Lakeland Solutions Review

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Molarity is defined as the

A) moles of solute per kilogram of solvent

B) moles of solute per liter of solution

C) mass of a solution D) volume of a solvent

Question 1

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• Review the definition of Molarity

Correct!

• Molarity is the moles of solute per liter of solution

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Under which conditions of temperature andpressure is a gas most soluble in water?

A) high temperature and low pressure

B) low temperature and low pressure

C) high temperature and high pressure

D) low temperature and high pressure

Question 2

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• Think about the best conditions to keep carbonation in pop

Correct!

• The best conditions are high pressure and low temperature. These produce a situation where the gas will be forced into the liquid

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What is the molarity of a solution of NaOH if2 liters of the solution contains 4 moles of NaOH?

A) 0.5 M B) 2.0 M

C) 8.0 M D) 80 M

Question 3

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• Molarity is moles of solute per liter of solution

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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A substance that conducts an electrical currentwhen dissolved in water is called

A) A catalyst B) A non-electrolyte

C) A metalloid D) An electrolyte

Question 4

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• Review your solutions vocabulary

Correct!

• An electrolyte is a solution that can conduct electricity

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Compared to a 2.0 M aqueous solution of NaClat 1 atmosphere, a 3.0 M aqueous solution ofNaCl at 1 atmosphere has aA) Lower boiling point and higher

freezing pointB) Lower boiling point and lower freezing point

C) Higher boiling point and lower freezing point

D) Higher boiling point and higher freezing point

Question 5

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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.

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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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

Question 6

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• Review the definition of molarity

Correct!

• 3.0 M means that there are 3.0 moles per liter of solution

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What is the total number of grams of HI in0.500 liter of 1.00 M HI?

A) 1.00 g B) 64.0 g

C) 0.5 g D) 128.0 g

Question 7

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• Use the molarity equation to solve for number of moles and then convert to grams

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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Which 1-molal aqueous solution has the lowestfreezing point?

Question 8

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• The lowest freezing point will have the lowest vapor pressure. The more ions present, the lower the vapor pressure.

Correct!

• The beaker contains the most ions which will reduce vapor pressure the most.

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What is the molarity of a solution that contains0.50 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

Question 9

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• Remember that Molarity is moles per liter

Correct!

• 0.50 mol/0.50 liters is 1.00 M

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What is the total number of moles of solute in2.0 liters of 3.0 M NaOH?

A) 1.0 mole B) 2.0 mole

C) 3.0 mole D) 6.0 mole

Question 10

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• Molarity equals moles of solute divided by liters of solution.

Correct!

• 3.0 M = x/2.0 L so x = (3.0)(2.0) = 6.0 mole

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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)

Question 11

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• The exponents in the expression tell you how many of each ion are present in the compound

Correct!

• The exponents in the expression mean that there are 2 A and 3 B in the solid.

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As the pressure on a gas confined above a liquidincreases, the solubility of the gas in the liquid

A) increases B) decreases

C) Remains the same D) Not enough information

Question 12

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• Think about what is the best way to keep carbonation in pop.

Correct!

• Increasing pressure increases the solubility of a gas in a liquid

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Which preparation produces a 2.0 M solution ofC6H12O6? [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

Question 13

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• Convert the grams of sugar to moles and divide by the liters in order to determine molarity

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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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.

Question 14

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• The addition of a solute causes a change in vapor pressure resulting in boiling point elevation and freezing point depression

Correct!

• The addition of a solute causes the boiling point to go up and the freezing point to go down.

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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

Question 15

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• %v/v = volume of solute x 100 volume of solution

Correct!

• 70 = x x 100 x = 413.7 mL 591

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