrations in environmental studies?

A

ppm, ppb, ppt

73
Q

What is 1 ppm equivalent to in terms of mass and volume?

A

1 g / 1000 L or 1 mg/L

74
Q

How do you calculate the concentration of oxygen in parts per million if 2.2 mg of oxygen is measured in 250 mL of water?

A

8.8 ppm

75
Q

What is the relationship between mass of solute and volume of solvent in a concentration calculation?

A

Concentration = mass of solute / Volume of solvent

76
Q

Fill in the blank: A box of apple juice has a fructose concentration of 12 g/100 mL, which is expressed as _______.

A

12% W/V

77
Q

What mass of fructose is present in a 175 mL glass of juice if the concentration is 12 g/100 mL?

A

21 g

78
Q

True or False: ppm can be expressed as 8.8 mg/L.

A

True

79
Q

What is the general formula for calculating the mass of solute when the concentration and volume are known?

A

Mass of solute = (Concentration) x (Volume)

80
Q

What is a standard solution?

A

A solution for which a precise concentration is known

Standard solutions are often prepared in a volumetric flask for precision.

81
Q

Define dilution in the context of solutions.

A

The process of reducing the concentration of a solution by adding more solvent

Dilution is commonly used in laboratory settings to achieve desired concentrations.

82
Q

What is a stock solution?

A

A solution that is in stock (available), usually a concentrated solution

Stock solutions are used as starting points for dilutions.

83
Q

What is the final concentration when 250 mL of a 16.0 mol/L nitric acid solution is diluted to 4.5 L?

A

Final concentration calculation needed

This question involves dilution calculations.

84
Q

If a 1.00-L bottle of acetic acid is labelled with a concentration of 17.4 mol/L and is diluted to prepare a 0.400 mol/L solution, what volume of diluted solution is prepared?

A

Volume of diluted solution calculation needed

This question requires understanding of dilution calculations.

85
Q

What was the concentration of the original test solution if a 10.00-mL sample is diluted to a final volume of 250.0 mL with a diluted concentration of 0.274 g/L?

A

Original concentration calculation needed

This problem demonstrates the reverse of a dilution calculation.

86
Q

What are the learning goals of this lesson on solutions and solubility?

A

Solve dilution calculation problems and explain the process of dilution

These goals guide the educational focus of the unit.

87
Q

Fill in the blank: A solution prepared in a _______ flask is known for its precision.

A

volumetric

Volumetric flasks are essential for preparing standard solutions accurately.

88
Q

What is the difference between quantitative analysis and qualitative analysis?

A

Quantitative analysis measures the quantity of a substance present, while qualitative analysis determines non-numerical information about a solution or reaction.

89
Q

What is qualitative analysis?

A

The determination of non-numerical information about a solution or reaction.

90
Q

Give an example of qualitative analysis.

A

Observing that a reaction is creating gas that is bubbling out of solution.

91
Q

What is quantitative analysis?

A

The measurement of the quantity of a substance present (e.g., stoichiometric calculations).

92
Q

How can quantitative analysis help chemical engineers?

A

It can help determine if an industrial chemical process is operating optimally.

93
Q

Why is quantitative analysis important in water quality analysis?

A

It is useful in determining if a contaminant is present in toxic amounts.

94
Q

Who can use quantitative analysis in medical labs?

A

Medical lab technicians can determine if a substance has a healthy or legal concentration in human blood.

95
Q

What is solution stoichiometry?

A

A method of calculating the concentration of substances in a chemical reaction by measuring the volumes of solutions that react completely.

96
Q

What conversion factor is used when studying solutions?

A

Molar concentration is used as a conversion factor, rather than molar mass.

97
Q

In Sample Problem #1, what is the mass of barium chromate that will precipitate?

A

5.94 g.

98
Q

What is the first step in solving Sample Problem #1?

A

Write a balanced chemical equation and state all givens.

99
Q

What is the formula for calculating the number of moles of potassium chromate in Sample Problem #1?

A

n = C × V.

100
Q

What is the mole ratio of K2CrO4 to BaCrO4 in Sample Problem #1?

A

1:1.

101
Q

What is the purpose of finding the limiting reactant?

A

To determine which reactant will run out first and limit the amount of product formed.

102
Q

What must you do to calculate the limiting reactant?

A

Determine the moles of each reactant and use the molar ratio.

103
Q

In Sample Problem #3, what is the first step to determine the mass of solid lead(II) sulfide formed?

A

Determine the amount of moles of each reactant.

104
Q

What is the balanced chemical equation for the reaction in Sample Problem #3?

A

Pb(CH3COO)2 (aq) + Na2S (aq) → PbS (s) + 2 NaCH3COO (aq).

105
Q

Fill in the blank: Solution stoichiometry is used to calculate the _______ of substances in a chemical reaction.

A

[concentration]

106
Q

True or False: Qualitative analysis provides numerical data about a reaction.

A

False.

107
Q

What is the molar mass of barium chromate used in Sample Problem #1?

A

253.33 g/mol.

108
Q

How do you determine the volume of Na2SO4 required in Sample Problem #2?

A

Use c = n/v after finding moles of BaCl2 and the mole ratio.

Grade 11 Chemistry (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions