Brainscape's Knowledge GenomeTM

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


See full index

Pharmaceutics FINAL > Part 1 --Acid-Base Equilibria > Flashcards

Part 1 --Acid-Base Equilibria Flashcards

1
Q

According to the Arrhenius Theory (1887), what is the definition of an acid and what is the definition of a base?

A

acid – A substance that liberates (releases) hydrogen ions

base – A substance that supplies (releases) hydroxyl ions

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

what is the name of the modern theory of acids and bases?

A

the Bronsted-Lowry theory

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

According to the Bronsted-Lowry theory, give the definition of an acid and a base

A

acid – a substance, CHARGED OR UNCHARGED, that is capable of donating a proton

base – a substance, CHARGED OR UNCHARGED, that is capable of accepting a proton from an acid

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

according to the modern theories of acids and bases, define “strong acid” and “weak acid”

give a specific example of each

A

strong acid – high tendencies to give up protons
ex: HCl in water

weak acid – low tendencies to give up protons
ex: acetic acid (CH3COOH) in water

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

the modern theory of defining strong acids and strong bases is _____ dependent

explain how acetic acid and hydrochloric acid could either be strong or weak acids given this statement

A

SOLVENT dependent

as mentioned, HCl is a strong acid in WATER. however, when placed in glacial acetic acid, it has WEAK acid properties. It has a low tendency to donate its proton

As mentioned, acetic acid is a weak acid in WATER. however, when placed in liquid ammonia, it has STRONG acid properties — high tendency to donate its protons

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

according to the modern theories of acids and bases, name and explain 2 classes of solvents

A

protophilic solvent (basic)
protogenic solvent

protophilic solvent — capable of accepting protons from the solute

protogenic solvent – a proton-donating compound (acids)

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

give 3 examples each of protophilic and protogenic solvents

A

protophilic solvents – acetone, ether, liquid ammonia

protogenic solvent – represented by ACIDS: acetic acid, sulfuric acid, hydrochloric acid

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

_____ solvents are also known as basic solvents

A

protophilic

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

what is a “protolytic reaction”?

A

reactions involving transfer of one or more protons

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

give an example of a protolytic reaction

give the full formula and identify the acid and base as well as conjugate pairs

A

HCl in water

HCl + H2O —> H3O+ + Cl-

acid = HCl
base = H2O

conjugate pair: HCl and Cl- & H2O and H3O+

notice: SINGLE HEADED ARROW. complete ionization.

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

HCl + H2O —> H3O+ + Cl-

this is complete ionization due to _______. There is no _____ in the final solution

A

this is complete ionization due to the SINGLE HEADED ARROW and the fact that HCl is a strong acid

there is NO HCl in the final solution. complete ionization occurred

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

there are ___ types of protolytic reactions.
name them

A

4 types:

ionization
neutralization
hydrolysis
displacement

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

according to the Lewis Electron Theory, define an acid and a base

A

acid – a molecule or ion that accepts an electron pair to form a covalent bond

base – the substance that provides the pair of unshared electrons by which the base coordinates with the acid

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

According to the Lewis Electron theory, the substance that PROVIDES the electron pair is the base or the acid?

A

base

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

define equilibrium

A

a balance between 2 opposing forces or actions

rate of forward reaction = rate of reverse reaction

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

differentiate between the pH conditions in the stomach and in the small intestine

A

stomach environment is much more acidic than small intestine environment

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

True or false

water is a base

A

false – water can act as an acid or a base depending on what it’s reacting with

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

give the formula for acetic acid in water and identify the acid and the base, as well as conjugate pairs

A

CH3COOH + H2O <—–> H3O+ + CH3COO-

acid = acetic acid
base = water

conjugate pairs:
CH3COOH and CH3COO-
H2O and H3O+

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

Give the formula for RATE of the FORWARD reaction of Acetic Acid in Water

A

Rf = k1 * [CH3COOH] * [H2O]

in general —-
rate of forward reaction is proportional to the concentration of the REACTANTS

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

Give the formula for the RATE of the REVERSE reaction of Acetic Acid in water

A

kr = k2 * [H3O+]^1 * [CH3COO-]^1

in general – rate of reverse reaction is proportional to the concentration of the PRODUCTS

^1 indicates 1 mole of that compound in reaction

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

at equilibrium, ___ = ____

A

Rf = Rr

aka……

k1 * [CH3COOH]^1 * [H2O]^1 = k2 * [CH3COO-] * [H3O+]

22
Q

___ is the symbol for the dissociation constant of a weak acid

A

ka

23
Q

k=…………………. (assume acetic acid in water)

A

k = [H3O+][CH3COO-]/[CH3COOH][H2O]

24
Q

Ka =……

A

the dissociation constant of a weak acid

[H3O+][CH3COO-]/[CH3COOH]

25
Q

why is water not in the formula for dissociation of a weak acid? (Ka)

A

water is in enough excess to be assumed as a constant

26
Q

is HAc representing the ionized or unionized form of acetic acid?

A

unionized

ionized is Ac-

27
Q

give 3 equations for dissociation constant of weak acid (Ka)
(assume acetic acid in water)

A

Ka = [CH3COO-][H3O+]/[CH3COOH]

Ka = x^2/(c-x)

ka= x^2/c

28
Q

true or false

all salt forms can undergo complete ionization

A

false – most salt forms

29
Q

name 2 formulas for dissociation concentration of a weak acid

A

x^2 = Kac

x = [H3O+] = square root of Kac

30
Q

give formula for a non-ionized weak base in water

A

B + H2O <—–> OH- + BH+

31
Q

give the dissociation constant for the ionization of weak bases in water

A

Kb = [OH-][BH+]/[B]

32
Q

give the dissociation concentration formula for weak bases

A

[OH-] = square root of Kbc

33
Q

give the formula for sodium acetate

A

Na+ CH3COO-

34
Q

water can either be….

A

a weak acid or a weak base

35
Q

when you increase the temperature, what happens to the rate of the reaction?

A

the rate of the FORWARD reaction is increased.

-higher dissociation
-favors product formation

36
Q

why do we normally not mess with temperature too much to increase the rate of dissociation?

A

requires complicated storage for the product to remain at that temp

37
Q

What are “monoprotic electrolytes”

A

acids that donate a single proton and bases that accept a single proton

38
Q

what are “polyprotic electrolytes”

A

acids/bases that are capable of donating/accepting two or more protons

39
Q

what is the term for an electrolyte that can accept/donate 2 protons? What about 3?

give examples

A

diprotic or dibasic
diprotic acid = carbonic acid

triprotic or tribasic
triprotic acid = phosphoric acid

40
Q

give the formula for phosphoric acid

A

H3PO4

41
Q

what is the term for a species that can function as either an acid or a base?

A

an AMPHOLYTE

42
Q

what is neutral pH?
what is [H3O+] and [OH-] at this pH?

A

neutral pH is 7

both [H3O+] and [OH-] are 10^-7moles/L

43
Q

pKw =

A

14 ALWAYS

44
Q

pH + pOH = …….

A

pKw

45
Q

pKa + pKb = …….

A

pKw

46
Q

pK is a _____ exponent

A

dissociation

47
Q

how to find the hydrogen ion concentration [H3O+] of a weak acid?

A

[H3O+] = square root of Kac

48
Q

how to find the hydroxyl ion concentration [OH-] of a weak base?

A

[OH-] = square root kbc

49
Q

what is the sulfuric acid formula

A

H2SO4

50
Q

pKa = ……

A

-log Ka

51
Q

what is Ka?

A

dissociation constant

52
Q
A

Pharmaceutics FINAL (8 decks)

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