Lakeland Solutions Review
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Question 1
What is the molarity of a solution that contains 40. grams of NaOH in
0.50 liter of solution?
A) 0.25
B) 0.5
C) 1.0
D) 2.0
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• Be sure to convert the 40 g to moles before
plugging into the molarity equation.
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Correct!
• 40 grams of NaOH is equal to 1 mole. 1 mole
divided by 0.5 L is equal to 2.0 M.
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Question 2
Which preparation produces a 2.0 M solution of C6H12O6? [molecular
mass = 180.0]
A) 90.0 g of C6H12O6 dissolved in
500.0 mL of solution
B) 90.0 g of C6H12O6 dissolved in
1000. mL of solution
C) 180.0 g of C6H12O6 dissolved in
500.0 mL of solution
D) 180.0 g of C6H12O6 dissolved in
1000. mL of solution
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• Be sure to convert the grams to moles and the
milliliters to liters.
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Correct!
• 180 g of C6H12O6 is equal to 1 mole. 1 mole
divided by 0.5 L (500 mL) is equal to 2.0 M.
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Question 3
What is the molarity of a solution of NaOH if
2 liters of the solution contains 4 moles of NaOH?
A) 0.5 M
B) 2.0 M
C) 8.0 M
D) 80 M
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• Molarity is moles of solute per liter of solution
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Correct!
• There are 4 moles of solute in 2 liters of
solution. Molarity is moles divided by liters so
4/2 = 2 M
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Question 4
A substance that conducts an electrical current
when dissolved in water is called
A) A catalyst
B) A non-electrolyte
C) A metalloid
D) An electrolyte
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• Review your solutions vocabulary
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Correct!
• An electrolyte is a solution that can conduct
electricity
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Question 5
Compared to a 2.0 M aqueous solution of NaCl
at 1 atmosphere, a 3.0 M aqueous solution of
NaCl at 1 atmosphere has a
A) Lower boiling point and higher B) Lower boiling point and lower
freezing point
freezing point
C) Higher boiling point and lower
freezing point
D) Higher boiling point and higher
freezing point
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• The addition of a solute changes the vapor
pressure of a solution. The more solute
dissolved, the greater the change in colligative
properties.
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Correct!
• The 3.0 M solution has more solute dissolved
than the 2.0 M solution. This means that
there will be a greater boiling point elevation
and freezing point depression
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Question 6
A 3.0 M HCl(aq) solution contains a total of
A) 3.0 grams of HCl per liter of
solution
B) 3.0 grams of HCl per mole of
solution
C) 3.0 moles of HCl per liter of
solution
D) 3.0 moles of HCl per mole of
solution
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• Review the definition of molarity
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Correct!
• 3.0 M means that there are 3.0 moles per liter
of solution
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Question 7
What is the total number of grams of HI in
0.500 liter of 1.00 M HI?
A) 1.00 g
B) 64.0 g
C) 0.5 g
D) 128.0 g
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• Use the molarity equation to solve for number
of moles and then convert to grams
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Correct!
• Molarity = moles/liters so 1.00 M = x/0.50 L. X
= 0.500 mol. Convert 0.500 mol to grams of HI
(mass = 128 g) to get 64 grams.
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Question 8
Which 1-molal aqueous solution has the lowest
freezing point?
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• The lowest freezing point will have the lowest
vapor pressure. The more ions present, the
lower the vapor pressure.
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Correct!
• The beaker contains the most ions which will
reduce vapor pressure the most.
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Question 9
What is the molarity of a solution that contains
0.50 mole of NaOH in 0.50 liter of solution?
A) 1.00 M
B) 0.25 M
C) 2.00 M
D) 0.50 M
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• Remember that Molarity is moles per liter
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Correct!
• 0.50 mol/0.50 liters is 1.00 M
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Question 10
What is the total number of moles of solute in
2.0 liters of 3.0 M NaOH?
A) 1.0 mole
B) 2.0 mole
C) 3.0 mole
D) 6.0 mole
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• Molarity equals moles of solute divided by
liters of solution.
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Correct!
• 3.0 M = x/2.0 L so x = (3.0)(2.0) = 6.0 mole
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Question 11
Given the Ksp expression: Ksp = [A3+]2 [B2–]3
Which reaction is represented by the expression?
A) A2B3(s)  3A3+(aq) + 2B2–(aq)
B) A2B3(s) 2A3+(aq) + 3B2–(aq)
C) A3B2(s) 3A3+(aq) + 2B2–(aq)
D) A3B2(s) 2A3+(aq) + 3B2–(aq)
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• The exponents in the expression tell you how
many of each ion are present in the
compound
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Correct!
• The exponents in the expression mean that
there are 2 A and 3 B in the solid.
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Question 12
As the pressure on a gas confined above a liquid
increases, the solubility of the gas in the liquid
A) increases
B) decreases
C) Remains the same
D) Not enough information
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• Think about what is the best way to keep
carbonation in pop.
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Correct!
• Increasing pressure increases the solubility of
a gas in a liquid
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Question 13
Which preparation produces a 2.0 M solution of
C6H12O6? [molecular mass = 180.0]
A) 90.0 g of C6H12O6 dissolved in
500.0 mL of solution
B) 90.0 g of C6H12O6 dissolved in
1000. mL of solution
C) 180.0 g of C6H12O6 dissolved in
500.0 mL of solution
D) 180.0 g of C6H12O6 dissolved in
1000. mL of solution
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• Convert the grams of sugar to moles and
divide by the liters in order to determine
molarity
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Correct!
• 180 grams of C6H12O6 is equal to 1 mole. 1
mole divided by 0.5 L (500 mL) is 2.0 M.
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Question 14
As a solute is added to a solvent, what happens to the freezing point
and the boiling point of the solution?
A) The freezing point decreases
and the boiling point
decreases.
B) The freezing point increases
and the boiling point increases.
C) The freezing point increases
and the boiling point decreases.
D) The freezing point decreases
and the boiling point increases.
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• The addition of a solute causes a change in
vapor pressure resulting in boiling point
elevation and freezing point depression
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Correct!
• The addition of a solute causes the boiling
point to go up and the freezing point to go
down.
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Question 15
A bottle of rubbing alcohol is labeled 70% v/v. If the bottle contains
591 mL, how much rubbing alcohol is in the bottle?
A) 591 mL
B) 70 mL
C) 413.7 mL
D) 177.3 mL
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• %v/v = volume of solute x 100
volume of solution
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Correct!
• 70 = x
x 100 x = 413.7 mL
591
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