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PH 105.1 > Quantitative chem > Flashcards

Quantitative chem Flashcards

1
Q

Defined as the application of quantitative analytical chemistry…

  • To the analysis & determination of the purity and quality of drugs & chemicals used in pharmacy.
  • To the analysis & determination of the chemical constituents found in the human body whose altered concentration during disease states serve as diagnostic aids in the practice of medicines.
  • To the analysis of medicinal agents and their metabolities found in biological systems
A

QUANTITATIVE PHARM CHEM

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2
Q

importance

A

1.) Pharmacists must have the knowledge to advise medical practitioners on drug quality
2.) Pharmacist must alert health professionals to the influence which drugs may have on clinical laboratory methods.
3.) Pharmacists must monitor drug levels during therapy.

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3
Q

In case the quality of a drug product is questioned by a physician, a pharmacist is:
Responsible for initiating steps to determine if a product is defective:

A
  • Calling and advising the drug manufacturer of the problem involving the product
  • Analyzing the preparation in the prescription laboratory, borrowing needed equipment from a clinical laboratory
  • Sending a portion of the sample to a private laboratory for analysis
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4
Q

MANIFESTATION OF A DEFECTIVE PRODUCT

A
  1. Improper Labeling
  2. Discoloration
  3. Presence of Cloudiness
  4. Presence of Crystals
  5. Presence of Precipitates
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5
Q

“Sum of all factors” which contribute directly or indirectly to the safety, effectiveness, and reliability of the product.

A

QUALITY

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6
Q

Refers to the “sum of all procedures” undertaken to ensure the identity and purity of a particular pharmaceutical.

Such procedures may range from the performance of single chemical experiments which determine the identity and ________ for the presence of particular pharmaceutical substance (thin layer chromatography, infrared spectroscopy, etc) to more complicated requirements of pharmacopoeial monographs.

A

QUALITY CONTROL

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7
Q

Quality control guarantees within resonance limits that a drug product:

A
  • Is free of impurities.
  • Is physically and chemically stable.
  • Contains the amount of active ingredients as stated on the label.
  • Provides optimal release of active ingredients when the product is administered.
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8
Q

REFERENCE BOOKS ON DRUG STANDARDS

A

British Pharmacopoeia
United States Pharmacopoeia
National Formulary
Homeopathic Pharmacopoeia of the United States
International Pharmacopoeia

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9
Q

From Great Britain

Product of merging by the 3 cities’ pharmacopoeia of London, Edinburgh, and Dublin in 1864

A

British Pharmacopoeia

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10
Q

1st American Pharmacopoeia, 1778

A

Lititz pharmacopoeia

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11
Q

Suggested to the medical society of NY the pharmacopoeia.

Father of USP

A

Dr. Lyman Spalding (January 6, 1817)

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12
Q

Exclusive for doctors, held every 10 years (revise USP)

In 1940, pharmacies invited and revised and updated USP every 5 years.

A

USP convention

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13
Q

Used to be a revolt/rebellious records coined as the NF of the unofficial preparations.

June 30, 1906: changed to National Formulary

A

National Formulary

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14
Q

Declared USP & NF as standards for medicinal and pharmaceutical substances.

A

President Theodore Roosevelt

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15
Q

Coined by Samuel Hahnemann

Principle: like cures like or the law of similarities (vaccines/immunizations)

A

Homeopathic Pharmacopoeia of the United States

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16
Q

Homeopathic Pharmacopoeia of the United States is coined by

A

Samuel Hahnemann

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17
Q

Published by WHO

Recommendation to national pharmacopoeia revisions

A

International Pharmacopoeia

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18
Q

First American pharmacopoeia, Lititz Pharmacopoeia, was published for use by the military hospital of the United States Army

A

1778

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19
Q

Massachusetts Medical Society published a 272-page pharmacopoeia containing information on monographs on 536 drugs and pharmaceutical preparations.

A

1808

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20
Q

Lyman Spalding submitted a plan to the medical society of the country of New York for the creation of national pharmacopoeia. He was recognized as the father of USP.

A

January 6, 1817 (submitted)

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21
Q

Draft pharmacopoeias were reviewed, consolidated, and adopted by the 1st USP convention assembled in Washington, DC.

A

January 1, 1820 (reviewed, consolidated, adopted)

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22
Q

The first USP was published in English and Latin.

A

December 15, 1820 (published)

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23
Q

The first edition of the National Formulary of unofficial preparations was published.

A

1888

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24
Q

The pharmacopoeial convention granted authority to issue supplements to the USP to maintain satisfactory standards.

A

1900

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25
Q

The title National Formulary of Unofficial Preparations was changed to National Formulary (NF).

President Roosevelt signed into law the First Federal Pure Food and Drug Act, designating both the USP and NF as establishing legal standards for medicinal and pharmaceutical substances.

A

June 30, 1906

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26
Q

Convention decided to revise the USP every 5 years while maintaining the use of periodic supplements. The NF was revised every 10 years.

A

1940

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27
Q

The USP Convention Inc. purchased the NF, unifying the unofficial compendia and providing the mechanism for a single national compendium.

A

1975

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28
Q

The first combined compendium, compromising the USP XX and NF XV, became official.

A

July 1, 1980

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29
Q

The USP 23 – National Formulary 18 was the first edition to drop the use of Roman numerals, in favor of Arabic numerals to indicate the edition.

A

1995

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30
Q

The USP-NF became an annual publication.

A

2002

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31
Q

METHODS OF ANALYSIS

A
  1. Volumetric Analysis
  2. Physicochemical Analysis
  3. Gravimetric Analysis
  4. Special Methods
32
Q

Determination of the volume of a solution of known concentration required to react with a given amount of the substance to be analyzed.

A

Volumetric Analysis

33
Q

Based on some physical or chemical property/properties of the substance being analyzed.

A

Physicochemical Analysis

34
Q

Employ instrumental techniques of physicochemical analysis

A

o Cinematographic
o Spectrophotometric
o Electrometric
o Thermal conductimetric
o Refractometric
o polarimetric

35
Q

Separation by extraction, precipitation, and other means of the constituent to be determined either in the natural state or in the form of definite compound the composition and of which is known to the analyst, and the weighing of the resulting product.

A

Gravimetric Analysis

36
Q

Those which requires a distinct type of technique.

Ex: alkaloid assaying, saponification value, acid value

A

Special Methods

37
Q

Used to denote the agreement of an experimental result or the agreement of the mean value of the experimental results with the hue value.

A

ACCURACY

38
Q

Measure of reproducibility of date within a series of results.

A

PRECISION

39
Q

The discrepancies in the results are caused by various sources of error to which all experimental data are subject.

A

Source and Nature of Errors

40
Q

2 types of errors

A

Indeterminate errors
Determinate errors

41
Q

Manifest themselves by slight variations in a series of observations made by the same observer under identical conditions.

Causes are difficult to detect such as the differences in the judgement and the skill of the analyst.

Indeterminate errors are intangible, and their elimination by the analyst is impossible.

A

Indeterminate Errors

42
Q

Nature that occurs in constant manner in each series of determinations.

usually detectable and so may be eliminated

Arise from causes such as:
- Personal error made by the analyst (ex. Inability to judge color changes sharply).

  • Errors of method caused by faulty procedure (ex. Incorrect sampling, contamination of precipitates, and improper selection of indicators).
  • Apparatus errors due to poor construction or calibration (ex. Inaccuracy in the calibration of burets or pipets, inequality in the length of the arms of the balance and incorrect weights).
A

Determinate Errors

43
Q

_______ and __________ burets are used to deliver accurate volumes of solutions in titrations.

A

Geissler (Acid)
Mohr (Base)

44
Q

Prior to use, burets are cleaned with detergent solutions followed by rinsing with distilled water and finally, with __________ of the solution to be measured.

A

three times 5-mL portion

45
Q

TITRATION SET-UP

A
  • Geissler (Acid) Buret
  • Mohr (Base) Buret
  • Buret Clamp
  • Iron Stand
  • Erlenmeyer Flask
46
Q

chemical substance being analyzed.

A

analyte or active constituent

47
Q

solution of known concentration

A

titrant

48
Q

slow addition of one solution of a known concentration (called a titrant) to a known volume of another solution of unknown concentration until the reaction reaches neutralization, which is often indicated by a color change.

A

titration

49
Q

Theoretical point at which equivalent amounts of analyte and titrant have reacted.

A

EQUIVALENCE POINT or STOICHIOMETRIC POINT

50
Q

Point at which there occurs a sudden change in some property of the reaction mixture.

A

END POINT

51
Q

Determination of the normality or molarity of a solution.

A

STANDARDIZATION

52
Q

Concentration expression and defined as the number of equivalents of solute per liter or milliequivalents per milliliter of a solution.

A

NORMALITY

53
Q

An expression of the concentration of a solution in terms of moles per liter.

A

MOLARITY

54
Q

Solution of known normality or molarity.

A

STANDARD SOLUTION

55
Q

A highly purified – about 99.99% (ultrapure) compound that serves as reference material in titration.

A

PRIMARY STANDARD

56
Q

A compound whose purity (97-98%) has been established by careful chemical analysis.

A

SECONDARY STANDARD

57
Q

Sometimes it is necessary to add an excess of the standard titrant and the excess amount is titrated with a second standard titrant.

A

BACK TITRATION

58
Q

The difference in volume and mass between the end point and equivalence point.

A

TITRATION ERROR

59
Q

Chemical which changes color at or very near the equivalence point.

Indicators are also very weak acids and bases.

o In acidic conditions, the color of the acid forms (HlN) predominates.

o In alkaline conditions, the color of conjugate base (lN) predominates.

A

INDICATOR

60
Q

complex compounds used

  1. To determine the end point in neutralization process.
  2. To determine hydrogen ion concentration (H+) of pH.
  3. To indicate that a desired change in pH has been affected.
A

indicator

61
Q

thymol blue

A

Red Yellow 1.2 – 2.8

62
Q

bromophenol blue

A

Yellow Violet 3.0 – 4.6

63
Q

methyl orange

A

Orange Yellow 3.1 – 4.4

64
Q

methyl red

A

Red Yellow 4.2 – 6.3

65
Q

chlorophenol blue

A

Yellow Blue 4.8 – 6.4

66
Q

bromothymol blue

A

Yellow Blue 6.0 – 7.6

67
Q

cresol red

A

Yellow Red 7.2 – 8.8

68
Q

phenolphthalein

A

Colorless Red 8.3 – 10.0

69
Q

TYPES OF TITRATIONS

A
  1. DIRECT TITRATIONS
  2. RESIDUAL (BACK TITRATION)
  3. INDIRECT TITRATION
    * Blank Titration
70
Q

Direct addition of a titrant to analyte.

A
  1. DIRECT TITRATIONS
71
Q

Adding excess amount of acid to a base to quantify with base.

A
  1. RESIDUAL (BACK TITRATION)
72
Q

Needs to perform pre-treatment before titration.

A
  1. INDIRECT TITRATION
73
Q

correcting errors, repeating the assay without the analyte.

A
  • Blank Titration
74
Q

Chemical processes in which an acid (proton donor) reacts with a base (proton acceptor), the product of a neutralization reaction in aqueous solution are water and salt.

A

neutralization reactions

75
Q

2 types of titrations

A

Alkalimetry - BASE
Acidimetry - ACID

76
Q
A

PH 105.1 (1 decks)

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