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Quantitative Analysis > Finals Review > Flashcards

Finals Review Flashcards

1
Q

Mass

A

Force required for acceleration

Independent of distance to earth center

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2
Q

Molarity

A

1 molar solution contains one mole of solute in one liter solution

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3
Q

Formality

A

One formal solution contains one FW of solute in 1 liter of solution

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4
Q

Normality

A

1 normal solution contains 1 equivalent weight of solute per liter of solution

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5
Q

Significant figures

A

Number of digits needed to express a result consistent with given or measured precision

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6
Q

Accuracy

A

Agreement between measured and true or accepted values

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7
Q

Precision

A

Reproducibility between replicate measurements

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8
Q

Determinable

A

Can be avoided or corrected. Also called systematic errors

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9
Q

Mass balance equation

A

For particular type of species. The sum of the added amounts must be equal to the s of all possible forms existing in the system

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10
Q

Colloidal precipitates

A

Small particles (1-100 nm), Tyndall effect

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11
Q

Crystalline precipitates

A

Diameter of negligible inches. Most desirable for analysis

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12
Q

Nuclear ion

A

Small aggregates form.

The formation of minimum size stable precipitate

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13
Q

Particle growth

A

Additional molecules deposit on growth nucleus

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14
Q

Supersaturation

A

SS

solution that contains more solute than would be present at equilibrium, which leads to precipitate formation

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15
Q

Weight

A

Attraction of earth

Distance to center of earth important

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16
Q

Titration

A

Determination by unknown reaction or reagent

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17
Q

End point

A

Empirical approximation of equivalence point

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18
Q

Indicator

A

Provides visual determination of end point

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19
Q

Back titration

A

End point is intentionally exceeded, then the excess titrant is titrated
Useful when forward end point is difficult to see
Useful when complete reaction is difficult to achieve

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20
Q

Volthard method

A

Excess Ag+ added to remove all X-

Excess Ag+ is back titrated with SCN- when all Ag+ is removed, SCN- reacts with Fe3+

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21
Q

Fabians method

A

Precipitate formed before equivalence point. Will have slight negative change due to adsorbed X-
After equivalence point, precipitate particles will have a slight positive charge due to adsorbed Ag+
Anionic dyes will be attracted to positively charged particles to form colored adsorbents

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22
Q

Kjeldahl procedure

A

Determine Nitrogen in biological samples

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23
Q

Buffers

A

Resistant to pH change due to moderate additions of H+ or OH-

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24
Q

Buffer capacity

A

Number of miles of strong acid or base that must be added to the buffer solution to change pH by 1 unit

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25
Polyprotic acids
Acids that can furnish more than one proton. They are weak acids Ka values associated with each proton loss
26
Principal species
Must be abundant solution species. | HA at low pH, A- at higher pH
27
Gran plot
Function derived from equilibrium expression before equivalence point
28
Ligand
Substance that acts as a Lewis base and furnishes electrons to a metal ion to form a complex.
29
Coordinate number
Number of bonds formed by the metal ion in a complex
30
Coordination geometry
Necessary orientation of ligand for complex formation
31
Unidented ligand
Ligand that can provide one electron lone pair in a complex. Eg NH3
32
Bidentate ligand
Ligand that can provide two election lone pairs in a complex
33
Chelating ligand
Multidented ligand that attaches to the metal ion through more than one atom
34
Direct titration
Chelates react with metal ion directly
35
Replacement titration
Metal ion displaces a different ion
36
Indirect titration
First, precipitate anion with excess metal ion, then titrate remaining metal ion with chelate
37
Water harness
Capacity of cations in water to replace sodium and potassium in soaps to form sparingly soluble products
38
Photon
Packet of light
39
I (intensity)
Power per unit solid angle
40
Power
Energy per second
41
Concentration polarization
Reaction concentration at electrode is less than in the bulk solution
42
Dissolution
Completely dissolve in a known amount of solvent
43
Singlet
All electrons are paired, no splitting observed in magnetic field. Diamagnetic
44
Triplet
Two electrons are unpaired, shows anomalous zee man effect in a magnetic field. Splitting degenerates energy states into 3 distinct states (paramagnetic)
45
Absorption
Radiation imparts energy to material and promotes it from ground state to excited state
46
Emission
Radiation produced as material relaxes from excited to lower energy state
47
``` Ion selective (membrane) (Indicator electrode) ```
Responds to salute by means of boundary potential development across a membrane
48
Inert metal | Indicator electrode
Eg Pt, Au Provides contact between the external circuit and solution but does not participate in reaction except to conduct electrodes
49
Reference electrode
Electrode of a half cell that never changes | Has constant potential
50
Dry ashing
Combustion of solid samples
51
Wet ashing
Combustion in the presence of a liquid
52
Standardization
Process used to determine the concentration of a secondary standard
53
Isosbestic point
If there are wavelengths at which molar absorptive Tunis the same for each form, the absorbance at that wavelengths will be constant for mixtures when the total number (formality) is fixed. (For substances with multiple solution forms having different absorption points)
54
Potentiometry
Determining the activity (concentration) of a given ion by measuring potential of working/indicator electrode relative to that of reference electrode
55
Electroactive species
Substance that can be oxidized or reduced and is therefore a participant in an electrode half reaction
56
Indicator electrode
Electrons present in the half cell that contains the electro active species
57
Oh mic potential
Voltage required to overcome electrical resistance
58
Overpotential
Voltage required to overcome the activation energy for electrode reaction
59
Oxidation
Process of releasing electrons, forms in more positive ion
60
Reduction
Process of gaining electrons
61
Oxidation agent
Causes oxidation to occur, agent is reduced in the process | i.e it is the thing that gets reduced
62
Reducing agent
Causes reduction to occur, agent is oxidized in the process i.e the thing that gets oxidized
63
Anode
Electrode at which oxidation occurs | Pt electrode dipping into Fe2+ solution
64
Cathode
Electrode at which reduction occurs | C electrode dipping into Ce4+ solution
65
Standard reduction potential
Under standard conditions, potential difference between a half cell and SHE. The given half cell reaction is always represented as a reduction process (SHE always at anode)
66
Detection limit
Smallest response that can be distinguished from background noise Quantity required to provide a signal to noise ratio of 2:1 or 3:1
67
Supercritical fluid extraction
Supercritical CO2 used as a solvent for extraction
68
Solid-Phase extraction (SPE)
Removal of an analyte from solution by selective and strong interactions with a solid material
69
Fraction removal
Fraction of analyte removed after "n" successive extractions with the same amount of solvent
70
Zwitterton
Molecules with both a positive and negative charge
71
Speciation
Distribution of analyte among species
72
Isoionic pH
PH of pure, neutral, polyprotic acid
73
Isoelectric pH
pH at which average charge of polyprotic acid is 0
74
Metal ion indicators
Compounds that change color when they bind to a metal
75
Common ion effect
A salt will be less soluble if one of its constituent ions is already present in solution
76
Coprecipitation
When a substance whose solubility exceeded precipitates along with another substance whose solubility is exceeded
77
Fugacity
Activity of a gas
78
Nucleation
Diluted form a disorganized cluster of sufficient size, which reorganizes into an ordered structure capable of growing into larger particles

Quantitative Analysis (2 decks)

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