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Quantitative Analysis > Quant Final Exam > Flashcards

Quant Final Exam Flashcards

1
Q

what; process of determining the identity of the constituents of a substance

A

Qualitative

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2
Q

how much; process of measuring how much of a constituent is present in a substance

A

Quantitative

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3
Q

substance being measured or detected; also called measurand

A

Analyte

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4
Q

a solution whose composition is known by virtue of the way that it was made from a reagent of known purity or by virtue of its reaction with a known quantity of a standard reagent

A

Standard Solution

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5
Q

liquid remaining above the solid after a precipitation

A

Supernatant

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6
Q

portion

A

Aliquot

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7
Q

a solution of anything in water

A

Aqueous

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8
Q

a suspension of a solid in a solvent

A

Slurry

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9
Q

to pour liquid off a solid or, perhaps, a denser liquid; the denser phase is left behind

A

Decant

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10
Q

General Steps in Chemical Analysis:
Step One

A

formulating the question (translating questions into specific questions)

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11
Q

General Steps in Chemical Analysis:
Step Two

A

selecting analytical procedures (literature search)

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12
Q

General Steps in Chemical Analysis:
Step Three

A

sampling (selecting representative materials)

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13
Q

General Steps in Chemical Analysis:
Step Four

A

sample preparation (converting sample into suitable form)

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14
Q

General Steps in Chemical Analysis:
Step Five

A

analysis (repeated measurements, applying different analytical methods if possible)

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15
Q

General Steps in Chemical Analysis:
Step Six

A

reporting and interpretation

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16
Q

General Steps in Chemical Analysis:
Step Seven

A

drawing conclusions

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17
Q

Avogadro’s Number

A

6.022E23

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18
Q

Molarity Formula

A

moles solute / liters solution

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19
Q

Molality Formula

A

moles solute / kilograms solvent

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20
Q

If the mobile phase is polar, which sample elutes first? The polar or nonpolar sample?

A

polar

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21
Q

Which elutes first in a cathode? Anions or cations?

A

anions

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22
Q

Weight Percent Formula

A

(mass solute / mass solution) x 100

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23
Q

Part Per Million Formula

A

(mass solute / mass solution) x 10E6

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24
Q

Part Per Billion Formula

A

(mass solute / mass solution) x 10E9

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25
Q

Dilution Formula

A

M1V1 = M2V2 (or C1V1 = C2V2)

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26
Q

Dilution Factor

A

sample volume / total volume

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27
Q

chemical analysis based on weighing a final product

A

Gravimetric Analysis

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28
Q

In addition and subtraction, how is the number of significant figures determined?

A

the last sig fig is determined by the number with the fewest decimal places
(EX: 5.3 + 16.41 = 21.7)

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29
Q

In multiplication and division, how is the number of significant figures determined?

A

the number with the fewest sig figs determines the number of sig figs in the final answer
(EX: 6.3 x 2.761 = 17)

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30
Q

In logarithms, how is the number of significant figures determined?

A

the number of significant figures in the final answer is equal to the number of sig figs in the mantissa
(EX: log(339) = 2.530 ; 10 ^ 2.530 = 339)
(NOTE: sig figs begin after the decimal; antilog is the opposite)

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31
Q

built-in error, consistent, and reproducible; in principle, detectable and correctable
(EX: improperly standardized balance, incorrectly prepared standard solutions)

A

Systematic Error

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32
Q

error from uncontrollable variables in the measurement; inconsistent error value; can be reduced by repeated trials but cannot be completely eliminated
(NOTE: sometimes expressed as standard deviation)

A

Random Error

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33
Q

how close a measurement is to the true/accepted value; nearness to the truth

A

Accuracy

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34
Q

how close together a set of measurements are; reproducibility

A

Precision

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35
Q

Relative Uncertainty Formula

A

absolute uncertainty / magnitude of measurement

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36
Q

Percent Relative Uncertainty Formula

A

relative uncertainty x 100

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37
Q

the actual amount by which a quantity is uncertain; usually given in parentheses by the given measurements

A

Absolute Uncertainty

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38
Q

Propagation of Error for Addition and Subtraction

A

e = sqrt( (e1)^2 + (e2)^2 + (e3)^2 )

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39
Q

Propagation of Error for Multiplication and Division

A

%e = sqrt( (%e1)^2 + (%e2)^2 + (%e3)^2 )

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40
Q

Which test compares mean values? F-Test or t-Test?

A

t-Test

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41
Q

Which test compares standard deviations? F-Test or t-Test?

A

F-Test

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42
Q

When does precipitation occur?

A

Q > Ksp

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43
Q

Equilibrium Constant Formula (K)

A

[products] / [reactants]
(NOTE: don’t forget the stoichiometric exponents when applicable)

44
Q

Equilibrium Constant for Reversed Reactions

A

K’ = 1 / K

45
Q

Equilibrium Constant for Added Reactions

A

K = K1 x K2

46
Q

When is a reaction favored?

A

K > 1 ; G is negative

47
Q

What does negative enthalpy mean?

A

exothermic

48
Q

What does positive enthalpy mean?

A

endothermic

49
Q

What does positive entropy mean?

A

products have greater entropy than reactants

50
Q

What does negative entropy mean?

A

reactants have greater entropy than products

51
Q

When is a reaction disfavored?

A

K < 1 ; G is positive

52
Q

What does negative G mean?

A

a spontaneous reaction

53
Q

What does positive G mean?

A

not a spontaneous reaction

54
Q

if a system at equilibrium is disturbed, the direction in which it proceeds back to equilibrium is such that the disturbance is offset

A

Le Chatelier’s Principle

55
Q

the equilibrium constant for the reaction in which a solid salt dissolves to give its constituent ions in solution

A

Solubility Product (Ksp)

56
Q

a salt is less soluble if one of its constituent ions is already present in the solution

A

Common Ion Effect

57
Q

When Q > K what direction will the reaction proceed?

A

Left

58
Q

When Q < K what direction will the reaction proceed?

A

Right

59
Q

electron pair acceptor

A

Lewis Acid

60
Q

electron pair donor

A

Lewis Base

61
Q

When ionic strength increases, what happens to the activity coefficient?

A

Decreases

62
Q

When ion charge increases, what happens to the activity coefficient?

A

Decreases

63
Q

When ion size increases, what happens to the activity coefficient?

A

Increases

64
Q

Ionic Strength Formula (mu)

A

(1/2) x SUM( C1(Z1)^2 + C2(Z2)^2… )

65
Q

True or False: Strong acids/bases dissociate completely.

A

True

66
Q

True or False: Weak acids/bases only partially dissociate.

A

True

67
Q

True or False: A stronger acid (HA) means a weaker conjugate base (A-).

A

True

68
Q

Which equation do you use to find the pH of a buffer zone?

A

Henderson-Hasselbach

69
Q

procedure for the analysis of nitrogen in organic compounds

A

Kjeldahl Nitrogen Analysis

70
Q

use to standardize the acid/base titrant in a titration

A

Primary Standards
(EX: KHP standardization of NaOH)

71
Q

True or False: At 1/2 Ve1, pH = pKa2.

A

True

72
Q

True or False: At 1/2 Ve2, pH = pKa1.

A

True

73
Q

when moles of H+ equals moles of OH-

A

Equivalence Point

74
Q

True or False: EDTA has a 1:1 stoichiometric ratio with any metal complex.

A

True

75
Q

What are the different types of EDTA titrations?

A

Direct, Indirect, Back, Masking, Displacement

76
Q

a species used to stabilize a metal ion and keep that metal in solution; binds loosely enough to be displaced by a titrant

A

Auxiliary Complexing Agent

77
Q

solute equilibrates between the mobile phase and sites on the surface of the stationary phase

A

Adsorption Chromatography
(NOTE: stronger adsorption means slower movement)

78
Q

different sized solutes penetrate pores in the stationary phase to different extents; larger solutes elute first

A

Size/Molecular Exclusion Chromatography

79
Q

ions in the mobile phase are attracted to counterions covalently attached to the stationary phase

A

Ion-Exchange Chromatography

80
Q

solute in the mobile phase is attracted to specific groups covalently attached to the stationary phase

A

Affinity Chromatography

81
Q

solute equilibrates between the mobile phase and a film of liquid attached to the stationary phase

A

Partition Chromatography

82
Q

What does A represent in the van Deemter equation?

A

Multiple Flow Paths/Eddy Diffusion

83
Q

What does B/ux represent in the van Deemter equation?

A

Longitudinal Diffusion

84
Q

What does Cux represent in the van Deemter equation?

A

Mass Transfer

85
Q

a form of chromatography in which the mobile phase is a gas

A

Gas Chromatography

86
Q

What do narrower columns mean?

A

higher resolution, shorter analysis time, greater sensitivity, lower sample capacity, higher pressure

87
Q

What happens as film thickness increases?

A

retention time increases, resolution increases, bleeding increases

88
Q

a device that detects substances eluted from a gas chromatography column by measuring changes in the thermal conductivity of the gas stream

A

Thermal Conductivity Detector

89
Q

a detector in which solute is burned in a mixture of H2 and air to produce CHO+ ions and electrons in the flame

A

Flame Ionization Detector

90
Q

a detector that is particularly sensitive to compounds with halogen atoms, nitro groups, and other groups with high electron affinity; high electron affinity analytes capture some of the electrons and reduce the detector current

A

Electron Capture Detector

91
Q

True or False: When concerning the stationary phase, like dissolves like.

A

True

92
Q

What do smaller particle sizes mean?

A

a larger number of theoretical plates

93
Q

a chromatographic technique using very small stationary phase particles and high pressure to force solvent through the column

A

High-Performance Liquid Chromatography (HPLC)

94
Q

Formula for E(cell)

A

E(cell) = E(cathode) - E(anode)

95
Q

Where does oxidation occur?

A

Anode

96
Q

Where does reduction occur?

A

Cathode

97
Q

When is a cell galvanic/voltaic?

A

when E(cell) > 0 or positive; means spontaneous

98
Q

Absorption Spectrophotometer

A

light source > monochromator > sample > detector

99
Q

Emission Spectrophotometer

A

light source > monochromator > sample >
monochromator > detector

100
Q

Radiation Energy Transition Types:
Microwave

A

Rotational

101
Q

Radiation Energy Transition Types:
Infrared

A

Vibrational

102
Q

Radiation Energy Transition Types:
UV/VIS

A

Electronic

103
Q

Radiation Energy Transition Types:
X-Ray

A

Bond Breaking and Ionization

104
Q

Polymer Goals

A

purification, molecular weight, monomer/polymer ratio, rigidity, thermal stability, toxicity analysis

105
Q

Polymer Challenges

A

inhomogeneous properties, high viscosity, soluble only in organic solvent

106
Q

methods used in polymer analysis

A

FTIR, Raman, UV/VIS, NMR, Gel Permeation Chromatography, Mass Spectroscopy, Thermal Gravimetric Analysis, Differential Scanning Calorimetry, Dynamic Light Scattering

Quantitative Analysis (3 decks)

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