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Total questions: 47
Worksheet time: 2hrs 34mins
Which of the following usually makes a substance dissolve faster in a solvent?
agitating the solution
increasing the particle size of the solute
lowering the temperature
decreasing the number of particles
What is the maximum amount of KCl that can dissolve in 200 g of water?
(The solubility of KCl is 34 g/100 g H2O at 20C.)
17 g
34 g
68 g
6900g
What is the solubility of silver nitrate if only 11.1 g can dissolve in 5.0 g of water at 20 degrees C?
2.2 g/ 100 g H2O
45 g/ 100 g H2O
22.2 g/ 100 g H2O
222 g/ 100 g H2O
Which of the following expressions is generally used for solubility?
grams of solute per 100 grams of solvent
grams of solute per 100 milliliters of solvent
grams of solute per 100 grams of solution
grams of solute per 100 milliliters of solution
Which of the following pairs of factors affects the solubility of a particular substance?
temperature and the nature of solute and solvent
temperature and degree of mixing
particle size and degree of mixing
particle size and temperature
If a crystal added to an aqueous solution causes many particles to come out of solution, the solution was
unsaturated
saturated
an emulsion
supersaturated
Which of the following substances is less soluble in hot water than in cold water?
Carbon dioxide
sodium chloride
sodium nitrate
potassium bromide
Which of the following occurs as temperature increases?
Solubility decreases.
Solubility increases.
Solubility remains the same.
Molarity doubles.
The solubility of a gas in a liquid is ____.
proportional to the square root of the pressure of the gas above the liquid
directly proportional to the pressure of the gas above the liquid
inversely proportional to the pressure of the gas above the liquid
unrelated to the pressure of the gas above the liquid
What happens to the solubility of a gas, in a liquid, if the partial pressure of the gas above the liquid decreases?
The solubility decreases.
The solubility increases.
The solubility remains the same.
The solubility cannot be determined.
In a concentrated solution there is ____.
no solvent
a large amount of solute
a small amount of solute
no solute
What is the molarity of a solution that contains 6 moles of solute in 2 liters of solution?
6M
12M
7M
3M
In which of the following is the solution concentration expressed in terms of molarity?
10 g solute/1000g solution
10 g solute/1000 mL solution
10 mL solute/1000 L solution
10 mol/ 1 L solution
Which of the following operations yields the number of moles of solute?
molarity moles of solution
molarity liters of solution
molarity mass of solution
moles of solution volume of solution
What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution
81 M
0.081 M
12 M
4.0 M
What is the molarity of 200 mL of solution in which 2.0 moles of sodium bromide is dissolved?
2.0M
10M
0.40M
4.0M
What is the number of moles of solute in 250 mL of a 0.4M solution?
0.1 mol
0.16 mol
0.62 mol
1.6 mol
What is the molarity of a solution containing 56 grams of solute in 959 mL of solution (molar mass= 26 g/mol)
1.5 M
2.2 M
2.1 M
0.0022 M
What mass of sucrose, C12H22O11, is needed to make 500.0 mL of a 0.200M solution?
34.2 g
100 g
17.1 g
68.4 g
What mass of Na2SO4 is needed to make 2.5 L of 2.0M solution?
178 g
284 g
356 g
710 g
What does NOT change when a solution is diluted by the addition of solvent?
volume of solvent
mass of solvent
number of moles of solute
molarity of solution
How many mL of a 2.0M NaBr solution are needed to make 200.0 mL of 0.50M NaBr?
25 mL
50 mL
100 mL
150 mL
The volume of 6.00 M HCl needed to make 319 mL of 6.80 M HCl is _____.
0.128 mL
6.8 mL
281 mL
362 mL
If 2.0 mL of 6.0M HCl is used to make a 500.0-mL aqueous solution, what is the molarity of the dilute solution?
0.024M
0.24M
0.30M
0.83M
To 225 mL of a 0.80M solution of KI, a student adds enough water to make 1.0 L of a more dilute KI solution. What is the molarity of the new solution?
180M
2.8M
0.35M
0.18M
If the percent by volume is 2.0% and the volume of solution is 250 mL, what is the volume of solute in solution?
0.5 mL
1.25 mL
5.0 mL
12.5 mL
In which of the following is concentration expressed in percent by volume?
10% (v/v)
10% (m/v)
10% (m/m)
10%
If the percent (mass/mass) for a solute is 4% and the mass of the solution is 200 g, what is the mass of solute in solution?
8.0 g
50 g
80 g
800 g
The volume of rubbing alcohol present in 620 mL of 40% (v/v) solution is_____.
372 mL
40.0 mL
248 mL
580 mL
How many milliliters of alcohol are in 167 mL of an 85.0% (v/v) alcohol solution?
252 mL
228 mL
145 mL
142 mL
Which of the following is NOT a colligative property of a solution?
boiling point elevation
supersaturation
vapor pressure lowering
freezing point depression
Colligative properties depend upon the ____.
nature of the solute
nature of the solvent
number of solute particles in a solution
freezing point of a solute
The molality of a solution containing 8.1 moles of solute in 4847 g of solvent is ____.
39 m
1.7 m
0.17 m
598 m
Which of the following is an expression of molality?
10 mol solute/ 1 kg of solvent
10 mol solute/ 1 L of solution
10 mol solute/ 1 L of solvent
10 mol solute/ 1 kg of solution
What is the mole fraction of ethanol in a solution of 3.00 moles of ethanol and 5.00 moles of water?
0.375
0.6
1.67
15
What is the molality of a solution containing 8.0 grams of solute in 0.50 kg of solvent? (molar mass of solute = 24 g)
0.67m
4m
1.67m
0.17m
What is the number of kilograms of solvent in a 0.70 molal solution containing 5.0 grams of solute? (molar mass of solute = 30 g)
0.24 kg
2.4 kg
0.11 kg
1.1 kg
To which of the following variables is change in boiling point directly proportional?
molarity of solution
molality of solution
percent by volume of solution
percent (mass/mass) of solution
What is the freezing point of a solution of 0.5 mol of LiBr in 500 mL of water?
–1.86C
–3.72C
–5.58C
–7.44C
What is the boiling point of a solution of 0.1 mole of glucose in 200 mL of water?
100.06⁰C
100.13⁰C
100.26⁰C
100.5⁰C
Which would NOT increase the rate at which a sugar cube dissolves?
Reducing the amount of solvent
Crushing the sugar cube
Stirring the solution
Heating the solvent
Three 10 g samples of sugar are represented below.
Sample A dissolves in water more slowly than sample B.
Sample B dissolves more slowly than sample C.
Which of the following best explains why sample A dissolves more slowly than the other two?
It has the most volume.
It has the smallest surface area.
It has the largest number of sugar molecules.
It has the fewest bonds between sugar modules.
A solution that is able to dissolve additional solute is best described as
supersaturated.
concentrated.
saturated
unsaturated.
Which of the following is not a colligative property?
molality
vapor-pressure lowering
boiling-point elevation
freezing-point depression
How do we make a dilution?
Add more solute
Remove solute
Remove solvent
Add more solvent
As we dilute a solution.....
The volume increases and the molarity (M) increases
The volume increases and the molarity (M) decreases
The volume decreases and the molarity (M) increases
The volume decreases and the molarity (M) decreases
What would the molarity of a solution be if you took 10 mL of a 13M stock solution and made a 300 mL solution?
390M
230M
0.43M
0.26M
