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1
Q

What quantities of a solution change when it is diluted?

A

The concentration and volume of the solution change.

The amount of solute remains constant.**

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2
Q

What happens during the first step of a solid dissolving in water?

A

Bonds in the solute are broken, which is endothermic

This step requires energy to break ionic bonds in the solid.

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3
Q

What is a solution of known concentration called?

A

A standard solution

Standard solutions are essential for various chemical analyses and reactions.

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4
Q

What is the role of the solute in a solution?

A

The solute is the part of the solution that is present in smaller amounts and is dissolved.

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5
Q

What is the first step in predicting the reactions that occur in solution chemistry?

A

analyze entities present and available to react.

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6
Q

What does quantitative analysis identify?

A

The amount of particular substance(s).

Examples include measuring bacteria or pollutants in drinking water.

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7
Q

What does V1 represent in the dilution formula?

A

V1 = initial volume of solution.

It indicates the volume before dilution.

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8
Q

How do acid-forming compounds dissolve?

A

by a process known as ionization.

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9
Q

State two conditions required for a solution to be in dynamic equilibrium.

A
  • The system is under constant conditions of temperature and pressure
  • The system is closed
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10
Q

Define a non-electrolyte.

A

A non-electrolyte is a substance that when dissolved in water will create a solution that does not conduct electricity.

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11
Q

What is qualitative analysis?

A

A process used to identify the presence of specific substances in solution.

Qualitative analysis is distinct from quantitative analysis, which measures the amount of a substance.

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12
Q

Define dilute in the context of solutions.

A

Dilute: a description of a solution that contains a relatively low amount of solute for a given quantity of solvent; opposite of concentrated.

A dilute solution has a higher solvent to solute ratio.

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13
Q

What is the definition of dynamic equilibrium?

A

A state of balance achieved by two forces in motion
- amount of solid dissolving is equal to the amount of solid crystalizing

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14
Q

What do aqueous solutions of certain cations and anions have?

A

Distinct colours.

Examples of cations include Ni2+, Fe3+, and Cu2+.

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15
Q

What do many substances do in water to form ions?

A

Dissociate

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16
Q

What do ionic compounds do upon dissolving according to Arrhenius?

A

they dissociate into positive and negative ions.

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17
Q

What occurs when a student dissolves a solute and the test tube feels warm?

A

The dissolving process is exothermic

This indicates the process releases energy to the surroundings.

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18
Q

What effect does decreased dissolved oxygen have on aquatic wildlife?

A

It negatively affects aquatic wildlife.

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19
Q

What do many metals produce when heated?

A

A distinctive colour of flame.

This occurs due to the thermal excitation of electrons.

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20
Q

What types of solutes and solvents can be involved in solutions?

A

solids, liquids, or gases

Various combinations lead to different types of solutions.

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21
Q

What is water commonly referred to as?

A

the universal solvent

This is due to its ability to dissolve a wide variety of substances.

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22
Q

How can you determine the presence of specific ions in an unknown solution?

A

By adding a known solution to see if a precipitate forms.

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23
Q

What happens to soluble (polar) molecular compounds in a solvent?

A

the solute particles distribute evenly through the solvent.

*forms homogeous solution

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24
Q

Define an electrolyte.

A

An electrolyte is a substance that when dissolved in water will create a solution that conducts electricity. ions

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25
Fill in the blank: The _______ equation shows only the chemical change that occurs.
net ionic ## Footnote The net ionic equation focuses on the ions that participate in the reaction.
26
What is biomagnification?
The process by which the concentration of toxic substances increases in each successive link in the food chain ## Footnote Biomagnification poses serious health risks to higher order mammals, including humans.
27
True or False: A homogeneous mixture may appear to contain only one substance with uniform properties.
True
28
What should you do after dissolving the solute in water?
Transfer the solution to a 100 mL volumetric flask
29
Define a heterogeneous mixture.
A heterogeneous mixture contains more than one type of particle in which the particles do not have a uniform concentration throughout the mixture.
30
What does low solubility indicate?
a substance does not dissolve well in water.
31
True or False: Solid solutes behave similarly to gas solutes in terms of solubility.
False
32
What is solubility?
the ability of a solute to dissolve in a solvent.
33
What does high solubility indicate?
a substance dissolves well in water.
34
What are spectator ions?
Ions that do not change in the reaction ## Footnote Spectator ions are cancelled out in the net ionic equation.
35
After measuring the solute, what is the next step in preparing the solution?
Dissolve the solute in 50 mL of water
36
What are quantitative properties?
Quantitative properties are numerical values assigned to the substance such as concentration.
37
How do polar and non-polar substances differ in solubility?
polar substances have high solubility and non-polar substances have low solubility.
38
What is a solution?
A solution is a type of homogeneous mixture composed of at least one solute and one solvent.
39
What is a precipitate?
A precipitate is an insoluble substance that forms when two solutions are mixed together.
40
What will happen to the amount of dissolved oxygen in a waterway if the ambient temperature is raised?
It will decrease.
41
What is required to calculate the concentration of individual ions?
Dissociation equations
42
What occurs when a student dissolves a solute and the test tube feels cool?
The dissolving process is endothermic ## Footnote This indicates the process absorbs energy from the surroundings.
43
True or False: Milk and fog are examples of solutions.
False
44
Define a homogeneous mixture.
A homogeneous mixture contains more than one type of particle in which the particles have a uniform concentration throughout the mixture.
45
What is the role of the solvent in a solution?
The solvent is the part of the solution that is present in larger amounts and does the dissolving.
46
What happens to the concentration of toxins as one moves up the food chain?
The concentration of toxins increases ## Footnote This occurs due to greater biomass being consumed by higher level consumers.
47
What is necessary for calculating the concentration of ions?
Amount concentration of the solution and a balanced chemical formula
48
What happens to a salt crystal in a dynamic equilibrium system?
A salt crystal is both dissolving and crystallizing at the same rate (mass of the crystal remains constant)
49
What process do soluble ionic solutes undergo when dissolving?
dissociation.
50
How do you determine the total energy change during dissolving?
Energy absorbed (broken) - energy released (formed) = total change in energy ## Footnote This equation helps identify if the process is endothermic or exothermic.
51
What can solubility values be used to calculate?
The maximum amount of solute that would be present or dissolve in various volumes of solution.
52
True or False: Any units of concentration or volume may be used in the dilution formula.
True. ## Footnote However, the units must be consistent throughout the calculation.
53
How does temperature affect the solubility of most solid solutes?
Most solids have higher solubility at higher temperatures.
54
In a true solution, what happens to the solute particles?
The solute particles do not separate from the solvent on standing, nor can they be filtered out.
55
What is a net ionic equation?
An equation that shows only the chemical change that occurs ## Footnote It excludes spectator ions that do not participate in the reaction.
56
Which elements are noted for their low solubility?
most elements, with examples like oxygen and chlorine.
57
What does c1 represent in the dilution formula?
c1 = initial concentration of solution. ## Footnote It indicates the concentration before dilution.
58
What is dissociation?
the process where an ion or molecule reacts in solution to create ions. | - ionics
59
Define an element.
An element is a chemical substance that consists of particles that contain only one type of atom.
60
What occurs in the final step of a solid dissolving in water?
Bonds form between water molecules and the ions, which is exothermic ## Footnote This step releases energy, warming the surrounding water.
61
Fill in the blank: Aqueous is the state given to a solution that is formed with a substance dissolved in _______.
water
62
What is a mixture?
A mixture consists of two or more substances and may be subcategorized as either homogeneous or heterogeneous.
63
What process do soluble molecular compounds undergo when dissolving?
dispersion.
64
True or False: In an endothermic change, the energy needed to break bonds is greater than the energy released when new bonds form.
True ## Footnote This indicates that the process absorbs energy.
65
What is dispersion in the context of dissolving?
the process of particles spreading evenly in a solution. | -molecular
66
What is an endothermic process?
A process that absorbs energy from the surroundings, making the surroundings cooler ## Footnote Endothermic processes require energy to break bonds.
67
What is the relationship between the rates of crystallization and dissolving in a dynamic equilibrium?
Must be occurring at exactly the same rate.
68
What happens to the solubility of gas solutes when conditions change to SATP?
It is expected to change, but the specific direction (increase or decrease) depends on the gas.
69
How does temperature affect the solubility of gas solutes?
Gases have lower solubility at higher temperatures.
70
What does V2 represent in the dilution formula?
V2 = final volume of solution. ## Footnote It indicates the volume after dilution.
71
What is a precipitation reaction?
A double replacement reaction in which a solid product (the precipitate) is formed.
72
What is the general trend in solubility for ionic compounds?
use the solubility table to predict their solubility.
73
What is an alloy?
An alloy is a solution created by mixing gold with other metals to improve strength and appearance.
74
what does 1 ppm equal?
1 ppm = 1mg/L
75
What is a stock solution?
A stock solution is a concentrated solution that is used in the preparation of more dilute solutions of the same solute. ## Footnote Stock solutions are commonly prepared in laboratories.
76
What does c2 represent in the dilution formula?
c2 = final concentration of solution. ## Footnote It indicates the concentration after dilution.
77
What is the dilution formula?
The dilution formula is c1 V1 = c2 V2. ## Footnote This formula relates the concentrations and volumes before and after dilution.
78
What is a soluble substance?
A soluble substance is one that will dissolve in water.
79
Define cation.
A cation is a positively charged ion that forms when a metallic atom loses electrons.
80
Define anion.
An anion is a negatively charged ion formed when a non-metallic atom gains electrons.
81
What are qualitative properties?
Qualitative properties are descriptions of quality such as colour, conductivity, solubility, and precipitates.
82
What is dilution?
Dilution is the process of increasing the amount of solvent, resulting in a less concentrated solution. ## Footnote Dilution decreases the concentration of solute in a solution.
83
What is a total ionic equation?
An equation that shows all soluble reactants and products dissociated into ions ## Footnote This type of equation provides a more accurate representation of the reaction.
84
What is an exothermic process?
A process that releases energy into the surroundings, warming the surroundings ## Footnote Exothermic processes occur when new bonds form.
85
Miscible substance:
capable of being mixed; they are usually two liquids that will mix together in all proportions.two liquids
86
What is an insoluble substance?
An insoluble substance is one that will not dissolve in water.
87
What factors affect solubility?
Temperature and pressure.
88
How do you ensure the solution is mixed properly in the volumetric flask?
Fill the flask to 100 mL and mix by inverting (use rubber stopper)
89
What is the difference between electrolytes and non-electrolytes?
Electrolytes dissociate; non-electrolytes dissolve but do not dissociate.
90
What level of a food pyramid contains the highest quantity of contamination?
The top level ## Footnote This level has the highest concentration due to biomagnification.
91
Which quantities do not change during dilution?
The amount of solute does not change. ## Footnote Only the concentration and volume of the solution change.
92
What are the two ways to make a solution?
* Dissolve a measured amount of pure solute in a certain volume of solvent * Dilute a standard solution
93
What happens when electrons return to their original energy level?
They emit visible light.
94
What do equilibrium arrows indicate in a chemical equation?
Equilibrium arrows indicate that both the forward and reverse processes are occurring at the same time.
95
Define concentrated in the context of solutions.
Concentrated: a description of a solution that has a high amount of solute for a given amount of solvent; opposite of dilute. ## Footnote A concentrated solution has a lower solvent to solute ratio.
96
What are the three steps in net ionic equations?
1. Ionic equations (Balanced reaction) 2. Total Ionic equations 3. Net ionic equation ## Footnote These steps outline the process of deriving net ionic equations from balanced chemical reactions.
97
ionization:
the process where neutral molecules, like those of acids or bases(non ionic), break down into charged particles called ions when dissolved in a solvent
98
What happens to the mass of solid at the bottom of a saturated solution of copper(II) sulfate at SATP?
The amount of solid will remain the same ## Footnote Some of the solid is dissolving, and an equal amount of solid is crystallizing out of the solution.
99
What is a pure substance?
A pure substance consists of one chemical only and may be subcategorized as either an element or a compound.
100
How do you prepare a solution of known concentration from a solid solute?
Follow these steps: 1. Calculate the mass of the solute required. 2. Dissolve the solute in half the final volume of solvent. 3. Transfer to a volumetric flask. 4. Fill to the final volume and mix.
101
Fill in the blank: A heat pack contains calcium chloride and water. When the pouch is broken, the calcium chloride _______.
dissolves ## Footnote The dissolution of calcium chloride is an endothermic process.
102
What distinguishes aqueous solutions from mixtures?
Aqueous solutions are transparent, not cloudy, indicating they are true solutions. - aqueous solutions are homogeneous mixtures where the substances are completely and evenly dissolved, while aqueous mixtures can be heterogeneous or homogeneous where the substances may not be fully dissolved or evenly distributed
103
How does pressure affect the solubility of gas solutes?
Gases have higher solubility at higher pressures.
104
What processes are occurring simultaneously in a dynamic equilibrium involving a salt crystal?
* Crystallization * Dissolving
105
True or False: In an exothermic change, the energy released to form new bonds is greater than the energy required to break existing bonds.
True ## Footnote This indicates that the process releases energy.
106
What must you always list when identifying entities in a dissolving process?
water H₂O(l).
107
Immiscible substance:
incapable of being mixed; they are usually two liquids that will not mix together
108
Is the formation of bonds and the breaking of bonds endo or exothermic?
Bond breaking is an endothermic process, because it requires energy. Bond forming is an exothermic process, because it releases energy.

Chem 20 (3 decks)

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