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Physical and Chemical Principles > Analytical Chemistry > Flashcards

Analytical Chemistry Flashcards

1
Q

A branch of chemistry that deals with the separation, identification and composition of matter

A

Analytical chemistry

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2
Q

Type of analysis that reveals the components of the sample

A

Qualitative analysis

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3
Q

Type of analysis that determines the amount of components present in a sample

A

Quantitative analysis

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4
Q

Two types of classical methods of analysis

A

Gravimetric Method

Volumetric Method

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5
Q

It deals with the measurement of the mass of a substance that is chemically related to the analyze

A

Gravimetric method of analysis

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6
Q

It measures the volume of solution necessary to react completely with the analyze

A

Volumetric method of analysis

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7
Q

Two types of modern method of analysis

A

Spectroscopic Method

Electroanalytic Method

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8
Q

It measures the electromagnetic radiation produced by the analyze or its interactions with it

A

Spectroscopic Method

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9
Q

It measures the electrical properties of the analyte such as current, potential, resistance and amount of charge

A

Electroanalytic Method

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10
Q

This factor is used to calculate the percentage of analyte in sample

A

Gravimetric Factor

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11
Q

A solution of known concentration is called

A

Standard solution

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12
Q

A process of determining the concentration of an unknown solution

A

Standardization

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13
Q

A substance of high purity used for standardization

A

Primary standard

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14
Q

Characteristics of a good primary standard

A

High purity
High equivalent weight
Stable - high temperature and humidity
Soluble in water

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15
Q

Types of titration

A

Direct
Back
Replacement

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16
Q

A type of titration where analyte reacts with the standard solution direct

A

Direct titration

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17
Q

A type of titration where an excess standard solution is added and the excess is determined by the addition of another standard solution

A

Back titration

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18
Q

A type of titration where the analyte is converted to sprout chemically related to it and the product of such is titration with a standard solution

A

Replacement titration

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19
Q

An acid is a proton donor according to

A

Bronsted-Lowry Theory

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20
Q

An acid in an electron-pair acceptor according to

A

Lewis

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21
Q

An acid produces hydronium ion in solution according to

A

Arrhenius

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22
Q

A base is an electron pair donor according to

A

Lewis

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23
Q

A base produces hydroxide ion according to

A

Arrhenius

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24
Q

An base is an proton acceptor according to

A

Bronsted-Lowry

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25
Q

Hydronium ion is also called

A

Protonated water

Solvated proton

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26
Q

This reaction involves formation of ions

A

Ionization reaction

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27
Q

This type of acids or bases completely ionize in solution

A

Strong acids and strong bases

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28
Q

This type of acids and bases partially ionize in solution

A

Weak acids and bases

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29
Q

These are strong acids (only on the first ionization) - 6

A 
Hydrochloric
Hydrobromic 
Hydroiodic 
Perchloric 
Nitric
Sulfuric
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30
Q

Common examples of strong bases

A

Bases of 1A and 2A

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31
Q

Common examples of weak acids -5

A 
Hydrofluoric
Hydrocyanic 
Sulfurous 
Phosphoric
Organic acids
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32
Q

A common example of a weak base

A

Ammonia and its derivatives

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33
Q

A general rule suggest that salts coming a — acids or bases hydrolysis in water, only the conjugate hydrolyzes in water

A

Weak

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34
Q

It is formed from the reaction of a strong acid and weak base

A

Acidic salt

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35
Q

It is formed from the reaction of a strong base and weak acid

A

Basic salt

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36
Q

It is a product of the reaction between a strong acid and a strong base

A

Neutral salt

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37
Q

These are solutions that contain weak acid or weak base and its conjugate salt. These tend to edit the changes in pH

A

Buffer solutions

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38
Q

5 primary standards for bases

A 
Benzoic acid
Oxalis acid
Potassium biiodate
Potassium hydrogen phthalate
Sulfamic acid
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39
Q

Chemical formula for benzoic acid

A

C6H5COOH

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40
Q

Chemical formulas for oxalis acid

A

H2C2O4.2H2O

41
Q

Chemical formula for potassium biiodate

A

KH(IO3)2

42
Q

Chemical Formula for KHP

A

KC8H5O4

43
Q

Chemical formula for sulfamic acid

A

HSO3NH2

44
Q

Primary standard for acids

A

Calcium carbonate
Mercuric oxide
Sodium carbonate
Tris-hydroxymethylaminomethane

45
Q

The presence of hydroxide, carbonate and bicarbonate in water is also referred to as

A

Alkalinity

46
Q

It is the measure of acid-neutralizing capacity of water

A

Alkalinity

47
Q

This analytical technique I’d one of the oldest. It started in the mid-1800’s

A

Precipitation titration

48
Q

In the precipitation titration, — is commonly employed

A

Silver nitrate

49
Q

The term called for the titration with AgNO3

A

Argentometric titration

50
Q

Indicators in Precipitimetry are the formation of (3)

A

Colored secondary precipitate
Colored complexion
Colored adsorption complex

51
Q

The formation of a colored secondary precipitate is seen in this method of Precipitimetry

A

Mohr Method

52
Q

This is a direct method for halides and cyanides

A

Mohr Method

53
Q

The indicator used in Mohr Method is

A

Sodium chromate

54
Q

The formation of a colored complexion is seen in this method

A

Volhard Method

55
Q

This is a direct method for silver and an indirect method for halides

A

Volhard Method

56
Q

The indicator used in Volhard Method is

A

Ferric alum

57
Q

The formation of a colored adsorption complex is seen in what method

A

Fajans Method

58
Q

This indicator is used in Fajans Method, which is also best for the determination of halides and cyanides

A

Dichlorofluorescin

59
Q

A titration method carries spout in an acidic condition

A

Volhard Method

60
Q

A titration carried out between pH 7-10

A

Mohr Method

61
Q

A titration carried out between pH 4-7

A

Fajans Method

62
Q

This type of titration is used for the determination of cation

A

Complex formation titration

63
Q

This is a method of determination of cyanide which is carried by the drop wise addition of silver nitrate solution of a cyanide forming a soluble cyanide complex of silver

A

Liebig Method

64
Q

The determination of nickel is by treating an — with a measured excess standard cyanide solution and the excess is determined by a standard silver nitrate solution

A

Ammoniacal solution of nickel

65
Q

EDTA stands for

A

Ethyldiaminetetraacetic acid

66
Q

The structure of EDTA suggests 6 potential sites for metal bonding: 4 carbonyl groups and 2 amino acid groups. Therefore edta is

A

Hexadentate

67
Q

The indicator used for titration with EDTA is

A

Eriochrome black T

68
Q

This reaction involves the transfer of electrons from one reactant to another

A

Redox

69
Q

It involves an increase in the oxidation state of an element

A

Oxidation reaction

70
Q

It involves a decrease in the oxidation state

A

Reduction reaction

71
Q

These type of cells have two electrodes which are immersed in an electrolyte solution

A

Electrochemical cells

72
Q

This is used to prevent the two solutions from mixing

A

Salt bridges

73
Q

The electrode where reduction occurs is

A

Cathode

74
Q

An electrode where oxidation occurs is

A

Anode

75
Q

An electrochemical cell that stores electrical energy

A

Galvanic cell

76
Q

galvanic cell is also called

A

Voltaic cell

77
Q

In this type of cell, the reaction at the anode and the cathode occurs spontaneously and allows flow of electrons from the anode to the cathode with the aid of an external conductor

A

Galvanic cell

78
Q

It is the potential of a cell with the hydrogen electrode as the anod

A

Electrode potential

79
Q

It is assigned a value of 0.000V at all temperatures

A

Standard hydrogen electrode

80
Q

It is the electrode potential when the activities of all reactants and products are unity

A

Standard electrode potential of a half reaction

81
Q

A positive value of the standard reduction potential implies that it was used as a cathode with the

A

She as anode

82
Q

High positive value of a reduction potential also indicate that the electrode in a good

A

Oxidizing agent

83
Q

Redox titration 3

A

Permanganate Process
Dichromate Process
Iodometric Titration

84
Q

A type of agent that contains two or more groups capable of competing with a metal ion

A

Chelating agent

85
Q

The endpoint for this titration method is the formation of a permanent faint turbidity

A

Liebig Method

86
Q

Silver to cyanide ratio for Liebig Method

A

2:1

87
Q

Analytical methods classified as micro analyses use sample mass ranging from

A

1-10 mg

88
Q

Chemicals which are tested by the manufacturers showing the actual percentages of impurities and labeled on the containers are

A

Reagent grade chemicals

89
Q

Other terms for reagent grade chemicals are

A

Analytical reagent

Certified reagent

90
Q

This can’t be done with platinum crucibles since it would cause a significant loss of analyte

A

Heating with sulfide a

91
Q

This grade of water is defined to be suitable for the determination of trace quantities which can be prepared by the distillation of deionized water

A

Grade 2

92
Q

The grade 2 water for the determination of trace quantities is defined by the

A

British standard 3978

93
Q

It is expressed as the volume of a solution chemically equivalent to a mass of a solid reagent

A

Tiger

94
Q

A process by which an agglomerate colloid return to its dispersed state during washing due to leaching of electrolyte responsible for its coagulation

A

Peptization

95
Q

The best indicator for the titration of a weak acid and a strong base

A

Phenolphthalein

96
Q

Why is it necessary to carry out titration in acidic solution in the Volhard Method

A

To prevent precipitation of iron as hydrated oxide

97
Q

This step is necessary before titration when an analyte in a sample is present in two different oxidation states

A

Prereduction

98
Q

This is the term used for the metallic reductions which is soaked in a dilute solution of mercuric chloride

A

Lindlars catalyst

Physical and Chemical Principles (6 decks)

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