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INORG LEC > PHARMA AIDS > Flashcards

PHARMA AIDS Flashcards

1
Q

Agents that are important in the:
-preparation
-preservation, &
-storage of pharmaceutical products

-are not API
-have little to NO pharmacological activity

A

pharmaceutical aids and necessities

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2
Q

adsorb fluids and moisture and keep pharmaceutical products dry

A

Adsorbents

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3
Q

inert substances and vehicles used in pharmaceutical to dilute and decrease the concentration of the API or increase the bulk of formulation

A

Diluents

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4
Q

are substances added for overcoming agglomeration of the dispersed particles and for increasing the viscosity of the medium so that particle settle down very slowly

A

Suspending Agents

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5
Q

substances used in the clarification process

A

Filter Aids

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6
Q

compound that are used to prevent chemical and physical degradation of liquid or semi-solid preparations against antimicrobial contamination

A

Preservatives

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7
Q

frequently employed in the conversion of drugs to chemical forms

A

Acids & Bases

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8
Q

maintain the pH of various formulations within prescribed limits

A

Buffers

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9
Q

prevent oxidative decomposition of pharmaceutically active components

A

Antioxidants

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10
Q

primary solvent or liquid phase in most liquid pharmaceutical preparations

A

Water

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11
Q

used for storage and as dispensing container for most drug products

A

Glass

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12
Q

Acid forms what in water?

A

H+

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13
Q

Base forms what in water?

A

-OH

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14
Q

can donate 2 or more H+ per molecule

A

Polyprotic acid

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15
Q

can only donate 1 H+ per molecule

A

Monoprotic acid

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16
Q

Brønsted-Lowry Theory

A

Acids: H+ donors
Bases: H+ acceptors

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17
Q

substances that can act as an acid or base

A

Amphoteric

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18
Q

Lewis Theory

A

Acids: electron pair acceptor
Bases: electron pair donor

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19
Q
  • taste sour (lemons, vinegar)
  • turn blue litmus paper red.
  • solutions: pH <7
  • can conduct electricity in solution.
A

Acids

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20
Q

are strong electrolytes.

A

Strong acids and bases

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21
Q
  • taste bitter and feel slippery.
  • turn red litmus paper blue.
  • solutions: pH > 7
  • can conduct electricity in solution.
A

Bases

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22
Q

Strong Acids (7):

A
  • HCl (hydrochloric acid)
  • HNO3 (nitric acid)
  • H2SO4 (sulfuric acid)
  • HBr (hydrobromic acid)
  • HI (hydroiodic acid)
  • HClO3 (chloric acid)
  • HClO4 (perchloric acid)
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23
Q

Strong Bases (8):

A
  • LiOH (lithium hydroxide)
  • NaOH (sodium hydroxide)
  • KOH (potassium hydroxide)
  • Ca(OH)2 (calcium hydroxide)
  • RbOH (rubidium hydroxide)
  • Sr(OH)2 (strontium hydroxide)
  • CsOH (cesium hydroxide)
  • Ba(OH)2 (barium hydroxide)
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24
Q

is the potential of hydrogen ions.

A

pH

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25
Q

is the potential of hydroxide ions.

A

pOH

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26
Q

As pH increases, pOH increases.
As pH decreases, pOH decreases.

TRUE OR FALSE

A

FALSE

As pH increases, pOH decreases.
As pH decreases, pOH increases.

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27
Q

OFFICIAL INORGANIC ACIDS

A
  • Boric acid (H3BO3)
  • Hydrochloric acid (HCl)
  • Diluted Hydrochloric acid
  • Nitric acid (HNO3)
  • Phosphoric acid (H3PO4)
  • Diluted Phosphoric acid
  • Sulfuric acid
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28
Q

Found in seawaters, certain plants, in nearly all fruits and in some volcanic steam jets.

Uses: Antiseptic, since it is a weak bacteriostatic acid agent; in 2% w/v concentration as eyewash and as buffer in ophthalmic solutions

A

Boric acid (H3BO3)

Synonyms: Hydrogen borate, Boracic acid, and Orthoboric acid.

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29
Q

Boric acid Available in three crystalline forms:

A

a. colorless, odorless, pearly scales
b. six-sided triclinic crystals
c. white, odorless powder with a soapy feel

The toxicity of boric acid makes it unfit to be taken orally.

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30
Q
  • Prepared/ obtained from NaCl or rock salt
  • When hydrogen chloride is dissolved in water it is formed. It is a simple diatomic molecule.
  • Use: A pharmaceutical aid as an acidifying agent
A

Hydrochloric acid (HCl)

Synonyms: Chlorhydric acid,
Spirit of Sea Salt, Muriatic acid

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31
Q

Uses:
1. Aiding in the conversion of pepsinogen into pepsin
and of proteins into peptones;
2. Serves as a gastric antiseptic; and,
3. It is also used in the management of gastric
achlorhydria and hypochlorhydria.

A

Diluted Hydrochloric acid

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32
Q

is the absence of HCl in the stomach

A

Achlorhydria

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33
Q

deficiency of HCl production of the stomach

A

Hypochlorhydria

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34
Q
  • Prepared from a mineral or a salt, knowns as Potassium nitrate.
  • Colourless but as it gets older it turns into a yellow cast.
  • Highly corrosive and toxic.
  • Causes severe skin burn.
  • Reacts with hydroxides, metals, and oxides to form nitrate salts.

Uses:
* Manufacture of sulfuric acid
* Coal tar dyes and explosives
* Nitrating agent in Pyroxylin USP XVII
* Source of nitrate ion in the preparation of milk of bismuth
* Externally, for the elimination of chancres and warts

A

Nitric acid (HNO3)

Aqua Fortis, Aqua Fuerte

Synonyms: Spirit of Nitre,

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35
Q
  • is a weak acid with the chemical formula H3PO4.
  • Present in teeth and bones and helps in metabolic processes
  • In its liquid form, it appears as a clear, colourless solution
  • In its solid form, it appears as a transparent, crystalline solid
A

Phosphoric acid (H3PO4)

Synonyms: Orthophosphoric acid, Acido Orthofosforico

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36
Q
  • The most important -oxy acid of phosphorus
  • Used to make phosphate salts for fertilizers.
  • Used in dental cement, albumin derivatives preparation and in the sugar and textile industries.
A

Phosphoric acid (H3PO4)

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37
Q

Uses:
* A tonic and stimulant to the gastric mucous membranes;
* A synergistic substance to pepsin and acids to the formulation of peptones.

A

Diluted phosphoric acid

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38
Q
  • At higher concentrations, it acts as an oxidizing agent and dehydrating agent.
  • A syrupy liquid which is odourless and has no colour.
  • Water-soluble and releases heat when dissolved in water.
  • Widely used in the manufacturing of fertilizers.
  • used in chemical synthesis and wastewater processes.
A

Sulfuric acid (H2SO4)

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39
Q

OFFICIAL INORGANIC BASES

A
  • Strong Ammonia Solution
  • Diluted Ammonia Solution
  • Calcium Hydroxide
  • Potassium Hydroxide
  • Sodium Hydroxide
  • Sodium Carbonate
  • Soda Lime
  • Potassium Bicarbonate
  • Sodium Bicarbonate
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40
Q

Uses:
* Bronsted base
* Manifacture of nitric acid and sodium bicarbonate
* Preparation of aromatic spirit and ammonia cal silver nitrate solution

A

Strong Ammonia Solution (NH4OH)

Synonyms: Ammonium hydroxide, Stronger Ammonia Water

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41
Q

is used to treat or prevent syncope

A

Aromatic Ammonia Spirit

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42
Q

is an alkaline solution of ammonia cal silver nitrate and is used to test for aldehydes

A

Tollens’ reagent

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43
Q
  • Prepared from strong ammonia solution
  • Known as ammonia water or household ammonia
  • Employed as circulatory inhalant through inhalation of vapors

Use:
Externally, it is used as counter-irritant agent

A

Diluted Ammonia Solution (NH4OH)

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44
Q

Preparation: Manufactured from lime or calcium oxide through the addition of water in limited amounts in slaking process, characterized by the avid absorption of water by the oxide lumps, and by the final disintegration into fine powder.

A

Calcium Hydroxide Ca(OH)2

Synonyms: Slaked lime,
Calcium hydrate

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45
Q

Uses:
* Medicinally used as fluid electrolyte and topical astringent
* Utilized for its high hydroxide ion concentration in pharmaceutical preparations
* Utilized for it’s potentially high hydroxide ion concentration
* Form calcium soaps, which have emulsifying properties
* Combined with NaOH or KOH in a mixture known as soda lime

A

Calcium Hydroxide Ca(OH)2

46
Q

Properties:
* Deliquescent
* Very strong base with caustic/ corrosive effect on tissues (handle carefully)

Uses:
* A caustic in veterinary practice
* A saponifying agent to hydrolyze esters of fatty acids into their constituent alcohols and potassium salt

A

Potassium Hydroxide (KOH)

Synonyms: Caustic potash, Potassa

47
Q

Properties:
* It attacks soft glass (containers should be made of hard glass with rubber stoppers
* Glass-stoppered bottles can be used if a little petroleum or paraffin is spread around the stopper
* Not borosilicate, a soft glass has high coefficients of thermal expansion; thus it does not require a high temperature to make them soft.

A

Sodium Hydroxide (NaOH)

Synonyms: Caustic soda , Soda lye

48
Q

Use:
Same as potassium hydroxide but has more advantage since it is less deliquescent, milder, and cheaper

A

Sodium Hydroxide (NaOH)

49
Q

Uses:
In pharmaceutical preparations, its basicity forms sodium salts of acidic drugs

A

Sodium Carbonate (Na2CO3.H2O)

Synonyms: Monohydrated Sodium Carbonate

50
Q

A mixture of Ca(OH)2 and NaOH or KOH or both intended for metabolism tests, anesthesia & O2 therapy.

A

Soda Lime (NaOH + Ca0)

51
Q

Uses:
Buffering agent for pharmaceutical preparations

A

Potassium Bicarbonate (KHCO3)

52
Q

Use:
Preferred in the preparation of effervescent mixtures containing sodium bicarbonate and organic acids such as tartaric or citric. These additives react to liberate CO2 that acts as a disintegrator producing effervescence when in water.

A

Sodium Bicarbonate (NaHCO3)

Synonym: Sodium Hydrogen Carbonate

53
Q

is a solution of a weak acid and its salt (conjugate base) or weak base and its salt (conjugate acid), that resists drastic changes in pH when small amounts of acid or base are added to it.

A

buffer

54
Q

Buffers control the pH of pharmaceutical products within certain specified limits for these reasons:

A
  • Chemical stability,
  • Solubility of the drug, and
  • Patients comfort.
55
Q

Characteristics of a Buffer:

A
  • It has a definite pH value.
  • Its pH value doesn’t change on keeping for a long time.
  • Its pH value doesn’t change on dilution.
  • Its pH value doesn’t change even with the addition of a small amount of a strong acid or a base.
56
Q

Factors which can produce alterations in pH includes the following:

A
  • Alkali in certain inexpensive containers;
  • Gases present in air such as CO2 and NH3;
  • Effects of temperature, light, humidity, radiation and solvent used; &
  • Presence of other chemicals resulting from contamination or from the unintentional/intentional mixing of different products.
57
Q

How to make buffers?

A buffer must contain a weak acid and its conjugate base. There are several ways a solution containing these two components can be made:

A
  • Buffers can be made from weak acids or base and their salts.
  • Buffers can be made from two salts that provide a conjugate acid-base pair.
  • Buffers can be made by adding a strong acid or base to a weak acid or base.
58
Q

Mechanism of Action of a Buffer

A
  • Acid / Its salt
  • Base / Its salt
59
Q

Important Considerations in Selecting or Choosing a Buffer

The selected buffer should not:

A

A. Participate in oxidation-reduction reaction
B. Alter the solubility of other components
C. Form complexes with active ingredient

60
Q

Consider the following when choosing a buffer:

A
  1. Volatile species should not be used as buffers
  2. It should not have any influence on the pharmacological activity of the API
  3. The use of pharmaceutical should be considered in choosing a buffer for a product. If it is to be ingested, buffers containing borates should not be used as they are toxic systematically.
61
Q

Two Inorganic Buffer Systems

A
  • Phosphate Buffer System
  • Borate Buffer System
62
Q

Uses :
It is included in preparation containing metals that would otherwise precipitate in the presence of phosphate. Since borates are toxic, this buffer system is suitable in external preparations, opthalmic, and nasal solutions but is contraindicated in parenteral solutions.

A

Borate Buffer System

63
Q

Three Primary Borate Buffer Systems

A
  1. FELDMAN’S BUFFER SYSTEM
  2. ATKIN’S AND PANTIN BUFFER SYSTEM
  3. GIFFORD BUFFER SYSTEM
64
Q

boric acid+NaCl (to make it isotonic) + sodium borate

A

FELDMAN’S BUFFER SYSTEM

65
Q

sodium carbonate + boric acid + NaCl

A

ATKIN’S AND PANTIN BUFFER SYSTEM

66
Q

boric acid + KCl (to make it hypotonic) + sodium borate

A

GIFFORD BUFFER SYSTEM

67
Q

Two Categories of Buffer System in Pharmacy

A
  • Standard Buffer Systems
  • Actual Pharmaceutical Buffer
68
Q

designed to provide a solution having a specific pH for analytical purposes

A

Standard Buffer Systems

69
Q

designed to maintain pH limits in drug preparation

A

Actual Pharmaceutical Buffer

70
Q

Standard buffer solutions having pH ranges between 1.2 and 10.0 can be prepared by the appropriate combinations of :

A
  • boric acid and sodium chloride, 0.2M
  • hydrochloric acid, 0.2M
  • potassium chloride, 0.2M
  • potassium phosphate, monobasic 0.2M
  • potassium biphthalate, 0.2M
  • sodium hydroxide, 0.2M
  • acetic acid, 2N
71
Q

50 mL potassium chloride solution with a specified volume of 0.2M HCI and water

A

hydrochloric
acid buffer

pH= 1.2 - 2.2

72
Q

50 mL of potassium biphthalate solution with a specified volume of 0.2M HCl and water

A

acid phthalate
buffer

pH= 2.2 - 4.0

73
Q

a specified amount of sodium acetate solutions with a specified volume of the acetic acid solution and water

A

acetate buffer

pH= 4.1 - 5.5

74
Q

50 mL of potassium biphthalate solution with a
specified volume of NaOH and water

A

neutralized phthalate buffer

pH= 4.5-5.8

75
Q

50 mL of monobasic potassium phosphate solution with a specified volume of NaOH and water

A

phosphate buffer

pH= 5.8 - 8.0

76
Q

50 mL of boric acid and potassium chloride solution with a specified volume of NaOH and water

A

alkaline
borate
buffer

pH= 8.0 - 10.0

77
Q
  • A chemical compound consisting of two hydrogen atoms and one oxygen atom forming a polar covalent bond.
  • Odorless, tasteless, and a colorless liquid that is in small quantities and greenish blue in deep layers.
  • One of the most important molecules to humanity.
  • A crucial pharmaceutical agent due to its solvent powers and physiological inertness.
A

WATER

78
Q

PROPERTIES OF WATER:

A
  • Water is polar.
  • Water is an excellent solvent.
  • Water has a high heat capacity.
  • Water has high heat vaporization.
  • Water has cohesive and adhesive properties.
  • Water is less dense as a solid than as a liquid.
79
Q

WHY IS WATER THE SOLVENT OF CHOICE?

A
  • Water is extensively used as a raw material, ingredient, and solvent in the processing, formulation, and manufacture of pharmaceutical products, active pharmaceutical ingredients (APIs), and intermediates.
  • Water can dissolve much more substances than any other liquid found in nature. However, water cannot dissolve every substance.
  • Water can be used in a variety of applications, some requiring extreme microbiological control and others requiring none.
  • Water may be present as an excipient or used for reconstitution of products, during synthesis, during production of the finished product or as a cleaning agent for rinsing vessels, equipment, primary packaging materials, etc.
80
Q

MAJOR CLASSIFICATIONS OF WATER

A
  • NATURAL WATER
  • POTABLE WATER
  • PURIFIED WATER
  • HEAVY WATER
81
Q

All forms of water, including any river, stream, dam, lake, pond, swamp, marsh, canal, whether natural or artificial or other body of water forming part of that water course. The purest natural water is rain water.

A

NATURAL WATER

82
Q

Water that is already filtered properly and is finally free from all contaminants and harmful bacteria. Purified water is fit to drink, or it can be called ‘drinking water after the purification processes, and is safe for both cooking and drinking.

It can be used during the manufacture of active substances and early stages of cleaning pharmaceutical manufacturing equipment.

A

POTABLE WATER

83
Q

Prepared by distillation, ion exchange, and reverse osmosis. Purified water is widely used for oral and topical products and in granulation processes for tablets and capsules.

First, it must meet the requirements for ionic and organic chemical purity and must be protected from microbial contamination before being used in pharmaceutical applications.

A

PURIFIED WATER

84
Q
  • Water that has high mineral contents (Ca2+ and Mg2+ ions) also bicarbonate and sulfates.
  • Calcium usually enters the water as either CaCO3, in the form of limestone and chalk, or calcium sulfate (CaCO4).
  • Slightly heavier than normal water and is not harmful to one’s health. (Formula of D2O)
A

HEAVY WATER

85
Q

TYPES OF NATURAL WATER

A

ALKALINE WATERS
CARBONATED WATERS
SALINE WATERS
SULFUR WATERS
CHALYBEATE WATERS
SILICEOUS WATERS
LITHIA WATERS

86
Q

Usually contain appreciable quantities of sodium and magnesium sulfates.

A

Alkaline Waters

87
Q

Those have been charged with carbon dioxide under pressure while in the Earth.

A

Carbonated Waters

88
Q

Have iron in solution or in suspension and are characterized by a ferruginous taste.

A

Chalybeate Waters

89
Q

Occur in the form of carbonate or chloride.

A

Lithia Waters

90
Q

Also called “Purgative Waters”. Hold relatively large amounts of magnesium and sodium sulfates with sodium chloride.

A

Saline Waters

91
Q

Have hydrogen sulfide.

A

Sulfur Waters

92
Q

Include very small amounts of soluble alkali silicates.

A

Siliceous Waters

93
Q

Description: clear, colorless, odorless liquid; purified by distillation or reverse osmosis.

Use: ingredient in official preparations and it tests and assays unless otherwise specified.

A

PURIFIED WATER

94
Q

Description: clear, colorless, odorless liquid; purified by distillation or reverse osmosis and contains no added substances.

Use: Pharmaceutic aid as a vehicle for dilution and reconstitution of suitable medicinal products for parenteral administration.

A

WATER FOR INJECTION

95
Q

Description: It is prepared from Water for Injection that is sterilized and packaged in prefilled syringes or in vials containing not more than 30 mL. It also has one or more suitable antimicrobial agents.

Use: to dilute or dissolve medications

NOTE: Label should state: “ NOT FOR USE IN NEONATES” as there were problems encountered with neonates and the toxicity of the bacteriostatic, benzyl alcohol

A

BACTERIOSTATIC WATER FOR INJECTION

96
Q

Description: clear, colorless, odorless liquid; water for parenteral; sterilized; no antimicrobial agent or other added substances.

Use: for fluid replacement only after suitable additives are introduced to approximate isotonicity and to serve as a vehicle for suitable medications.

A

STERILE PURIFIED WATER FOR INJECTION

97
Q

Description: clear, colorless liquid; water for injection that has been sterilized; no antimicrobial agent or other substance.

Use: an irrigating solution

A

STERILE WATER FOR IRRIGATION

NOTE: Label must say: “For irrigation only and NOT for injection”

98
Q

Description: It is prepared from Water for Injection, sterilized and suitably packaged with no added microbial agents.

Use: May relieve symptoms of inflamed, swollen blood vessels in your nasal passages.

A

STERILE WATER FOR INHILATION

99
Q

Are compounds that have the capability of functioning chemically as reducing agents.

They are pharmaceutical necessities since their addition prevents oxidative decomposition in the products.

A

Antioxidants

100
Q

Mechanism of Action of Antioxidants

A
  • An antioxidant is oxidized in place of an active compound.
  • The antioxidant reduces the already oxidized active constituent back to its normal oxidation state.
  • Inorganic antioxidants act through redox reactions. Redox reaction is when the oxidation-reduction reaction takes place simultaneously.
101
Q

Uses:
The formation of free iodine is prevented in diluted hydriodic and syrup.
Its presence in ferrous iodide syrup ensures the non-formation of both ferric ions and molecular iodine.

A

Hypophosphorous Acid (H2P02)

102
Q

Uses:
Salt of hypophosphorous acid are antioxidants
Sodium hypophosphite is a preservative in certain foods.
Ammonium hypophosphite is likewise a preservative in many preparations

A

Hypophosphorous Acid (H2P02)

103
Q

Uses:
It will protect many susceptible compounds from oxidation by reducing the oxidized form back to its original compounds or by reacting with oxygen before the susceptible compounds do.

A

Sulfur Dioxide (S02)

Synonym: Sulfurous Anhydride

104
Q

Uses:
It is usually in injectable preparations in impulses or vials.
It is used in industry to bleach wood pulp, fumigate grains, and arrest fermentation.

A

Sulfur Dioxide (S02)

105
Q

Synonyms:
Sodium hydrogen sulfite
Sodium acid sulfate
Leucogen

Uses:
It prevents oxidation of the compounds of phenol and catechol nucleus to quinones.

A

Sodium bisulfite (NaHSO3) or
Sodium metabisulfite (Na2S2O5)

106
Q

Uses:
It prepares water-soluble derivatives of normally insoluble drugs.

Bisulfite and metabisulfite can be found in ascorbic acid injections as reducing agents.

A

Sodium bisulfite (NaHSO3) or
Sodium metabisulfite (Na2S2O5)

107
Q

Uses:
As an inert atmosphere, it retards oxidation in oxidation-sensitive products and replaces air in containers for parenteral and solutions for topical applications.

A

Nitrogen (N2)

108
Q

Uses:
It contains sulfur in two different oxidation states.

> the oxidized sulfur atom is in a +6 state resisting further oxidation.

 > the remaining sulfur atom is in a zero oxidation state.
A

Sodium thiosulfate (Na2S2O3)

109
Q

Uses:

This oxidation polarity allows the compound to act as a reducing agent.

It also act as an antidote for cyanide poisoning.

A

Sodium thiosulfate (Na2S2O3)

110
Q

Uses:
Nitrite can act as both a reducing and oxidizing agent. Reduction of compounds with sodium nitrite results in the formation of nitrates.
It is an antidote for cyanide poisoning.

A

Sodium nitrite (NaNO2)

111
Q

Uses:
Nitrites in brine solutions are curing ingredients of meats and fish for they are excellent color developers, enhance flavor production, and prevent microbial growth. However, nitrite ions remain in cured meats and react with organic amines to form potentially carcinogenic N-nitrosamines.

A

Sodium nitrite (NaNO2)

INORG LEC (2 decks)

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