Question 1

Isotonic saline is 0.89% NaCl (w/v). Suppose you wanted to make 1.0 L of isotonic solution of NH4Cl. What mass of NH4Cl would you need?

Accepted Answer

A)  1.6 g 
B)  8.1 g 
C)  8.9 g 
D)  54 g 
A)  1.6 g 
B)  8.1 g 
C)  8.9 g 
D)  54 g

Question 2

What is the %(w/w) of a salt solution prepared by dissolving 7.5 g of salt in 242.5 g of water?

Accepted Answer

A)  0.030% 
B)  0.30% 
C)  0.75% 
D)  3.0% 
A)  0.030% 
B)  0.30% 
C)  0.75% 
D)  3.0%

Question 3

The following shows the beginning of the laboratory preparation of an aqueous solution of the hypothetical compound AB (150.5 g/mol).  
-What will be the molarity of the solution when the preparation is complete?

Accepted Answer

A)  51.0 M 
B)  0.00510 M 
C)  0.339 M 
D)  0.00339 M 
A)  51.0 M 
B)  0.00510 M 
C)  0.339 M 
D)  0.00339 M

Question 4

What is the mass of salt in a 400-gram sample of salt water which is 1.50% (w/w)?

Accepted Answer

A)  1.50 grams 
B)  2.67 grams 
C)  3.00 grams 
D)  6.00 grams 
A)  1.50 grams 
B)  2.67 grams 
C)  3.00 grams 
D)  6.00 grams

Question 5

A solution is prepared by dissolving 215 grams of methanol, CH3OH, in 1000. grams of water. What is the boiling point of this solution? [The boiling point elevation constant for water is 0.52°C/mole solute in 1000 g of water]

Accepted Answer

A)  93.0°C 
B)  96.5°C 
C)  103.5°C 
D)  107.0°C 
A)  93.0°C 
B)  96.5°C 
C)  103.5°C 
D)  107.0°C

Question 6

Consider the following image of a separatory funnel.  
-Which of the following correctly describes the contents of the funnel?

Accepted Answer

A)  Both liquids are nonpolar. 
B)  Both liquids are polar. 
C)  One liquid is polar and the other nonpolar. 
D)  Impossible to determine polarity from the data given. 
A)  Both liquids are nonpolar. 
B)  Both liquids are polar. 
C)  One liquid is polar and the other nonpolar. 
D)  Impossible to determine polarity from the data given.

Question 7

Which of the following is true regarding the solubility of liquids and solids?

Accepted Answer

A)  Solubility always decreases as temperature increases. 
B)  Solubility always increases as temperature increases. 
C)  Solubility usually decreases as temperature increases. 
D)  Solubility usually increases as temperature increases. 
A)  Solubility always decreases as temperature increases. 
B)  Solubility always increases as temperature increases. 
C)  Solubility usually decreases as temperature increases. 
D)  Solubility usually increases as temperature increases.

Question 8

Which of the following relates the name of an electrode to its sign?

Accepted Answer

A)  The anode is the negative electrode. 
B)  The cathode is the positive electrode. 
C)  both a and b 
D)  neither a nor b 
A)  The anode is the negative electrode. 
B)  The cathode is the positive electrode. 
C)  both a and b 
D)  neither a nor b

Question 9

Which of the following is associated with cells in an isotonic solution?

Accepted Answer

A)  crenation 
B)  hemolysis 
C)  reverse osmosis 
D)  none of these 
A)  crenation 
B)  hemolysis 
C)  reverse osmosis 
D)  none of these

Question 10

Which of the following can pass through a dialysis membrane?

Accepted Answer

A)  colloidal particles 
B)  macromolecules 
C)  small molecules 
D)  none of them 
A)  colloidal particles 
B)  macromolecules 
C)  small molecules 
D)  none of them

Question 11

In a solution of a solid in a liquid, the solid is called which of the following?

Accepted Answer

A)  concentrate 
B)  dissolvate 
C)  solute 
D)  solvent 
A)  concentrate 
B)  dissolvate 
C)  solute 
D)  solvent

Question 12

Which of the following is true of glucose, C6H12O6, when it dissolves in water?

Accepted Answer

A)  It dissociates into ions. 
B)  It forms covalent bonds with water. 
C)  It forms hydrogen bonds with water. 
D)  None of the above, glucose does not dissolve in water. 
A)  It dissociates into ions. 
B)  It forms covalent bonds with water. 
C)  It forms hydrogen bonds with water. 
D)  None of the above, glucose does not dissolve in water.

Question 13

Which of the following terms can be used to quantitatively describe the concentration of a solution?

Accepted Answer

A)  concentrated 
B)  dilute 
C)  molarity 
D)  all of these 
A)  concentrated 
B)  dilute 
C)  molarity 
D)  all of these

Question 14

Which of the following is true of all strong electrolytes?

Accepted Answer

A)  They are all ionic compounds. 
B)  They all dissociate completely. 
C)  both a and b 
D)  neither a nor b 
A)  They are all ionic compounds. 
B)  They all dissociate completely. 
C)  both a and b 
D)  neither a nor b

Question 15

A solution is prepared by dissolving 215 grams of methanol, CH3OH, in 1000. grams of water. What is the freezing point of this solution? [The freezing point depression constant for water is 1.86°C/mole solute in 1000g of water]

Accepted Answer

A)  -6.72°C 
B)  -12.5°C 
C)  -25.0°C 
D)  -40.3°C 
A)  -6.72°C 
B)  -12.5°C 
C)  -25.0°C 
D)  -40.3°C

Question 16

A solution is prepared by dissolving 3.50 grams of NH4Cl in enough water to make 250. mL of solution. What is the concentration of this solution?

Accepted Answer

A)  0.0327 M 
B)  0.0654 M 
C)  0.131 M 
D)  0.262 M 
A)  0.0327 M 
B)  0.0654 M 
C)  0.131 M 
D)  0.262 M

Question 17

What is the maximum diameter of solute particles in a true solution?

Accepted Answer

A)  1 pm 
B)  1 nm 
C)  1 ìm 
D)  1 mm 
A)  1 pm 
B)  1 nm 
C)  1 ìm 
D)  1 mm

Question 18

Given three solutions, each of which contains 1.0 g of solute dissolved in 100 mL of water, which of the following solutes will cause the solution to have the highest osmolarity?

Accepted Answer

A)  ribose, C5H10O5 
B)  glucose, C6H12O6 
C)  sucrose, C12H22O11 
D)  None, they all have the same osmolarity. 
A)  ribose, C5H10O5 
B)  glucose, C6H12O6 
C)  sucrose, C12H22O11 
D)  None, they all have the same osmolarity.

Question 19

A solution is prepared by dissolving 104.1 grams of barium chloride, BaCl2 in 1000. grams of water? What is the freezing point of this solution? [The freezing point depression constant for water is 1.86°C/mole solute in 1000g of water]

Accepted Answer

A)  -1.86°C 
B)  -2.79°C 
C)  -3.72°C 
D)  -5.58°C 
A)  -1.86°C 
B)  -2.79°C 
C)  -3.72°C 
D)  -5.58°C

Question 20

How many moles of solute are contained in 500. mL of 0.50 M KCl?

Accepted Answer

A)  0.25 
B)  0.50 
C)  1.0 
D)  2.0 
A)  0.25 
B)  0.50 
C)  1.0 
D)  2.0

Exam 6: Solutions and Colloids

Isotonic saline is 0.89% NaCl (w/v). Suppose you wanted to make 1.0 L of isotonic solution of NH4Cl. What mass of NH4Cl would you need?

What is the %(w/w) of a salt solution prepared by dissolving 7.5 g of salt in 242.5 g of water?

The following shows the beginning of the laboratory preparation of an aqueous solution of the hypothetical compound AB (150.5 g/mol). -What will be the molarity of the solution when the preparation is complete?

What is the mass of salt in a 400-gram sample of salt water which is 1.50% (w/w)?

A solution is prepared by dissolving 215 grams of methanol, CH3OH, in 1000. grams of water. What is the boiling point of this solution? [The boiling point elevation constant for water is 0.52°C/mole solute in 1000 g of water]

Consider the following image of a separatory funnel. -Which of the following correctly describes the contents of the funnel?

Which of the following is true regarding the solubility of liquids and solids?

Which of the following relates the name of an electrode to its sign?

Which of the following is associated with cells in an isotonic solution?

Which of the following can pass through a dialysis membrane?

In a solution of a solid in a liquid, the solid is called which of the following?

Which of the following is true of glucose, C6H12O6, when it dissolves in water?

Which of the following terms can be used to quantitatively describe the concentration of a solution?

Which of the following is true of all strong electrolytes?

A solution is prepared by dissolving 215 grams of methanol, CH3OH, in 1000. grams of water. What is the freezing point of this solution? [The freezing point depression constant for water is 1.86°C/mole solute in 1000g of water]

A solution is prepared by dissolving 3.50 grams of NH4Cl in enough water to make 250. mL of solution. What is the concentration of this solution?

What is the maximum diameter of solute particles in a true solution?

Given three solutions, each of which contains 1.0 g of solute dissolved in 100 mL of water, which of the following solutes will cause the solution to have the highest osmolarity?

A solution is prepared by dissolving 104.1 grams of barium chloride, BaCl2 in 1000. grams of water? What is the freezing point of this solution? [The freezing point depression constant for water is 1.86°C/mole solute in 1000g of water]

How many moles of solute are contained in 500. mL of 0.50 M KCl?

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Isotonic saline is 0.89% NaCl (w/v). Suppose you wanted to make 1.0 L of isotonic solution of NH₄Cl. What mass of NH₄Cl would you need?

A solution is prepared by dissolving 215 grams of methanol, CH₃OH, in 1000. grams of water. What is the boiling point of this solution? [The boiling point elevation constant for water is 0.52°C/mole solute in 1000 g of water]

Which of the following is true of glucose, C₆H₁₂O₆, when it dissolves in water?

A solution is prepared by dissolving 215 grams of methanol, CH₃OH, in 1000. grams of water. What is the freezing point of this solution? [The freezing point depression constant for water is 1.86°C/mole solute in 1000g of water]

A solution is prepared by dissolving 3.50 grams of NH₄Cl in enough water to make 250. mL of solution. What is the concentration of this solution?

A solution is prepared by dissolving 104.1 grams of barium chloride, BaCl₂ in 1000. grams of water? What is the freezing point of this solution? [The freezing point depression constant for water is 1.86°C/mole solute in 1000g of water]