Biochemistry Chapter 3-AP Bio Part 3

Question 0

Hydrogen ion (H+)

Answer 0

A single proton with a charge of 1+

Question 1

What happens occasionally to a hydrogen atom participating in a hydrogen bond between TWO water molecules

Answer 1

The hydrogen atom shifts from one molecule to the other, leaving its electron behind

Question 2

Hydroxide ion

Answer 2

(OH-) the water molecule that lost a proton that has a charge of -1

Question 3

Hydronium ion

Answer 3

The proton that binds to the other water molecule.

Question 4

H+ does not what

Answer 4

Exist on its on in an aqueous solution, always associated with H3O+

Question 5

Dynamic equilibrium

Answer 5

When water molecules disassociate at the same rate that they are being reformed from H+ and OH-. At this point the concentration of water greatly exceeds the concentrations of H+ and OH-.

Question 6

The dissociation of water is __________________

Answer 6

Reversible and rare

Question 7

H+ and OH- are extremely ____________

Answer 7

Negative

Question 8

What can changes in H+ and OH- result in

Answer 8

Drastically affect a cell’s proteins and other complex molecules.

Question 9

What happens when acids dissolve in water

Answer 9

They donate additional H+ to the solution

Question 10

Acid

Answer 10

A substance that increases the hydrogen ion concentration of a solution

Question 11

Acidic solution

Answer 11

A solution having more H+ than OH-

Question 12

Base

Answer 12

A substance that reduces the H+ concentration of a solution

Question 13

How to bases reduce H+ ion concentration

Answer 13

Directly by accepting hydrogen ions or indirectly by dissociating to form hydroxide ions, which combine with hydrogen ions and form water.

Question 14

Weak acids

Answer 14

Acids that reversibly release and accept back hydrogen ions.

Question 15

pH

Answer 15

The negative logarithm (base 10) of the hydrogen ion concentration

Question 16

pH _________ as concentration ____________

Answer 16

Declines, increases

Question 17

A solution of pH 3 is not twice as acidic as pH 6

Answer 17

but (10 x 10 x 10) more acidic

Question 18

Buffer

Answer 18

A substance that minimizes changes in the concentration of H+ and OH- ions by accepting hydrogen ions from the solution when they are in excess and donating hydrogen ions to the solution when they have been depleted.

Question 19

Carbonic acid

Answer 19

A buffer formed when CO2 reacts with water in blood plasma. Dissociates to yield a bicarbonate ion (HCO3-) and a hydrogen ion (H+)

Question 20

The chemical equilibrium between carbonic acid and bicarbonate acts a

Answer 20

pH regulator

Question 21

What happens if the H+ concentration in blood begins to fall

Answer 21

The reaction proceeds to the right and more carbonic acid dissociates, replenishing hydrogen atoms

Question 22

What happens if the H+ concentration in blood begins to rise

Answer 22

The reaction proceeds to the left, with HCO3- (the base) removing the hydrogen ions from the solution and forming H2CO3.

Question 23

Carbonic acid-bicarbonate buffering system consists of

Answer 23

an acid and a base in equilibrium with each other.

Question 24

Most buffers have

Answer 24

Acid base pairs

Question 25

What happens when CO2 dissolves in seawater (ocean acidification)

Answer 25

It reacts with water to form carbonic acid which lowers the pH of the ocean

Question 26

What happens as seawater acidifies

Answer 26

The extra hydrogen ions combine with carbonate ions to form bicarbonate ions,,,reducing the carbonate ion concentration.