Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Biochemistry > Acids and Bases > Flashcards

Acids and Bases Flashcards

1
Q

True or false. There can be partial changes in polarity within 1 molecule?

A

True.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

The __________ of adjacent water molecules allow them to form hydrogen bonds with one another.

A

Polar regions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Rate these bonds in order of strength.
Ionic bonds, covalent bonds, hydrogen bonds, Van der Waals

A

1.) Covalent (20-200 kcal/mol)
2.) Ionic (10-100 kcal/mol)
3.) Hydrogen (5 kcal/mol)
4.) Van der Waals (0.5 kcal/mol)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Solutes dissolve in __________.

A

Liquids.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

_________ dissolve solutes.

A

Solvents

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

In a _________: solute dissolves in solvent.

A

Solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Define solubility

A

Ease of dissolving

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What does water dissociate into?

A

H+ + OH-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is the pH range for cell survival?

A

6.8 - 7.8

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Sulfuric acid is considered a (strong/weak) acid that (will/will not) ionize completely in water.

A

strong, will

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

An acid is a molecule that can give up a (H+/OH-).

A

H+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

A base is a molecule that can give up a (H+/OH-).

A

OH-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

HCl is an example of a (strong/weak) acid. When added to water it (completely/partially) ionizes.

A

strong/completely

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

An example of a (strong/weak) base is NaOH. When added to water it (completely/partially) ionizes.

A

strong/completely

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

An example of a (weak/strong) (acid/base) is CH3COOH. When added to water it will (completely/partially) ionize.

A

Weak/acid/partially

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Acetic acid can act as a ______________ and its properties can be described by the ____________________ Equation.

A

Buffer/Henderson-Hasselbalch

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

The Henderson-Hasselbach equation only applies to (strong/weak) acids or bases.

A

Weak

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What measurement is the acid dissociation constant?

A

pKa

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What does pKa measure?

A

How strong or weak an acid is

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

True or false. pKa is a number that helps us understand how easily an acid can give away a hydrogen ion (H+) to become a negatively charged ion (anion).

A

True.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

If an acid has a (low/high) pKa, it means it’s strong and readily gives away its hydrogen ion. If it has a (low/high) pKa, it’s a weak acid and doesn’t easily give away its hydrogen ion.

A

Low/high

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Why are pKa values important?

A

They help us predict how substances will behave in chemical reactions and how they will interact with other chemicals. So, pKa is a way to quantify the strength of acids.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What does the Henderson-Hasselbach equation calculate (2)? And which values does it use to calculate this?

A

The pH of a solution given:
1.) The pKa (strength of acid/base) of a weak acid or base
2.) The concentration of the protonated or deprotonated forms

And the ratio of (deprotonated):(protonated) forms of a weak acid or base, given:
1.) The pH and the pKa of the weak

24
Q

If you have a weak base B and it reacts with a proton (H+), it becomes its ________ because it has gained a proton.

A

conjugate acid BH+

25
Q

Which equation is this:

pH=pKa + log (deprotonated)/protonated)

A

The Henderson-Hasselbach equation

26
Q

If you have a weak acid HA and it loses a proton (H+), it becomes its ____________ because it has lost a proton.

A

Conjugate base A-

27
Q

When the pH = pKa, the amount of _______and _______ are equal

A

Salt and acid

28
Q

When pH = pKa what is the resulting pH?

A

4.74

29
Q

Acedic acid will buffer best _______ pH units above and below its pKa.

A

1.0 pH units

30
Q

Could acetic acid act as a buffer in the cell?

A

No. 4.74 +/- 1.0 is not in the range of 6.8-7.8 (cell pH)

31
Q

Give an example of an extracellular fluid buffer system.

A

Bicarbonate-carbonic acid buffer system

32
Q

Give an example of an RBC buffer system.

A

Hb buffer system

33
Q

Give an example of an intracellular buffer system.

A

Phosphate buffer system

34
Q

Proteins act as what 2 buffering systems?

A

Intracellular and plasma buffers

35
Q

A _____________ can maintain a solution at roughly the same pH and resist the action of an alkaline or an acid. (Up to a point)

A

Buffer

36
Q

HA represents a ___________ ________.

A

Weak acid.
H= H+
A= Whatever else is needed to complete the weak acid

37
Q

In HA «» H+ + A- , what does A- represent?

A

Conjugate base

38
Q

In HA «» H+ + A- Is the equilibrium equal

A

No, it pulls toward HA, because this is a weak acid. It only partially dissociates

39
Q

When HA (weak acid) interacts with OH- (alkaline) what happens?

A

H20 and A- are produced, creating a neutral solution and a virtually unchanged pH.

40
Q

When adding a soluble salt of HA to the solution, what happens? And why?

A

The soluble salt acts as a strong base and therefore can fully disassociate, creating a lot of A-, which will react with the H+ in the solution and create HA. Because this is a weak acid it will not have much effect on the pH.

41
Q

How does a salt form in a neutralization reaction?

A

When a metal ion from a base replaces the H+ ion from an acid.

42
Q

The direction of the reaction is determined by whether it raises or lowers the ______.

A

pH

43
Q

In a buffering system, how is the pH lowered?

A

Releasing H+

44
Q

In a buffering system, how is the pH raised?

A

Binding H+

45
Q

How can we predict the chemical reaction based on the relative concentrations of H+.

A

If we are removing H+ from solution, we compensate by releasing H+ into solution.

If we are adding H+ to the solution, we compensate by removing H+ from the solution.

46
Q

Which enzyme is working to create equilibrium with dissolved CO2 in the bicarbonate-carbonic acid buffering system?

A

Anhydrase

47
Q

Which buffering system is the most effective extracellular buffer?

A

The bicarbonate buffering system

48
Q

How can the lung modify its rate of CO2 removal?

A

By increasing ventilation

49
Q

In CO2 formation in the tissues: When CO2 is produced as a result of fuel oxidation, it will dissolve and be converted to what, using what enzyme in the RBC.

A

Converted to H2CO3 by carbonic anhydrase.

50
Q

In CO2 formation in the tissues: After CO2 is converted to H2CO3, what happens to it? Via what?

A

It will ionize and be exported in the plasma via the HCO3-/Cl- transporter (anion exchanger protein.)
HCO3- leaves the cell and Cl- enters.

51
Q

How is the H+ buffered in the RBC, once H2CO3 is ionized?

A

It is buffered by Hb

52
Q

What does the oxygenation of hemoglobin promote?

A

Dissociation of hydrogen ions from hemoglobin. The H+ then bind to the HCO3- (with carbonic anhydrase) and form carbonic acid, which then dissociates to form CO2 and H20, and the CO2 gets breathed out.

53
Q

The body maintains it’s pH with buffers that help maintain neutral pH and by the expiration of ______ through the lungs, and the excretion of ______ and other ions through the kidneys.

A

CO2, NH4+

54
Q

What 3 parts does a buffer have?

A

1.) Aqueous solution
2.) A weak acid
3.) The weak acid’s conjugate base

H20+HA «» H30+ + A-

55
Q

If pH>pKa, then A- concentration is (> or <) than HA?

A

>

56
Q

If pH is less than pKa, then A- concentration is (less than/greater than) HA?

A

Less than

Biochemistry (14 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions