Question 1

How many grams of vitamin B12 are present in a 100.0 mL blood serum sample with a vitamin B12 concentration of 148 ng/L?

Accepted Answer

A)  1.48 x 10-9 g 
B)  1.48 x 10-8 g 
C)  1.48 x 10-5 g 
D)  1.48 g 
A)  1.48 x 10-9 g 
B)  1.48 x 10-8 g 
C)  1.48 x 10-5 g 
D)  1.48 g B

Question 2

What volume of 2.00 % NaCl must be diluted to make 10.00 mL of 0.90% NaCl, also known as normal saline solution?

Accepted Answer

A)  4.5 mL 
B)  0.18 mL 
C)  9.0 mL 
D)  22.2 mL 
A)  4.5 mL 
B)  0.18 mL 
C)  9.0 mL 
D)  22.2 mL A

Question 3

A gas sample occupies 10.28 L at 8.34 atm. Its volume at 6.98 atm (assuming constant temperature conditions) is ___.

Accepted Answer

A)  12.3 L 
B)  5.66 L 
C)  8.60 L 
D)  15.6 L 
A)  12.3 L 
B)  5.66 L 
C)  8.60 L 
D)  15.6 L A

Question 4

A bottle of 6.000 M NaOH is on the lab bench. You are instructed to use 75.00 mL of 0.5000 M NaOH. How much 6.000 M NaOH do you have to dilute to 75.00 mL to meet the requirement?

Accepted Answer

A)  The solution cannot be produced from 6.000 M NaOH. 
B)  37.50 mL 
C)  9.000 mL 
D)  6.250 mL 
A)  The solution cannot be produced from 6.000 M NaOH. 
B)  37.50 mL 
C)  9.000 mL 
D)  6.250 mL

Question 5

Standard temperature and pressure corresponds to

Accepted Answer

A)  temperature of 0C and pressure of 1 psi. 
B)  temperature of 25C and pressure of 1 atm. 
C)  temperature of 0C and pressure of 2 psi. 
D)  temperature of 0C and pressure of 1 atm. 
A)  temperature of 0C and pressure of 1 psi. 
B)  temperature of 25C and pressure of 1 atm. 
C)  temperature of 0C and pressure of 2 psi. 
D)  temperature of 0C and pressure of 1 atm.

Question 6

A water sample taken from the ocean is 36 ppt salt content. What is the mass of salt present in a liter of this ocean water?

Accepted Answer

A)  0.028 g 
B)  27.8 g 
C)  36 g 
D)  36,000 g 
A)  0.028 g 
B)  27.8 g 
C)  36 g 
D)  36,000 g

Question 7

According to Gay-Lussac's law, when the Kelvin temperature of a gas doubles (at constant volume), its pressure will ___

Accepted Answer

A)  double 
B)  reduced to 1/2 
C)  quadruple 
D)  remain the same 
A)  double 
B)  reduced to 1/2 
C)  quadruple 
D)  remain the same

Question 8

When a person inhales air,

Accepted Answer

A)  lung volume decreases and lung pressure increases. 
B)  lung volume increases and lung pressure decreases. 
C)  lung volume decreases and lung pressure decreases. 
D)  lung volume increases and lung pressure increases. 
A)  lung volume decreases and lung pressure increases. 
B)  lung volume increases and lung pressure decreases. 
C)  lung volume decreases and lung pressure decreases. 
D)  lung volume increases and lung pressure increases.

Question 9

Ethyl alcohol (CH3CH2OH) is completely soluble in water. It is made of both polar and non-polar groups. Ethyl alcohol is best classified as a(n) ___ substance.

Accepted Answer

A)  hydrophilic 
B)  hydrophobic 
C)  lipophilic 
D)  amphipathic 
A)  hydrophilic 
B)  hydrophobic 
C)  lipophilic 
D)  amphipathic

Question 10

Sodium fluoride is added to drinking water. A 25-L sample of city water contains 0.018 g NaF. Express this concentration in molarity.

Accepted Answer

A)  0.000017 M 
B)  0.00072 M 
C)  0.018 M 
D)  18 M 
A)  0.000017 M 
B)  0.00072 M 
C)  0.018 M 
D)  18 M

Question 11

Which of the following is a general statement concerning the solubility of organic compounds?

Accepted Answer

A)  The larger molecules dissolve best in a solvent with a low molecular weight. 
B)  The polar organic compounds dissolve best in polar solvents. 
C)  The nonpolar compounds can dissolve well in polar solvents if the molecules are close to the same size. 
D)  Those compounds that have only covalent bonds dissolve well in water. 
A)  The larger molecules dissolve best in a solvent with a low molecular weight. 
B)  The polar organic compounds dissolve best in polar solvents. 
C)  The nonpolar compounds can dissolve well in polar solvents if the molecules are close to the same size. 
D)  Those compounds that have only covalent bonds dissolve well in water.

Question 12

A sample of nitrogen gas exerts a pressure of 9.80 atm at 32 C. What would its temperature be (in C) when its pressure is increased to 11.2 atm?

Accepted Answer

A)  76 C 
B)  - 6.2 C 
C)  49 C 
D)  3.5 x 102 C 
A)  76 C 
B)  - 6.2 C 
C)  49 C 
D)  3.5 x 102 C

Question 13

The "bends" is a condition in which nitrogen gas is released from solution in the blood vessels of a scuba diver. It is caused by a diver rising too quickly to the surface of the water. This condition is explained by Henry's Law. The solubility of a gas in solution ___ as the pressure ___.

Accepted Answer

A)  decreases/decreases 
B)  increases/decreases 
C)  decreases/increases 
A)  decreases/decreases 
B)  increases/decreases 
C)  decreases/increases

Question 14

Unlike acetic acid (CH2COOH), which is completely soluble in water, 1-hexanoic acid (CH2CH2CH2CH2CH2COOH) is only slightly soluble in water because

Accepted Answer

A)  only acetic acid forms hydrogen bonds. 
B)  acetic acid has a higher boiling point than 1-hexanoic acid. 
C)  the increased length of carbon chain in 1-hexanoic acid increases its hydrophobic character. 
D)  acetic acid does not ionize in water. 
A)  only acetic acid forms hydrogen bonds. 
B)  acetic acid has a higher boiling point than 1-hexanoic acid. 
C)  the increased length of carbon chain in 1-hexanoic acid increases its hydrophobic character. 
D)  acetic acid does not ionize in water.

Question 15

Which of the following ionic substances is insoluble in water?

Accepted Answer

A)  KNO3 
B)  BaSO4 
C)  Na3PO4 
D)  NH4Br 
A)  KNO3 
B)  BaSO4 
C)  Na3PO4 
D)  NH4Br

Question 16

For solute particles to be soluble in liquid solvents

Accepted Answer

A)  they must be about the same size as the solvent molecules and be able to interact with the solvent molecules through noncovalent interactions. 
B)  the solvent must be nonpolar. 
C)  they must be polar. 
D)  they must be of smaller size than solvent molecules and be able to interact with solvent molecules through covalent interactions. 
A)  they must be about the same size as the solvent molecules and be able to interact with the solvent molecules through noncovalent interactions. 
B)  the solvent must be nonpolar. 
C)  they must be polar. 
D)  they must be of smaller size than solvent molecules and be able to interact with solvent molecules through covalent interactions.

Question 17

The calculations of Boyle's, Charles', and Gay-Lussac's laws assume that the gases involved behave as ideal gases.

Accepted Answer

A) True 
 B)False

Question 18

Arrange the terms solution, suspension, and colloid in order of increasing size of the dispersed particles.

Accepted Answer

A)  solution < suspension < colloid 
B)  solution < colloid < suspension 
C)  suspension < solution < colloid 
D)  colloid < solution < suspension 
A)  solution < suspension < colloid 
B)  solution < colloid < suspension 
C)  suspension < solution < colloid 
D)  colloid < solution < suspension

Question 19

Soaps are amphipathic compounds. Which statement best describes them?

Accepted Answer

A)  Soaps cannot be attracted to either polar or nonpolar compounds. 
B)  Soaps dissolve best in polar solvents, which is why they can remove dirt. 
C)  Soaps have a hydrophobic end, which will attract nonpolar substances, such as soil on clothing. 
D)  The soaps that are the most effective in cleaning contain the calcium ion. 
A)  Soaps cannot be attracted to either polar or nonpolar compounds. 
B)  Soaps dissolve best in polar solvents, which is why they can remove dirt. 
C)  Soaps have a hydrophobic end, which will attract nonpolar substances, such as soil on clothing. 
D)  The soaps that are the most effective in cleaning contain the calcium ion.

Question 20

Barometers measure atmospheric pressure and temperature.

Accepted Answer

A) True 
 B)False

How many grams of vitamin B₁₂ are present in a 100.0 mL blood serum sample with a vitamin B12 concentration of 148 ng/L?

What volume of 2.00 % NaCl must be diluted to make 10.00 mL of 0.90% NaCl, also known as normal saline solution?

A gas sample occupies 10.28 L at 8.34 atm. Its volume at 6.98 atm (assuming constant temperature conditions) is ___.

A bottle of 6.000 M NaOH is on the lab bench. You are instructed to use 75.00 mL of 0.5000 M NaOH. How much 6.000 M NaOH do you have to dilute to 75.00 mL to meet the requirement?

Standard temperature and pressure corresponds to

A water sample taken from the ocean is 36 ppt salt content. What is the mass of salt present in a liter of this ocean water?

According to Gay-Lussac's law, when the Kelvin temperature of a gas doubles (at constant volume), its pressure will ___

When a person inhales air,

Ethyl alcohol (CH₃CH₂OH) is completely soluble in water. It is made of both polar and non-polar groups. Ethyl alcohol is best classified as a(n) ___ substance.

Sodium fluoride is added to drinking water. A 25-L sample of city water contains 0.018 g NaF. Express this concentration in molarity.

Which of the following is a general statement concerning the solubility of organic compounds?

A sample of nitrogen gas exerts a pressure of 9.80 atm at 32 C. What would its temperature be (in C) when its pressure is increased to 11.2 atm?

The "bends" is a condition in which nitrogen gas is released from solution in the blood vessels of a scuba diver. It is caused by a diver rising too quickly to the surface of the water. This condition is explained by Henry's Law. The solubility of a gas in solution _ as the pressure _.

Unlike acetic acid (CH₂COOH), which is completely soluble in water, 1-hexanoic acid (CH₂CH₂CH₂CH₂CH₂COOH) is only slightly soluble in water because

Which of the following ionic substances is insoluble in water?

For solute particles to be soluble in liquid solvents

The calculations of Boyle's, Charles', and Gay-Lussac's laws assume that the gases involved behave as ideal gases.

Arrange the terms solution, suspension, and colloid in order of increasing size of the dispersed particles.

Soaps are amphipathic compounds. Which statement best describes them?

Barometers measure atmospheric pressure and temperature.

Science and Measurements

Atoms and Elements

Compounds

An Introduction to Organic Compounds

Reactions

Acids, Bases, and Equilibrium

Organic Reactions Hydrocarbons, Carboxlic Acids, Amines, and Related Compounds

Organic Reactions 2-Alcohols, Ethers, Aldehydes, and Ketones

Carbohydrates

Lipids and Membranes

Peptides, Proteins, and Enzymes

Nucleic Acids

Metabolism

Filters

Exam 6: Gases, Solutions, Colloids, and Suspensions

How many grams of vitamin B12 are present in a 100.0 mL blood serum sample with a vitamin B12 concentration of 148 ng/L?

What volume of 2.00 % NaCl must be diluted to make 10.00 mL of 0.90% NaCl, also known as normal saline solution?

A gas sample occupies 10.28 L at 8.34 atm. Its volume at 6.98 atm (assuming constant temperature conditions) is ___.

A bottle of 6.000 M NaOH is on the lab bench. You are instructed to use 75.00 mL of 0.5000 M NaOH. How much 6.000 M NaOH do you have to dilute to 75.00 mL to meet the requirement?

Standard temperature and pressure corresponds to

A water sample taken from the ocean is 36 ppt salt content. What is the mass of salt present in a liter of this ocean water?

According to Gay-Lussac's law, when the Kelvin temperature of a gas doubles (at constant volume), its pressure will ___

When a person inhales air,

Ethyl alcohol (CH3CH2OH) is completely soluble in water. It is made of both polar and non-polar groups. Ethyl alcohol is best classified as a(n) ___ substance.

Sodium fluoride is added to drinking water. A 25-L sample of city water contains 0.018 g NaF. Express this concentration in molarity.

Which of the following is a general statement concerning the solubility of organic compounds?

A sample of nitrogen gas exerts a pressure of 9.80 atm at 32 C. What would its temperature be (in C) when its pressure is increased to 11.2 atm?

The "bends" is a condition in which nitrogen gas is released from solution in the blood vessels of a scuba diver. It is caused by a diver rising too quickly to the surface of the water. This condition is explained by Henry's Law. The solubility of a gas in solution ___ as the pressure ___.

Unlike acetic acid (CH2COOH), which is completely soluble in water, 1-hexanoic acid (CH2CH2CH2CH2CH2COOH) is only slightly soluble in water because

Which of the following ionic substances is insoluble in water?

For solute particles to be soluble in liquid solvents

The calculations of Boyle's, Charles', and Gay-Lussac's laws assume that the gases involved behave as ideal gases.

Arrange the terms solution, suspension, and colloid in order of increasing size of the dispersed particles.

Soaps are amphipathic compounds. Which statement best describes them?

Barometers measure atmospheric pressure and temperature.

Science and Measurements

Atoms and Elements

Compounds

An Introduction to Organic Compounds

Reactions

Acids, Bases, and Equilibrium

Organic Reactions Hydrocarbons, Carboxlic Acids, Amines, and Related Compounds

Organic Reactions 2-Alcohols, Ethers, Aldehydes, and Ketones

Carbohydrates

Lipids and Membranes

Peptides, Proteins, and Enzymes

Nucleic Acids

Metabolism

Filters

How many grams of vitamin B₁₂ are present in a 100.0 mL blood serum sample with a vitamin B12 concentration of 148 ng/L?

Ethyl alcohol (CH₃CH₂OH) is completely soluble in water. It is made of both polar and non-polar groups. Ethyl alcohol is best classified as a(n) ___ substance.

The "bends" is a condition in which nitrogen gas is released from solution in the blood vessels of a scuba diver. It is caused by a diver rising too quickly to the surface of the water. This condition is explained by Henry's Law. The solubility of a gas in solution _ as the pressure _.

Unlike acetic acid (CH₂COOH), which is completely soluble in water, 1-hexanoic acid (CH₂CH₂CH₂CH₂CH₂COOH) is only slightly soluble in water because