Solutions Flashcards
1
Q
What is a solution?
A
A solution is a homogenous mixture of two or more substances.
2
Q
What are the components of a solution?
A
A solution is made up of two components: solute and solvent.
3
Q
What is a binary solution?
A
A binary solution consists of two components, like salt dissolved in water.
4
Q
What is an aqueous solution?
A
An aqueous solution is formed by dissolving a substance in water, where water is the solvent.
5
Q
What is the role of water in aqueous solutions?
A
Water is a universal solvent because it can dissolve a large number of substances, especially ionic and polar covalent compounds.
6
Q
What is the solute in a solution?
A
The solute is the component of the solution that is present in a smaller amount.
7
Q
What is the solvent in a solution?
A
The solvent is the component of the solution that is present in a larger amount.
8
Q
What is an example of a solute and solvent in a solution?
A
In a sugar solution, sugar is the solute, and water is the solvent.
9
Q
What is a saturated solution?
A
A saturated solution is one in which no more solute can dissolve at a particular temperature.
10
Q
What happens when more solute is added to a saturated solution?
A
If more solute is added to a saturated solution, it will remain undissolved and settle at the bottom.
11
Q
How do you prepare a saturated solution of NaCl in water?
A
To prepare a saturated solution of NaCl, add NaCl to water until no more dissolves at room temperature.
12
Q
What is a 2M solution of NaOH?
A
A 2M solution of NaOH is prepared by dissolving 20g of NaOH in water and making the volume up to 250 mL.
13
Q
What is a 0.1M solution of NaCl?
A
A 0.1M solution of NaCl is prepared by dissolving 5.85g of NaCl in water and making the volume up to 1000 mL.
14
Q
What is an unsaturated solution?
A
An unsaturated solution is one that has less solute than required to saturate it at a particular temperature.
15
Q
How can you tell if a solution is unsaturated?
A
If you add more solute to the solution and it dissolves, it is unsaturated.
16
Q
What is a supersaturated solution?
A
A supersaturated solution contains more solute than required to form a saturated solution at a particular temperature.
17
Q
How is a supersaturated solution created?
A
A supersaturated solution is created by heating a saturated solution and then adding more solute that would normally not dissolve at that temperature.
18
Q
What happens when a crystal is added to a supersaturated solution?
A
When a crystal is added to a supersaturated solution, excess solute may deposit on the crystal.
19
Q
How can you distinguish between unsaturated, saturated, and supersaturated solutions?
A
In an unsaturated solution, the solute dissolves. In a saturated solution, the solute remains undissolved. In a supersaturated solution, excess solute may deposit on the crystal.
20
Q
Can a supersaturated solution dissolve more solute?
A
Yes, a supersaturated solution can dissolve more solute than a saturated one at the same temperature.
21
Q
How many types of solutions exist based on physical states?
A
There are nine types of solutions: gaseous solutions, liquid solutions, and solid solutions.
22
Q
What is a gaseous solution?
A
A gaseous solution is a mixture where gas is dissolved in another gas, liquid, or solid.
23
Q
What is an example of a gas in a gas solution?
A
Air is a gaseous solution where oxygen is dissolved in nitrogen.
24
Q
Give an example of a gas in a liquid solution.
A
Carbon dioxide dissolved in water is an example of a gas in a liquid solution (e.g., carbonated drinks).
25
How is a gas in a solid solution formed?
Hydrogen gas dissolved in palladium is an example of a gas in a solid solution.
26
What is a liquid solution?
A liquid solution is a mixture where a liquid solute is dissolved in a liquid solvent, solid, or gas.
27
Give an example of a liquid in a gas solution.
Water vapor in air is an example of a liquid in a gas solution.
28
Give an example of a liquid in a liquid solution.
Alcohol dissolved in water is an example of a liquid in a liquid solution.
29
What is a liquid in solid solution?
Mercury dissolved in gold is an example of a liquid in solid solution (amalgam).
30
What is a solid solution?
A solid solution is a mixture where a solid solute is dissolved in a solid solvent or in liquid.
31
Give an example of a solid in gas solution.
Smoke, which consists of carbon particles dissolved in air, is an example of a solid in gas solution.
32
Give an example of a solid in liquid solution.
Salt dissolved in water is an example of a solid in liquid solution.
33
Give an example of a solid in solid solution.
Brass, an alloy of copper and zinc, is an example of a solid in solid solution.
34
How is brass made?
Brass is made by dissolving zinc in copper, creating a solid solution.
35
What is sterling silver made of?
Sterling silver is made of 92.5% silver and 7.5% copper, forming a solid solution.
36
What is bronze made of?
Bronze is an alloy of copper and tin, forming a solid solution.
37
What are the three categories of substances used in daily life?
The three categories are gaseous solutions, liquid solutions, and solid solutions.
38
What is an example of a gaseous solution?
Air is a gaseous solution made of different gases such as nitrogen (N2), oxygen (O2), and carbon dioxide (CO2).
39
What is a liquid solution?
A liquid solution is a mixture where a solute is dissolved in a solvent. Examples include drinking water, beverages, vinegar, and medicines.
40
Give an example of a solid solution.
Brass, an alloy of copper and zinc, is an example of a solid solution. Jewelry is also made from solid solutions of gold and copper or silver.
41
Why is pure gold not used for jewelry?
Pure gold is very soft, so it is mixed with copper or silver to make it harder and suitable for jewelry.
42
What is the definition of concentration of a solution?
Concentration is the proportion of solute in a solution. It measures the amount of solute present in a given amount of solvent or solution.
43
What is a dilute solution?
A dilute solution contains a small amount of solute dissolved in the solvent.
44
What is a concentrated solution?
A concentrated solution contains a large amount of solute dissolved in the solvent.
45
What is a standard solution?
A standard solution is a solution of known concentration.
46
Give an example of a dilute solution.
A solution with 5g of sugar dissolved in 100cm³ of water is a dilute solution compared to a solution with 8g of sugar in the same amount of water.
47
What is the difference between a dilute and concentrated solution?
A dilute solution has fewer solute particles per unit volume, while a concentrated solution has more solute particles per unit volume.
48
What is percentage composition in relation to solutions?
Percentage composition is the number of parts of solute present in 100 parts of solution or the fraction of solute in a solution multiplied by 100.
49
What is Percentage Mass by Mass?
Percentage Mass by Mass (m/m) is the number of grams of solute present in 100 grams of solution. Example: A 10% sugar solution means 10 grams of sugar in 90 grams of solvent, making the total solution weight 100 grams.
50
What is the formula for Percentage Mass by Mass?
% mass/mass = (mass of solute / mass of solution) x 100
51
What is Percentage Mass by Volume?
Percentage Mass by Volume (m/v) is the number of grams of solute present in 100 cm³ of solution. Example: A 10% NaCl solution means 10 grams of NaCl in enough solvent to make 100 cm³ of solution.
52
What is the formula for Percentage Mass by Volume?
% mass/volume = (mass of solute / volume of solution) x 100
53
What is Percentage Volume by Mass?
Percentage Volume by Mass (v/m) is the volume in cm³ of solute dissolved in 100 grams of solution. Example: A 10% alcohol solution means 10 cm³ of alcohol in solvent to make a 100-gram solution.
54
What is the formula for Percentage Volume by Mass?
% volume/mass = (volume of solute / mass of solution) x 100
55
What is Percentage Volume by Volume?
Percentage Volume by Volume (v/v) is the volume in cm³ of solute dissolved per 100 cm³ of solution. Example: A 10% alcohol solution means 10 cm³ of alcohol in solvent to make 100 cm³ of solution.
56
What is the formula for Percentage Volume by Volume?
% volume/volume = (volume of solute / volume of solution) x 100
57
What is Molarity (M)?
Molarity is the concentration unit defined as the number of moles of solute dissolved per dm³ (liter) of solution. It is represented by 'M'.
58
What is the formula for Molarity?
M = (moles of solute) / (volume of solution in dm³)
59
What is the calculation of molarity for 7.50 mol of CaCO₃ in 1.50 dm³ solution?
Molarity = (7.50 mol) / (1.50 dm³) = 5.0 M
60
What is the unit for molarity?
The unit for molarity is mol/dm³, which is also equivalent to mol/L (moles per liter).
61
What is the formula for molarity?
Molarity (M) is the number of moles of solute per liter (dm³) of solution. M = (moles of solute) / (volume of solution in dm³)
62
What does a 1M NaOH solution mean?
A 1M NaOH solution means that 1 mole (40 grams) of NaOH is dissolved in 1 dm³ (liter) of solution.
63
What happens if 20.0g of NaOH is dissolved in 1 dm³ of solution?
If 20.0g of NaOH is dissolved in 1 dm³ of solution, the molarity will be 0.500M NaOH.
64
How do you calculate the molarity of a solution with a given mass of solute?
Molarity (M) = (mass of solute in grams) / (molar mass of solute) x (volume of solution in dm³)
65
What is the molarity if 80.0g of NaOH is dissolved in 1 dm³ of solution?
If 80.0g of NaOH is dissolved in 1 dm³ of solution, the molarity will be 2M NaOH.
66
What is solubility?
Solubility is the amount of solute that can dissolve in a given amount of solvent to form a saturated solution at a specific temperature.
67
What factors affect solubility?
Factors affecting solubility include temperature, pressure, nature of the solute, and nature of the solvent.
68
What is the solubility rule 'like dissolves like'?
'Like dissolves like' means that polar substances dissolve in polar solvents, and non-polar substances dissolve in non-polar solvents. For example, NaCl dissolves in water but not in benzene.
69
How does the nature of the solute affect solubility?
The solubility of a solute changes depending on its nature. For example, sodium chloride has high solubility in water, while sugar has lower solubility.
70
What is an example of an ionic compound with high solubility in water?
Sodium chloride (NaCl) is an example of an ionic compound that has high solubility in water.
71
How does temperature affect solubility?
Generally, the solubility of solids in liquids increases with temperature. However, the solubility of gases decreases as temperature increases.
72
What does the principle 'like dissolves like' mean?
'Like dissolves like' means that polar substances dissolve in polar solvents, and non-polar substances dissolve in non-polar solvents.
73
Are non-polar substances soluble in polar solvents?
No, non-polar substances (like benzene and petrol) are insoluble in polar solvents (like water).
74
What is the solubility of grease or paint in non-polar solvents?
Grease and paint are soluble in non-polar solvents like petrol, ether, or carbon tetrachloride.
75
Why is lithium chloride (LiCl) soluble in water but not in gasoline?
LiCl is soluble in water due to the polarity of water molecules that can interact with and hydrate the ions in LiCl, whereas gasoline is non-polar and cannot interact with LiCl ions.
76
What happens when an ionic compound like lithium chloride (LiCl) is dissolved in water?
When LiCl dissolves in water, the positive and negative ions are surrounded by water molecules, a process known as hydration.
77
Why are ionic compounds insoluble in non-polar solvents like benzene?
Ionic compounds are generally insoluble in non-polar solvents because the solvent molecules cannot attract the ions strongly enough to overcome the ionic bonds holding the crystal together.
78
What are immiscible liquids?
Immiscible liquids are liquids that do not dissolve in each other and form two separate phases, like water and benzene.
79
Which liquids are completely miscible?
Liquids that dissolve freely in each other in any proportion, like benzene and carbon tetrachloride, are completely miscible.
80
Why are water and benzene immiscible?
Water and benzene are immiscible because they have different polarities—water is polar, while benzene is non-polar, and their molecules don't interact well with each other.
81
What is the process of hydration when dissolving ionic compounds in water?
Hydration is the process where water molecules surround and interact with the ions in an ionic compound, pulling them away from the crystal to form a solution.
82
What is meant by 'like dissolves like' in solubility?
'Like dissolves like' means that substances with similar intermolecular forces (polar with polar, non-polar with non-polar) are more likely to dissolve in each other.
83
What happens when ethanol is mixed with water?
Ethanol and water mix freely because both substances can form hydrogen bonds due to the presence of the -OH group on ethanol.
84
How does pressure affect the solubility of gases?
The solubility of gases increases with pressure. For example, carbon dioxide is dissolved in soda water under pressure, and when the bottle is opened, the gas escapes due to the pressure reduction.
85
What happens when soda water is opened?
When a soda bottle is opened, the pressure inside the bottle is released, causing the solubility of carbon dioxide to decrease, which leads to effervescence (bubbles).
86
What type of substances dissolve well in water?
Polar and ionic substances dissolve well in water because water is a polar solvent.
87
Does the solubility of solids and liquids change with pressure?
No, solids and liquids are incompressible, so their solubility is not affected by changes in pressure.
88
What was observed in the Activity 6.2 experiment when different solutes were mixed with water or methylated spirit?
In the experiment, some solutes dissolved in the solvent (e.g., salt in water), while others did not (e.g., iodine in water).
89
What is the effect of mixing equal volumes of alcohol and water?
When equal volumes of alcohol and water are mixed, the total volume of the mixture decreases rather than increasing due to molecular interactions.
90
What is the relationship between intermolecular forces and solubility?
Solutes with similar intermolecular forces to the solvent tend to dissolve better in the solvent, as their forces interact more effectively.
91
What happens to the solubility of gases with an increase in temperature?
"The solubility of gases decreases as temperature increases because the kinetic energy of the molecules increases
92
Does the solubility of solids in liquids always increase with temperature?
"No
93
Which salts show increased solubility with higher temperatures?
"Potassium nitrate (KNO3)
94
Which salts show decreased solubility with higher temperatures?
"Cerium sulfate (Ce2(SO4)3)
95
What happens to the solubility of sodium sulfate at 32.4°C?
"At 32.4°C
96
What is a solution?
A solution is a homogeneous mixture of two or more components where the solute and solvent cannot be easily differentiated. Example: salt solution.
97
Solutions can be separated by filtration. True or False?
False
98
The Tyndall effect occurs when light is scattered by __________ particles in a colloidal dispersion.
colloidal
99
What is an example of a colloidal system?
An example of a colloidal system is the mixture of starch in water.
100
Which of the following is a true solution? \n(a) Milk \n(b) Saltwater \n(c) Gelatin \n(d) Paint
(b) Saltwater
101
What phase in colloids refers to liquid dispersed in solid?
Solid emulsion is the phase where liquid is dispersed in solid.
102
Which of the following is more likely to dissolve a polar solute like AgCl? \n(a) CH4 \n(b) NH3
(b) NH3
103
Which type of solvent is more likely to dissolve alcohol or CH3OH: polar or non-polar?
Polar solvent is more likely to dissolve alcohol or CH3OH.
104
Colloidal particles can be seen with the naked eye. True or False?
False
105
Which solvent is more likely to dissolve nonpolar substances, like CH4? \n(a) Water \n(b) Benzene
(b) Benzene
106
Colloidal particles do not settle at the bottom of the container. True or False?
True
107
A colloid is a mixture where solute particles are large enough to be seen with the naked eye. True or False?
False
108
Which of the following is an example of an aerosol? \n(a) Milk \n(b) Smoke \n(c) Gelatin \n(d) Paint
(b) Smoke
109
Fill in the blank: Colloidal particles are typically between ________ and 100 nm in diameter.
1 nm
110
Which of the following is an example of a liquid emulsion? \n(a) Mayonnaise \n(b) Paint \n(c) Saltwater \n(d) Gelatin
(a) Mayonnaise
111
Solutions are homogeneous mixtures. True or False?
True
112
AgCl is more likely to dissolve in __________ because both are polar.
NH3
113
What happens when a colloid is allowed to stand for a long time?
The colloidal particles do not settle at the bottom.
114
Which is NOT a characteristic of a colloid? \n(a) The particles scatter light \n(b) The particles are visible to the naked eye \n(c) The particles are in a dispersed phase \n(d) The particles cannot be separated by filtration
(b) The particles are visible to the naked eye
115
In a colloid, solute particles are larger than those in a true solution. True or False?
True
116
Which of these is an example of a colloid? \n(a) Salt solution \n(b) Milk \n(c) Water \n(d) Air
(b) Milk
117
Fill in the blank: The particles in a true solution cannot be separated by __________.
filtration
118
Which of the following is a gel colloid? \n(a) Paint \n(b) Gelatin \n(c) Milk \n(d) Whipped cream
(b) Gelatin
119
What is a suspension?
A suspension is a heterogeneous mixture of undissolved particles in a given medium, where the composition is not uniform.
120
In a suspension, particles are small enough to pass through filter paper. True or False?
False
121
Suspended particles in a suspension settle down at the bottom due to __________.
sedimentation
122
Which of the following is an example of a suspension? \n(a) Salt solution \n(b) Muddy water \n(c) Milk \n(d) Air
(b) Muddy water
123
Suspensions are homogeneous mixtures. True or False?
False
124
What is the process of separating clear liquid from settled particles called?
Decantation
125
What size are the particles in a suspension?
Particles in a suspension are over 1000 nm in size.
126
Which of the following medicines needs to be shaken before use? \n(a) Antibiotics \n(b) Paracetamol \n(c) Antiacid \n(d) All of the above
(d) All of the above
127
Suspension particles can be seen with the naked eye. True or False?
True
128
Which of the following is NOT a property of a suspension? \n(a) Particles settle down \n(b) Particles can pass through filter paper \n(c) Particles are large enough to be seen \n(d) Can be separated by filtration
(b) Particles can pass through filter paper
129
Fill in the blank: In a suspension, particles are large enough to be seen with the __________ eye.
naked
130
What happens to suspended particles when left for some time?
They settle at the bottom of the container.
131
Which of the following is an example of a colloid? \n(a) Salt solution \n(b) Muddy water \n(c) Milk \n(d) Flour in water
(c) Milk
132
Which of the following mixtures can be filtered? \n(a) Solution \n(b) Colloid \n(c) Suspension \n(d) All of the above
(c) Suspension
133
Fill in the blank: A suspension is a __________ mixture of particles.
heterogeneous
134
What is the size of particles in a colloid?
Particles in a colloid range from 1 to 1000 nm in size.
135
Which property distinguishes a colloid from a suspension? \n(a) Particle size \n(b) Homogeneity \n(c) Ability to scatter light \n(d) Settling of particles
(a) Particle size
136
Suspensions may scatter light, but they are not transparent. True or False?
True
137
Which is an example of a solution? \n(a) Milk \n(b) Salt in water \n(c) Mud in water \n(d) Flour in water
(b) Salt in water
138
What property distinguishes a suspension from a true solution?
A suspension has larger particles that settle down, whereas a true solution has smaller particles that do not settle.
139
Which of the following cannot be separated by filtration? \n(a) Solution \n(b) Colloid \n(c) Suspension
(a) Solution
140
What is molarity?
Molarity is the number of moles of solute dissolved per dm³ (liter) of solution.
141
Solubility refers to the amount of solute in grams dissolved in 100 grams of solvent to prepare a saturated solution at a given temperature. True or False?
True
142
Which of the following are immiscible liquids? \n(a) Water and alcohol \n(b) Oil and water \n(c) Salt and water \n(d) Alcohol and vinegar
(b) Oil and water
143
What size are the particles in a colloidal solution?
Particles in a colloidal solution range from 1 nm to 1000 nm in diameter.
144
What effect occurs when light is scattered by colloidal particles in a transparent medium?
The Tyndall effect occurs when light is scattered by colloidal particles in a transparent medium.
145
In a suspension, particles are large enough to be seen with the naked eye. True or False?
True
146
The process of particles settling at the bottom of a suspension is called __________.
sedimentation
147
Which solution contains more solute than required to saturate it at a given temperature?
A supersaturated solution contains more solute than required to saturate it at a given temperature.
148
Which of the following is an example of a saturated solution? \n(a) Sugar in water at room temperature \n(b) Sugar in water at high temperature \n(c) Sugar in water after it dissolves completely
(a) Sugar in water at room temperature
149
Which of the following is true for a supersaturated solution? \n(a) It cannot dissolve any more solute \n(b) It contains more solute than required to saturate it at a given temperature \n(c) It is a dilute solution
(b) It contains more solute than required to saturate it at a given temperature
150
Fill in the blank: A solution is a __________ mixture of two or more substances.
homogeneous
151
Which solution can dissolve further solute at a given temperature? \n(a) Saturated solution \n(b) Unsaturated solution \n(c) Supersaturated solution
(b) Unsaturated solution
152
Which of the following is NOT a property of a colloidal solution? \n(a) Particles are intermediate in size between those of a solution and a suspension \n(b) Particles are large enough to be seen with the naked eye \n(c) Tyndall effect is observed \n(d) Particles cannot be separated by filtration
(b) Particles are large enough to be seen with the naked eye
153
Water is a universal solvent. True or False?
True
154
Which of the following statements is correct? \n(a) A saturated solution can dissolve further solute \n(b) A supersaturated solution cannot dissolve more solute \n(c) A dilute solution has a high concentration of solute
(b) A supersaturated solution cannot dissolve more solute
155
Which of the following is the definition of a concentrated solution? \n(a) A solution with a small amount of solute \n(b) A solution with a large amount of solute
(b) A solution with a large amount of solute
156
Fill in the blank: A dilute solution contains a __________ amount of solute dissolved in the solvent.
small
157
What is the concentration of a solution a measure of?
The concentration of a solution is a measure of the amount of solute in a given amount of solvent or solution.
158
Which of the following liquids dissolve freely in one another in any proportion? \n(a) Immiscible liquids \n(b) Miscible liquids \n(c) Suspensions
(b) Miscible liquids
159
Percentage concentration of a solution is the number of parts of solute present in __________ parts of solution.
100
160
Which of the following is an example of a colloid? \n(a) Sugar in water \n(b) Milk \n(c) Salt in water \n(d) Alcohol in water
(b) Milk
161
What is the solvent in an aqueous solution?
Water is the solvent in an aqueous solution.
162
Which of the following solutions is more dilute? \n(a) 1.0M \n(b) 0.05M
(b) 0.05M
163
Milk is an example of: \n(a) Solution \n(b) Colloids solution \n(c) Suspension
(b) Colloids solution
164
Water droplet in air is an example of: \n(a) Gas in gas \n(b) Liquid in gas \n(c) Liquid in liquid
(b) Liquid in gas
165
When there is a low concentration of solute in a solution, it is known as: \n(a) Dilute solution \n(b) Saturated solution \n(c) Concentrated solution
(a) Dilute solution
166
What is the molarity of a NaNO₃ solution made by diluting 250.0 cm³ of a 1.60 M solution to a final volume of 400 cm³?
(b) 0.200 M
167
What is the concentration, in % mass by volume (m/v), of a solution containing 15.0 g KCl in 600.0 cm³ solution? \n(a) 1% \n(b) 3% \n(c) 2% \n(d) 0.005%
(b) 3%
168
When KCl dissolves in water, the following will be produced: \n(a) 1 kg of solvent \n(b) 1 dm³ of solvent \n(c) 1 kg of solution \n(d) Super saturated solution
(c) 1 kg of solution
169
What is the molarity of a Na₂SO₄ solution when 2 moles of Na₂SO₄ are dissolved in 1 dm³ of solution? \n(a) 0.4 M \n(b) 1.0 M \n(c) 0.2 M \n(d) 0.16 M
(b) 1.0 M
170
Molarity is the number of moles of solute dissolved in: \n(a) 1 kg of solvent \n(b) 1 kg of solution \n(c) 1 dm³ of solution \n(d) 1 dm³ of solvent
(c) 1 dm³ of solution
171
The molarity of a NaOH solution by dissolving 4 g of it in 250 mL of water is: \n(a) 0.8 M \n(b) 2.0 M \n(c) 0.5 M \n(d) 0.1 M
(d) 0.1 M
