Question 1

A stockroom attendant has a 15.0%(w/v) solution of KOH. What volume of this solution should she use if she needs to prepare 20.0 mL of a 10.0%(w/v) solution?

Accepted Answer

A)  6.67 mL 
B)  7.50 mL 
C)  13.3 mL 
D)  15.0 mL 
A)  6.67 mL 
B)  7.50 mL 
C)  13.3 mL 
D)  15.0 mL

Question 2

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

Accepted Answer

A)  8.9 g 
B)  11 g 
C)  23 g 
D)  75 g 
A)  8.9 g 
B)  11 g 
C)  23 g 
D)  75 g

Question 3

400 g of salt solution is prepared by dissolving 30 g of salt in water. What is the %(w/w) of this solution?

Accepted Answer

A)  0.075% 
B)  7.5% 
C)  0.069% 
D)  6.9% 
A)  0.075% 
B)  7.5% 
C)  0.069% 
D)  6.9%

Question 4

A solution is prepared by dissolving 4.40 g of KSCN in enough water to make 340.0 mL of solution. What is the concentration of the solution?

Accepted Answer

A)  0.0440 M 
B)  0.0543 M 
C)  0.119 M 
D)  0.133 M 
A)  0.0440 M 
B)  0.0543 M 
C)  0.119 M 
D)  0.133 M

Question 5

A solution is prepared by dissolving 7.7 g of lithium iodide, LiI, in enough water to make 400.0 mL of solution. What is the %(w/v) of LiI?

Accepted Answer

A)  0.96% 
B)  1.9% 
C)  3.9% 
D)  7.7% 
A)  0.96% 
B)  1.9% 
C)  3.9% 
D)  7.7%

Question 6

Which of the following is true of electrolytes?

Accepted Answer

A)  All electrolytes dissolve only in water and no other polar liquid. 
B)  All electrolytes contain cations and anions. 
C)  All electrolytes dissolve only in water and no other polar liquid and contain cations and anions. 
D)  None of these are true. 
A)  All electrolytes dissolve only in water and no other polar liquid. 
B)  All electrolytes contain cations and anions. 
C)  All electrolytes dissolve only in water and no other polar liquid and contain cations and anions. 
D)  None of these are true.

Question 7

To which of the following is the term "water of hydration" applied?

Accepted Answer

A)  the water molecules required to dissolve a solid 
B)  the water molecules associated with ions in solution 
C)  the water molecules present in the crystals of a solid 
D)  none of these 
A)  the water molecules required to dissolve a solid 
B)  the water molecules associated with ions in solution 
C)  the water molecules present in the crystals of a solid 
D)  none of these

Question 8

The following photograph shows the laboratory apparatus required for preparing 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 9

A glycine solution is 2.50%(w/w). How much of glycine is there in a sample that has a mass of 250.0 g?

Accepted Answer

A)  1.25 g 
B)  5.00 g 
C)  6.25 g 
D)  12.5 g 
A)  1.25 g 
B)  5.00 g 
C)  6.25 g 
D)  12.5 g

Question 10

Which of the following solutions has the highest osmolarity?

Accepted Answer

A)  0.20 M NaCl has the highest osmolarity. 
B)  0.15 M BaCl2 has the highest osmolarity. 
C)  0.10 M AlCl3 has the highest osmolarity. 
D)  All of these have the same osmolarity. 
A)  0.20 M NaCl has the highest osmolarity. 
B)  0.15 M BaCl2 has the highest osmolarity. 
C)  0.10 M AlCl3 has the highest osmolarity. 
D)  All of these have the same osmolarity.

Question 11

A solution 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, will cause the solution to have the highest osmolarity. 
B)  Glucose, C6H12O6, will cause the solution to have the highest osmolarity. 
C)  Sucrose, C12H22O11, will cause the solution to have the highest osmolarity. 
D)  All of these will cause the solution to have the same osmolarity. 
A)  Ribose, C5H10O5, will cause the solution to have the highest osmolarity. 
B)  Glucose, C6H12O6, will cause the solution to have the highest osmolarity. 
C)  Sucrose, C12H22O11, will cause the solution to have the highest osmolarity. 
D)  All of these will cause the solution to have the same osmolarity.

Question 12

Which of the following is true of the formula weights of a substance that exists in both anhydrous and hydrated forms?

Accepted Answer

A)  They have the same formula weight. 
B)  The hydrated form always has a lower formula weight. 
C)  The hydrated form always has a higher formula weight. 
D)  We cannot make any general statement about the formula weights of the two forms. 
A)  They have the same formula weight. 
B)  The hydrated form always has a lower formula weight. 
C)  The hydrated form always has a higher formula weight. 
D)  We cannot make any general statement about the formula weights of the two forms.

Question 13

Which of the following is true of colloidal particles?

Accepted Answer

A)  They are smaller than 1 nm. 
B)  They scatter light. 
C)  They are smaller than 1 nm and they scatter light 
D)  None of these are true 
A)  They are smaller than 1 nm. 
B)  They scatter light. 
C)  They are smaller than 1 nm and they scatter light 
D)  None of these are true

Question 14

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

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 15

Which of the following laws describes the relationship between pressure and the solubility of gases in liquids?

Accepted Answer

A)  Avogadro's law 
B)  Boyle's law 
C)  Dalton's law 
D)  Henry's law 
A)  Avogadro's law 
B)  Boyle's law 
C)  Dalton's law 
D)  Henry's law

Question 16

Which of the following is true of electrolytes?

Accepted Answer

A)  All electrolytes have mobile ions. 
B)  All electrolytes contain equal numbers of cations and anions. 
C)  All electrolytes have mobile ions and contain numbers of cations and anions. 
D)  None of these are true. 
A)  All electrolytes have mobile ions. 
B)  All electrolytes contain equal numbers of cations and anions. 
C)  All electrolytes have mobile ions and contain numbers of cations and anions. 
D)  None of these are true.

Question 17

What happens when methanol, CH3OH, 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 these are correct as it 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 these are correct as it does not dissolve in water.

Question 18

A solution is prepared by dissolving 104.1 grams of barium chloride, BaCl2 in 1000.0 grams of water. What is the freezing point of the solution? (The freezing point depression constant for water is 1.86°C/mole solute in 1000 g 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 19

Which of the following is a colligative property?

Accepted Answer

A)  molarity 
B)  percent concentration 
C)  parts per million 
D)  osmotic pressure 
A)  molarity 
B)  percent concentration 
C)  parts per million 
D)  osmotic pressure

Question 20

A bottle of vodka is labeled as 60 proof. What is its alcohol content in terms of (v/v)%?

Accepted Answer

A)  7.5% 
B)  15% 
C)  30.0% 
D)  60.0% 
A)  7.5% 
B)  15% 
C)  30.0% 
D)  60.0%

Exam 6: Solutions and Colloids

A stockroom attendant has a 15.0%(w/v) solution of KOH. What volume of this solution should she use if she needs to prepare 20.0 mL of a 10.0%(w/v) solution?

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

400 g of salt solution is prepared by dissolving 30 g of salt in water. What is the %(w/w) of this solution?

A solution is prepared by dissolving 4.40 g of KSCN in enough water to make 340.0 mL of solution. What is the concentration of the solution?

A solution is prepared by dissolving 7.7 g of lithium iodide, LiI, in enough water to make 400.0 mL of solution. What is the %(w/v) of LiI?

Which of the following is true of electrolytes?

To which of the following is the term "water of hydration" applied?

The following photograph shows the laboratory apparatus required for preparing 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?

A glycine solution is 2.50%(w/w). How much of glycine is there in a sample that has a mass of 250.0 g?

Which of the following solutions has the highest osmolarity?

A solution 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?

Which of the following is true of the formula weights of a substance that exists in both anhydrous and hydrated forms?

Which of the following is true of colloidal particles?

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

Which of the following laws describes the relationship between pressure and the solubility of gases in liquids?

Which of the following is true of electrolytes?

What happens when methanol, CH3OH, dissolves in water?

A solution is prepared by dissolving 104.1 grams of barium chloride, BaCl2 in 1000.0 grams of water. What is the freezing point of the solution? (The freezing point depression constant for water is 1.86°C/mole solute in 1000 g of water.)

Which of the following is a colligative property?

A bottle of vodka is labeled as 60 proof. What is its alcohol content in terms of (v/v)%?

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What happens when methanol, CH₃OH, dissolves in water?

A solution is prepared by dissolving 104.1 grams of barium chloride, BaCl₂ in 1000.0 grams of water. What is the freezing point of the solution? (The freezing point depression constant for water is 1.86°C/mole solute in 1000 g of water.)