Chemistry Review

Which of the following solutions has the greatest concentration of hydrogen ions [H+]? A. Gastric juice at pH 2 B. Vinegar at pH 3 C. Tomato juice at pH 4 D. Black coffee at pH 5 E. Household bleach at pH 12

A. Gastric juice at pH 2

Hydrophobic substances such as vegetable oil are A. Nonpolar substances that repel water molecules B. Nonpolar substances that have an attraction for water molecules C. Polar substances that repel water molecules D. Polar substances habe an affinity for water E. Charged molecules that hydrogen-bond with water molecules

A. Nonpolar substances that repel water molecules

Which bonds must be broken for water to vaporize? A. Ionic bonds B. Nonpolar covalent bonds C. Polar covalent bonds D. Hydrogen bonds E. Covalent bonds

D. Hydrogen bonds

Why does ice float in water? A. The liquid water molecules have more kinetic energy and thus support the ice. B. The ionic bonds between the molecules in ice prevent the ice from sinking C. Ice always has air bubbles that keep it float D . Hydrogen bonds stabilize and keep the molecules of ice farther apart than the water molecules of liquid water E. The crystalline lattice of ice causes it to be denser than liquid water

D. Hydrogen bonds stabilize and keep the molecules of ice farther apart than the water molecules of liquid water.

Many mammals control their body temperature by sweating. Which behavior of water is most directly responsible for the ability of swear to lower body temperature? A. Water's change in density when it condenses B. Water's ability to dissolve molecules on the air C. The absorption of heat by the formation of hydrogen bonds D. The absorption of heat by hydrogen bonds E. Water's high surface tension

D. The absorption of heat by hydrogen bonds

Which of the following statements is true about buffer solutions? A. They maintain a constant pH when bases are added to them but not when acids are added to them B. They maintain a constant pH when acids are added to them but not when bases are added to them C. They maintain a constant pH of exactly 7 in all living cells and biological fluids D. They maintain a relatively constant pH E. They are found only in living systems and biological fluids

D. They maintain a relatively constant pH

If the pH of a solution is decreased from 9 to 8, it means that the A. Concentration of H+ has decreased 10 times what it was at pH 9 B. Concentration of H+ has increased 10 times what it was at pH 9 C. Concentration of OH- has increased 10 times what it was at pH 9 D. Concentration of OH- has increased 10 times what it was at pH 9 E. B and D are correct

E. Concentration of H+ has increased 10 times what it was at pH 9 and Concentration of OH- decreased 10 times what it was at pH 9.

Which of the following solutions has the greatest concentration of hydroxide ions [OH-]? A. Lemon juice at pH 2 B. Vinegar at pH 3 C. Tomato juice at pH 4 D. Urine at pH 6 E. Seawater at pH 8

E. Seawater at pH 8

The slight negative charge at one end of one water molecule is attracted to the slight positive charge of another water molecule. What is this attraction called? A. A covalent bond B. A hydrogen bond C. An ionic bond D. A hydrophilic bond E. A hydrophobic bond

A. A Covalent Bond

At what temperature is water at its densest? A. 0°C B. 4°C C. 32°C D. 100°C E. 212°C

B. 4°C

Which of the following is possible due to the high surface tension of water? A. Lakes don't freeze solid in winter, despite low temperatures B. A water strider can walk across the surface of a small pond C. Organisms resist temperature changes, although they give off heat due to chemical reactions D. Water can act as a solvent E. The pH of water remains exactly neutral

B. A water strider can walk across the surface of a small pond.

Desert rabbits are adapted to the warm climate because their large ears aid in the removal of heat due to the A. High Surface tension of water B. High heat of vaporization of water C. High specific heat of water D. Buffering capacity of water E. Dissociation of water molecules

B. High heat of vaporization of water

Ice is lighter and floats in water because it is a crystalline structure in which each water molecule is bonded to a maximum of four other water molecules by which kind of bond? A. Ionic B. Hydrogen C. Covalent D. A and C only E. A, B, and C

B. Hydrogen

Which of the following is true when an ice cube cools a drink? A. Molecules collisions in the drink increase B. Kinetic energy in the drink decreases C. A calorie of heat energy is transferred from the ice to the water of the drink D. The specific heat of the water in the drink decreases E. Evaporation of the water in the drink increases

B. Kinetic energy in the drink decreases

In a single molecule of water, the two hydrogen atoms are bonded to a single oxygen atom by A. Hydrogen bonds B. Nonpolar covalent bonds C. Polar covalent bonds D. Ionic bonds E. Van der Waals interactions

B. Nonpolar Covalent Bonds

Which of the following is a correct definition of a kilocalorie? A. The amount of heat required to raise the temperature of 1 g of water by 1°F B. The amount of heat required to raise the temperature of 1 g of water by 1°C C. The amount of heat required to raise the temperature of 1 kg of water by 1°F D. The amount of heat required to raise the temperature of 1 kg of water by 1°C E. The amount of heat required to raise the temperature of 1,000 g of water by 1°F

B. The amount of heat required to raise the temperature of 1 g of water by 1°C

The formation of ice during colder weather helps moderate the seasonal transition to winter. This is mainly because A. The breaking of hydrogen bonds absorbs heat B. The formation of hydrogen bonds releases heat C. The formation hydrogen bonds absorbs heat D. There is greater evaporative cooling of lakes E. Ice denser than liquid water

B. The formation of hydrogen bonds releases heat.

What determines the cohesiveness of water molecules? A. Hydrophobic interactions B. Nonpolar covalent bonds C. Ionic bonds D. Hydrogen bonds E. Both A and C

D. Hydrogen Bonds

Water's high specific heat is mainly a consequence of the A. Small size of the water molecules B. High specific heat of oxygen and hydrogen atoms C. Absorption and release of heat when hydrogen bonds break and form D. Fact that water is a poor heat conductor E. Inability of water to dissipate heat into dry air

C. Absorption and release of heat when hydrogen bonds break and form.

What do cohesion, surface tension, and adhesion have in common with reference to water? A. All increase when temperature increases B. All are produced by ionic bonding C. All are properties related to hydrogen bonding D. All have with nonpolar covalent bonds E. C and D only

C. All are properties related to hydrogen bonding

If the pH of a solution is increased from pH 5 to pH 7, it means that the A. Concentration of H+ is 2 times greater than what it was at pH 5 B. Concentration of H+ is 2 times less than what it was at pH 5 C. Concentration of OH- is 100 times greater than what it was at pH 5 D. Concentration of OH- is 100 times less than what it is was at pH 5 E. Concentration of H+ is 100 times greater and the concentration of OH- is 100 times less than what they were pH 5

C. Concentration of OH- is 100 times greater than what it was at pH 5

Water's surface tension and heat storage capacity is accounted for by its A. Orbitals B. Weight C. Hydrogen bonds D. Mass E. Size

C. Hydrogen bonds

Temperature usually increases when water condenses. Which behavior of water is most directly responsible for this phenomenon? A. The change in density when it condenses to form a liquid or solid B. Reactions with other atmospheric compounds C. The release of heat by the formation of hydrogen bonds D. The release of heat by the breaking of hydrogen bonds E. The high surface tension of water

C. The release of heat by the formation of hydrogen bonds

Which of the following is an example of a hydrophobic material? A. Paper B. Table salt C. Wax D. Sugar E. Pasta

C. Wax