ANALYTICAL CHEMISTRY > Electroanalytical Methods > Flashcards

Electroanalytical Methods Flashcards

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1
Q

A technique that uses direct electric current to drive non-spontaneous chemical reaction.

A

Electrolysis

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2
Q

Industrial method for producing sodium hydroxide (Caustic soda) by electrolyzing brine, yielding NaOH, chlorine gas and hydrogen gas.

A

Chlor-alkali Process

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3
Q

Widely used to study the electrical properties os chemical reactions and systems.
Rely on measuring the various electrochemical parameters to gain insight to concentration, activity and behavior of chemical reaction.

A

Electroanalytical Methods

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4
Q

The measure of standard potential of an electrochemical half-cell under standard conditions: 1M, 25C, 1 atm.

A

Half-cell Potential (Eº)

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5
Q

The potential of an electrode with respect to a reference electrode, often measured at equilibrium.

A

Electrode Potential (E)

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6
Q

The concentration of a specific ion of species in a solution.

A

Concentration (C) express in Molarity

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7
Q

The ratio of concentrations of products to reactants at any point in a reaction.

A

Reaction Quotient (Q)

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8
Q

The effective concentration of a species in a solution, accounting for the interactions with other ions.

A

Activity (A)

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9
Q

The total amount of electric charge passed through the system during a reaction or titration.

A

Charge (Q)

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10
Q

The flow of electric charge through a circuit.

A

Current (I)

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11
Q

The current related to the electrochemical reaction (due to electron transfer) at an electrode.

A

Faradaic Current

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12
Q

The current due to double-layer charging or the other non-electrochemical processes at the electrode.

A

Non-Faradaic Current

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13
Q

The maximum current observed in a voltammetric experiment, often used to determine the analyte’s concentration.

A

Peak Current

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14
Q

The potential at which the current reaches half of its maximum in a voltammetric experiment.

A

Half-Wave Potential

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15
Q

The volume of titrant required to reach the equivalence point or endpoint in titration methods.

A

End Point

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16
Q

Most commonly used electroanalytical method at which it rely on phenomena occurring at the interface between measuring an electrode and the solution, in conjunction with a reference electrode.

A

Interfacial Method

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17
Q

Two classification of Interfacial Methods

A

Static
Dynamic

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18
Q

This classification involves no significant current flow, such as potentiometry.

A

Static

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19
Q

This classification involves measuring a variable such as current under controlled potential conditions, like voltammetry and amperometry.

A

Dynamic

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20
Q

This is a static method at which it measures the potential without significant current flow, used for the measurement of pH or ion concentration.

A

Potentiometry

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21
Q

A dynamic method at which it measures the current as a function of applied potential, used for studying redox reactions.

A

Voltammetry

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22
Q

A dynamic method wherein it measures the current at a fixed potential, used for the detection of glucose in biosensors.

A

Amperometry

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23
Q

This measures the total charge passed in a reaction, typically used in titration of ions with known amount of electricity.

A

Colourimetry

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24
Q

This measures the electrical conductivity of a solution, used in monitoring of ion concentration and reaction progress.

A

Conductormetry

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25
Provides a stable and known potential against which the potential of the measuring electrode can be measured.
Reference Electrode
26
This electrode is composed of Pt and H2 gas at 1 atm, used as standard measurement in electrochemistry. Use an electrolyte 1M of H+.
Standard Hydrogen Potential (SHE)
27
Calomel composition
Mercury + Hg2Cl2
28
Uses saturated KCl as electrolyte with an electrode composition of caliomel, used in corrosion study and pH measurement.
Saturated Calomel Electrode (SCE)
29
The electrode of this reference electrode is Ag wire coated with AgCl that uses saturated KCl or 3M KCl as its electrolyte.
Silver/Silver Chloride (Ag/AgCl)
30
This is the site where the redox reactions of interest take place to complete an electrochemical cell and enable the observation of the reaction.
Measuring Electrode
31
This is a measureing electrode was developed to improve the selectivity for specific ions or molecules.
Membrane Electrode
32
A type of electrode with a special ion-exchange glass, selective to H+
Glass Electrode
33
The first pH meter invented in 1934 by an American Chemist named _______.
Arnold O. Beckman
34
In modern pH meters, the _______ design is commonly used, which integrates both pH-sensitive glass and the reference electrode into a single unit.
Combination Electrode
35
CE design typically features tube-within-a-tube structure: The inner tube contains _______, while the outer tube contains ______, commonly an Ag/AgCl electrode, along with _______.
pH-sensitive Electrode Reference Electrode Salt bridge
36
A component of pH meter which is a single probe that contains both the measuring electrode and the reference electrode.
Combination Electrode
37
This is a sensitive part of pH meter, a bulb at the tip of the probe that responds to hydrogen ion concentration.
Glass Electrode
38
Stable reference point for potential measurement which is typically filled with KCl solution.
Reference Electrode
39
The outer casing of the electrode that is made of plastic or glass that protects internal component.
Electrode Body
40
The point where the reference electrode connects to the solution; allows ionic contact.
Junction (Porous Fit)
41
Digital or analog device that shows the pH reading; may include calibration and temperature controls.
pH Meter Display Unit
42
This is the deviation of an electrode's potential from its theoretical potential.
Polarization
43
Two classification of Polarization
Concentration and Kinetic Polarization
44
_____ arises. because of the limited rate of mass transfer of reactant from bulk solution to an electrode surface.
Concentration Polarization
45
This is the movement of ions from one region to another.
Mass Transfer
46
Three mechanisms of Mass Transfer
Convection Migration Diffusion
47
Transport resulting from physical motion of the solution due to stirring, vibration, or thermal gradients.
Convection
48
Movement of ions driven by electrostatic attraction between charged ions and electrodes of opposite charge.
Migration
49
Movement of species down a concentration gradient; the rate is directly proportional to the concentration difference.
Diffusion
50
The oldest voltammetric method developed in 1922; 1st practical and symmetric use of voltammetry.
Polarography
51
Polarography uses __________ Electrode.
Dropping Mercury Electrode (DME)
52
Refers to the maximum/highest current that can be achieved for a specific reaction under given conditions.
Limiting Current
53
Widely used in electrochemical analysis to study redox properties of various substance
Voltammetric Method
54
A linearly ramped potential applied tot he measuring electrode; the current measured as a function of applied potential (Polarogram)
Polarography
55
Triangular waveform potential sweep across wide range; current as a function of applied potential.
Cyclic Volatammetry (CV)
56
Linearly increasing potential from a starting point; current as a function of applied potential .
Linear Sweep Voltammetry (LSV)
57
Superimposed potential pulseson a linear sweep; difference in current before and after each pulse
Differential Pulse Voltammetry (DPV)
58
The square wave modulation of potential; current response to square wave potential oscillations.
Square Wave Voltammetry (SWV)
59
A single pulse potential applied at set intervals; current measured at pulse maximum.
Normal Pulse Voltammetry (NPV)
60
Preconcentration of analyte followed by potential sweep; current during the stripping process.
Stripping Voltammetry
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