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PHYPHARM > IONIC EQUILIBRIUM & BUFFERS > Flashcards

IONIC EQUILIBRIUM & BUFFERS Flashcards

1
Q

formation of ions

A

ionization

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2
Q

separation of a species into to two or more

A

dissociation

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3
Q

The equilibrium established between the unionized molecules and the ions in the solution of weak electrolytes.

A

ionic equilibrium

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4
Q

degree of ionization is pH dependent

A

weak electrolytes

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5
Q

particles have no charge

A

unionized

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6
Q

with charge

A

ionized

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7
Q

Acid + acid

A

unionized, lipophilic, insoluble

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8
Q

Base + base

A

unionized, lipophilic, insoluble

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9
Q

Acid + base

A

salt form, ionized, hydrophilic, soluble

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10
Q

Formed by a chemical reaction between: a base and an acid.

A

salts

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11
Q

will not completely dissolved in water; they only partially dissolved in water

A

weak acid & base

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12
Q

Protolysis or the transfer of protons

A

Protolytic Reaction

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13
Q

A basic solvent capable of accepting protons from the solute

e.g., acetone, ether, liquid ammonia

A

protophilic

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14
Q

A proton-donating compound and is represented by acids

formic acid, acetic acid, sulfuric acid, liquid HCl, and liquid HF

A

protogenic

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15
Q

Neither accept nor donates protons

hydrocarbons

A

aprotic

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16
Q

A specie that can function either as an acid or base and are said to be amphoteric in nature

A

ampholyte

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17
Q

Compounds or mixtures of compounds that by their presence in a solution, resist changes in pH upon the addition of small quantities of acid or alkali

A

buffers

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18
Q

acetic acid and sodium acetate

A

weak acid & conj base

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19
Q

ammonium hydroxide and ammonium chloride

A

weak base & conj acid

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20
Q

resistance to a change in pH

A

buffer action

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21
Q

acidity constant

A

Ka

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22
Q

basicity constant

A

Kb

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23
Q

self-ionization of water

A

Autoprotolysis

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24
Q

acts both as an acid and as a base

A

amphoteric

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25
Q

water dissociation constant

A

Kw

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26
Q

donates/accepts one proton (one Ka)

A

monoprotic

27
Q

donates/accepts two or more protons

A

polyprotic

28
Q

The degree of acidity and basicity depends on
H+, OH-, pH or pOH

A

pH value

29
Q

negative logarithm of a value

A

p function

30
Q

pH and pOH lie between

A

0 - 14

31
Q

The ____ in the scientific notation gives you an idea of the pH, and vice versa.

A

exponential term

pH = 8

[H+] = 1 x 10-⁸

32
Q

the higher the OH-, the more ____ the substance is

A

basic

33
Q

the higher the H+, the more ____ the substance is

A

acidic

34
Q

strong acid

A

pH = -logCa

35
Q

strong base

A

pH = 14 + logCb

36
Q

weak acid

A

pH = -1/2log(Ca x Ka)

37
Q

weak base

A

pH = 14 + 1/2log(Cb x Kb)

38
Q

The magnitude of resistance of buffer to pH changes

A

Buffer Capacity (β)

39
Q

Buffer Capacity (β) is also known as

A

Buffer index
Buffer efficiency
Buffer value

40
Q

Exact Equation for Buffer Capacity

A

B = 2.3C (Ka[H+] / (Ka + [H+])²

C = total conc. of buffer

41
Q

Maximum Buffer Capacity

A

0.576C

42
Q

BLOOD

maintained at pH ____

A

7.4

43
Q

primary buffer in plasma

A

BLOOD

44
Q

BLOOD

secondary buffer in

A

erythrocytes

45
Q

BLOOD

life threatening at pH

A

less than 6.9, greater than 7.8

46
Q

LACRIMAL FLUID (TEARS)

maintained at pH

A

7.4

47
Q

LACRIMAL FLUID (TEARS)

discomfort & flow of tears at pH

A

less than 6.6, greater than 9

48
Q

average pH of urine

A

6 (about 4.5 - 7.8)

49
Q

Frequently used in formulation of ophthalmic solutions

A

pharmaceutical buffers

50
Q

Boric acid + sodium carbonate (pH 5-9)

A

GIFFORD

51
Q

Salts of sodium phosphate + NaCl (pH 6-8)

A

SORENSEN

52
Q

Salts of sodium phosphate + NaCl (pH 6-8) is also called

A

PHOSPHATE BUFFERED SALINE (PBS)

53
Q

Boric acid + sodium borate + NaCl (pH 7-9)

A

PALITZSCH

54
Q

CLARK-LUBS MIXTURES

HCl & KCl

A

1.2 - 2.2

55
Q

CLARK-LUBS MIXTURES

HCl & potassium hydrogen phthalate

A

2.2 - 4.0

56
Q

CLARK-LUBS MIXTURES

NaOH & potassium hydrogen phthalate

A

4.2 - 5.8

57
Q

CLARK-LUBS MIXTURES

NaOH & KH₂PO₄

A

5.8 - 8.0

58
Q

CLARK-LUBS MIXTURES

H₃BO₃, NaOH, & KCl

A

8 - 10

59
Q

General Procedures for Preparing Pharmaceutical Buffer Solutions

Select a weak acid having pKa approximately ____ to the desired pH at which the buffer is used

A

equal

60
Q

General Procedures for Preparing Pharmaceutical Buffer Solutions

Calculate the ____ of salt and weak acid.

A

molar ratio

61
Q

General Procedures for Preparing Pharmaceutical Buffer Solutions

Concentration of individual salt and acid of ____ is sufficient

A

0.05 - 0.5M

62
Q

General Procedures for Preparing Pharmaceutical Buffer Solutions

Determine the ____ and ____ Adjust if necessary.

A

pH & β

63
Q

Expressing the quantities of the hydroxide and hydrogen ions into a logarithmic scale

A

SORENSEN’S pH

64
Q
  • One of the most important properties of a drug
  • Can be related to
    o Physiologic and pharmacologic activity
    o Solubility
    o Absorption
  • Predicts which direction an acid-base reaction lies and what extent the reaction goes to completion
    o Measures the extent on how a weak acid or weak
    base will undergo ionization or not
A

Acid dissociation constant
Acidity constant
Ka

PHYPHARM (28 decks)

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