DETERMINATION OF SINGLE BASE MUTATIONS RELATED TO THE GENE SPECIFIC DISEASES BY USING ELECTROCHEMICAL DNA BIOSENSORS IN THE INTEGRATED SYSTEM
Den Naturwissenschaftlichen Fakultäten der Friedrich-Alexander-Universität Erlangen-Nürnberg zur Erlangung des Doktorgrades
vorgelegt von Burcu Ülker
aus Izmir
Als Dissertation genehmigt von den Naturwissenschaftlichen Fakultäten der Universität
Erlangen-Nürnberg
Tag der mündlichen Prüfung: 06.07.2005
Vorsitzender der Promotionskommission: Prof. Dr. D.-P. Häder Erstberichterstatter: Prof. Dr. Ulrich Nickel Zweitberichterstatter: Prof. Dr. Carola Kryschi
Abbreviations
A Adenine a Activity BSA Albumin fraction V C Cytosine CE Counter electrode σ Charge density D Diffusion coefficient DNA Deoxyribonucleic acid DPV Differential pulse voltammogram
Eappl Applied potential
0 Ered ox Standard redox potential EDTA Ethylene diamine tetra acetic acid F Faraday constant (96.487 coulombs) FcII Factor II FcV Factor V G Guanine HET Heterozygote I Inosine IHP Inner Helmholz Plane iRs Ohmic potential j Current density (current per unit area, A/cm2) J Flux 2 j0 Exchange current density (A/cm ) µ i Chemical potential
µ* i Electrochemical potential MUT Mutated n Number of electrons NaAc Sodium acetate buffer NAP 1-Naphthylphosphate NC Non-complementary
NOS N-oxysuccinimide esters OHP Outer Helmholz Plane PCR Polymerase chain reaction pNPP p-Nitrophenylphosphate
QMT Nexterion hybridization buffer R Universal gas constant (8.314 JK-1mol-1) RE Reference electrode RNA Ribonucleic acid RT Room temperature SDS Sodium dodecyl sulphate Silane 3-Glycidyloxypropyl-trimethoxysilane SPC Screen printed chip SPE Screen printed electrode SSC Sodium saline citrate T Thymine T Temperature TBS Tris buffered saline WB Washing buffer WE Working electrode WT Wild type η Overpotential
φ Galvanic potential
1 Introduction 9 2 Theoretical Information 11 2.1 Electroanalytical Chemistry 11
2.1.1 Preface 11 2.1.2 Faradaic and Non-faradaic Processes 11 2.1.3 Electrochemical Cell 12 2.1.4 Electrode Reactions 12 2.1.5 Nernst Equation 14 2.1.6 Electrical Double Layer 15 2.1.7 The Electrode Set-up 16 2.1.8 Mass Transport 18 2.1.9 Overpotential 20 2.1.10 Controlled Potential Techniques 21 2.1.11 Working Electrodes 23
2.2 Nucleic Acids 24
2.2.1 Structure of Nucleic Acids 24 2.2.2 Hybridization and Denaturation 26 2.2.3 Mutations 27
2.3 Nucleic Acid Diagnostics 27
2.3.1 Preface 27 2.3.2 Polymerase Chain Reaction 28 2.3.3 Biosensors 30 2.3.4 Electrochemical DNA Biosensors 30
3 Experimental 31 3.1 Chemicals and Solutions 31
3.1.1 Chemicals 31 3.1.2 Solutions 32
3.2 Measurement Set-ups 35
3.2.1 Electrochemical Measurement Set-ups 35 3.2.2 Colorimetric Measurement Set-up 36
3.3 Preparation of Screen Printed Chips 36
3.4 Methods 39
3.4.1 Surface Preparation 39 3.4.2 Label-free Electrochemical Detection Method 42 3.4.3 Enzyme-based Electrochemical Detection Method 44 3.4.4 Enzyme-based Colorimetric Detection Method 46
4 Results 49 4.1 Optimisation of Detection Methods 49
4.1.1 Preface 49 4.1.2 Optimisation of Surface Preparation 49 4.1.2.1 Preface 49 4.1.2.2 Screen Printing Procedure 50 4.1.2.3 Effect of Pre-treatment Conditions 52 4.1.2.4 Silane Surface Chemistry 54 4.1.2.5 Electrochemical Properties of Inosine Base 57 4.1.2.6 Probe Immobilization 59 4.1.3 Optimisation of Hybridization 61 4.1.3.1 Preface 61 4.1.3.2 Hybridization Time 61 4.1.3.3 Hybridization Temperature 63 4.1.3.4 Optimum Washing Conditions 66 4.1.3.5 Sensitivity of the Detection Methods 68
4.2 Investigation of Optimum Probe Sequences 71
4.3 Determination of Single Base Mutations 74
4.4 Development of Lab-on-a-chip Technology 77
4.4.1 Preface 77 4.4.2 Detection Process in the Cartridge 78 4.4.3 Integrated Process in the Cartridge 80
5 Summary 83 6 References 86 7 Zusammenfassung 93
Introduction 9
1 Introduction
Determination of specific nucleic acid sequences in biological and environmental samples can lead to early diagnosis of inherited human diseases as well as identification and detection of pathogens1. The determination of nucleic acids in biological samples consists of three steps: Sample preparation, specific nucleic acid amplification and detection.
In the sample preparation step, the extraction and purification of the nucleic acids are performed. First, the relevant cells are lysed by destroying their cellular membrane in order to release the nucleic acids. Then the released nucleic acids are extracted and purified by using different methods.
Usually, the amount of extracted nucleic acids is not sufficient for the determination. Therefore, a part of the nucleic acid is amplified, for example, using polymerase chain reaction (PCR). During the PCR, many copies of the specific DNA sequence are created. The reaction is initiated using a pair of short primer sequences which match the ends of the sequence to be copied. Thereafter, each cycle of the reaction copies the sequence between the primers. Primers can bind to the copies as well as the original sequence, so in time the total number of copies increases exponentially.
The simplest method for the detection of amplified nucleic acids is gel electrophoresis whereby the DNA is separated according to length and stained with ethidium bromide. However, this method is label intensive and not sequence specific. Sequence specificity can be achieved by transferring the separated DNA to a membrane and hybridising with a radioactively2 labelled probe. This method is very sensitive but complex handling with hazardous radioactive labels are necessary. The other methods which are achieved by labelling the probe with biotin3,4, digoxigenin3,5 or fluorescent dyes6 in order to avoid the use of hazardous radioactive labels are also not suitable for the routine analysis because of the long, expensive and complicated steps of these procedures. Therefore a new, sensitive, low-cost and sequence specific detection of nucleic acid hybridization by using electrochemical DNA biosensors has recently been reported1,8-10 . An electrochemical DNA biosensor is an electrode with immobilised sequence specific single strand DNA (probe) for the identification of target DNA based on its hybridization reaction with its complementary sequence (target) under suitable conditions. The sequence-specific hybridization events can be detected directly (label-free)11-13 or indirectly by using labels
10 Introduction
(indicator-based). The labels can be indicators which intercalate into the DNA double helix (metal complexes, antibiotics)14-16 or which interact specifically with guanine bases of DNA10,17-19. The other possible detection method represents the use of substrate which is changed to an electrochemically active end product in the presence of a specific enzyme (enzyme-based)20.
Electrochemical DNA biosensors, based on electrochemical transduction of hybridization events, have great promise for the task of pharmaceutical, clinical, environmental and forensic applications. Such devices couple the high specificity of DNA hybridization reactions with the high sensitivity, low cost and portability of electrochemical transducers21. The electrochemical biosensors can be assembled to a miniaturised array22. These miniaturised arrays of DNA biosensors are termed DNA chips.
The development of DNA chips is motivated by their potential for application in disease diagnosis, genome sequencing23, the detection of polymorphisms24 and single-base mismatches25. However, such micro fabricated devices are costly and difficult to prepare and handle. For this reason, newly developed DNA chips must offer lower cost and greater material efficiencies to gain acceptance over traditional nucleic acid diagnostic methods. Further reduction in the cost of performing nucleic acid diagnostics can be realized by utulizing less expensive detection methods and electrode materials.
The aim of the current work is the development of low-cost DNA chips for the determination of single base mutations, which lead to inherited diseases or disorders (Factor V and Factor II) from blood samples on the fluidic platform in a disposable integrated cartridge in which the processes of sample preparation, PCR and detection are accomplished automatically.
The use of a fully automated detection system in combination with its low cost, its simplicity in handling and the disposability of the DNA chips make the determination methods, which are developed for detection of gene-specific inherited diseases, suitable for routine laboratory analysis and point-of-care diagnosis.
Theoretical Information 11
2 Theoretical Information
2.1 Electroanalytical Chemistry35,36
2.1.1 Preface
Electroanalytical chemistry is concerned with the interplay between electricity and chemistry, namely the measurements of electrical quantities, such as current, potential and charge and their relationship to chemical parameters. The factors effecting the transport of charges across the interfaces between two phases are the important issue in electroanalytical chemistry. One of these two phases contributing to the interface is an electrolyte, through which charge is carried by the movements of ions. Electrolytes can be liquid solutions or fused salts, or they can be ionically conducting solids such as sodium β-alumina, which has mobile sodium ions. The second phase at the interface might be another electrolyte, or it might be a conductor, through which charge is carried by electronic movement. The conductors can be solid or liquid. The transition of the charges, the crossing from one conducting phase into the other at the interface leads to a difference in potential. These two-phase systems can be formed by using two solid (metal-metal) or one solid and one liquid phase (metal-electrolyte). The metal-electrolyte systems describe the basis of electrochemistry whereas the metal-metal systems are used commonly for the measurement of temperature.
2.1.2 Faradaic and Non-faradaic Processes35
Two types of processes occur at the electrodes. One of these is the transferration of charges over the metal-solution interface. This electron transfer causes oxidation or reduction to occur. Since these reactions are governed by Faraday’s law, they are called faradaic processes. Faraday's law relates the amount of charge involved in an electrochemical reaction with the number of moles of reactant and the number of electrons required for the reaction. The faradaic processes are usually important in investigation of electrode reactions in the electrochemical cells. Non-faradaic processes involve the accumulation of charges at the metal-solution interface. In case of non-faradaic processes such as adsorption or desorption, the structure of the electrode and solution interface can change, influenced by changing potential or solution composition.
12 Theoretical Information
Non-faradaic processes occurring at electrodes cause a flow of non-faradaic currents (charging currents). 2.1.3 Electrochemical Cell36-38
The system which is formed by electrode-electrolyte phases is called electrochemical half- cell. The connection of two half-cells through a salt bridge forms an electrochemical cell (Scheme 1). The electrodes of both half-cells must be connected to a voltmeter in order to measure the cell potential.
Voltmeter
Salt bridge Electrode Electrode
Electrolyte
Half cell 1 Half cell 2
Scheme 1. Electrochemical Cell
2.1.4 Electrode Reactions35-39
Electrode reactions are heterogeneous chemical processes. These reactions occur due to the charge transfer through the interface of both phases, electrode and electrolyte. The heterogeneous charge transfer is caused by the varying chemical potentials (µ) of metal ions (Mez+) in the solution (L) and on the metal surface (M).
Due to the contact between two phases, with time, a chemical equilibrium develops at the interface.
Theoretical Information 13
µ ()L = µ (M ) with µ = µ o + RT ⋅ln a (1) i i i i i
In the systems featuring a difference of the chemical potentials as depicted in equation 2, the ions are transferred from the metal to the solution.
µ ()M > µ (L) (2) Mez+ Mez+
The ion transition leads to a negative charge on the metal surface, while the positively charged metal ions are assembled at the solution boundary. Thus, an electrical double layer is formed to compensate for the excess of charge on the electrode (qe), since the interface must be neutral. Due to the formation of an electrical double layer, the difference in the galvanic potential in both phases will be increased and the transfer of the metal ions will be more difficult.
The work necessary for the transition of the ions against the double layer is equal to the difference of the chemical potential in both phases and depends on the chemical environment.
∆µ = µ ()M − µ (L) (3) Mez+ Mez+
Another additional work is required to move the metal ions against the electrical field. This work is proportional to the galvanic potential (φ) and hence depends on the electrical properties of an environment that is very much larger than an ion itself. These two amounts of work for a single species can not be separated experimentally, but the differences in the scales of the environments responsible for them, make it possible to separate them mathematically. Butler and Guggenheim developed the conceptual separation and introduced the * electrochemical potential (µ ), for species i with charge zi in phase α:
*α α α µi = µi + zi Fϕ (4)
α Where µ is the familiar chemical potential, zi Fϕ is the amount of electrochemical work.
In the case of equal electrochemical potentials in both phases, an electrochemical equilibrium balances at the interface.
14 Theoretical Information
* * µi ()L = µi (M) (5)
The difference of the galvanic potential in both phases in a half cell is given by equation 6.
∆φ = φ M − φ L (6)
This difference of the potential between metal (M) and solution (L) without a passing current can be calculated by means of the concentration dependency of the chemical potential as given in equation 7.
µ 0 ( M ) − µ 0 ( L ) a ( M ) z+ z+ RT z+ ∆φ = φ − φ = Me Me + ln Me (7) M L zF zF a ( L ) Mez+
The galvanic potential consists of two different terms. One is dependent on the concentration whereas the other one is not. The term which is not dependent on the concentration is called standard potential, where the value of the activity coefficients of the components in both phases are one (a=1) in the reference conditions. The resulted equation which explains the concentration dependency of galvanic potential for metal/metal ions half cell is Nernst Equation (equation 8).
o RT a ( L ) ∆φ = ∆φ + ln i (8) zF ai ( M ) R is the universal gas constant (8.314 JK-1mol-1), T is the temperature in Kelvin, n is the number of electrons transferred in the reaction, and F is the Faraday constant (96.487 coulombs).
2.1.5 Nernst Equation35-37,40
Redox processes proceed in the half cells, which are formed by dipping an electrode into the electrolyte containing redox active components. Redox processes are reversible processes fast enough to be considered stable in thermodynamic equilibrium. The basic electrode reaction occurring at the redox electrode is,
ne − + Ox ⇔ Re d
Theoretical Information 15
where Ox and Red are the oxidised and reduced forms, respectively, of the redox couple. Such reactions occur in a potential region which makes the electron transfer thermodynamically or kinetically favourable. The relationship between the potential of the electrode and the concentration of the electroactive species at the surface is described with Nernst Equation (equation 9).
0 RT [Ox ] E = E Red Ox + ln (9) Red Ox nF [Re d ]
o where E red/ox is the standard potential for the redox reaction.
The Nernst Equation is only valid if the system is in an electrochemical equilibrium. The redox potential will adjust slowly if the transition of the electrons at the corresponding electrode is slow. In this case, the Nernst Equation is not valid.
2.1.6 Electrical Double Layer36, 39, 40
The electrical double layer is the array of the charged particles and/or oriented dipoles which exists at every material interface. In electrochemistry, such layers reflect the ionic zones formed in the solution to compensate for the excess of charge on the electrode. Accordingly, such a counter-layer is made of ions of opposite sign to that of the electrode. The electrical double layer consists of three main parts: the metallic phase, an inner layer and an outer or diffuse layer.
The layer closest to the electrode, inner layer (Helmholtz Layer), contains solvent molecules and specifically adsorbed ions. The locus of the electrical centers of the specifically adsorbed ions is called the Inner Helmholz Plane (IHP). The total charge density (µC/cm2) from specifically adsorbed ions in this layer is σi. Whenever the interaction between ion and the metal is not strong enough for the desolving process, the ion can not come as close to the metal as the specifically adsorbed ions. The imaginary plane passing through the electrical centers of the closest approaching solvated ions is known as the Outer Helmholtz Plane (OHP). The interaction of the solvated ions with the charged metal involves only long-range electrostatic forces, thus, this interaction is essentially independent from the chemical properties of the ions. These ions are said to be non-specifically adsorbed. Unlike specifically adsorbed ions at the IHP which form a two-dimensional monolayer, the non-specifically adsorbed ions are not all located at the OHP but are distributed in a three-dimensional region, called the diffuse layer, which extends from the OHP all the way into the bulk of the solution.
16 Theoretical Information
The excess charge density in the diffuse layer is σd, so that the total excess charge density on the solution side of the double layer, σs, is given by:
σ s = σ i + σ d = −σ M (10) where σM is the charge density on the metal.
In controlled-potential techniques, the charging of the double layer is responsible for the background current known as the charging current, which limits the detectability of redox active substances. Such a charging process is non-faradaic because electrons are not transferred across the electrode-solution interface. It occurs when a potential is applied across the double layer, or when the electrode area or capacitance is changing. Note that the current is the time derivative of the charge. Hence, when such processes occur, a residual current is flowing based on the differential equation:
dq dE dA dC i = = C A + C ( E − E ) + A(E − E ) dl (11) dt dl dt dl pzc dt pzc dt where dE/dt is the potential scan rate, dA/dt is the rate of the change of the area, Cdl is the capacitance per unit area, Epzc is the potential at zero charge and dCdl/dt is the rate of capacitance change. The term dCdl/dt yields importance if adsorption processes change the double layer capacitance.
2.1.7 The Electrode Set-up37
The overall chemical reaction taking place in an electrochemical cell is made up of two independent half reactions, which constitute the real chemical changes at the two electrodes. Each half reaction responds to the interfacial potential difference at the corresponding electrode. In electrochemistry, one of these specific electrochemical reactions is important, and the electrode at which it occurs is called the working electrode, whereas the other is called the reference electrode.
Since the reference electrode exhibits constant conditions, the potential difference between the reference electrode and the measurement buffer is constant. Therefore, the working electrode is responsible for any changes within the cell. Thus, the observed potential of working electrode is evalued with respect to the reference electrode. If the passage of current does not effect the potential of the reference electrode, the potential (E) of working electrode is given by equation (12).
Theoretical Information 17
E appl = E + iR s = E eq + η + iR s (12)
The term iRs is the ohmic potential drop in the solution, the Eeq is the potential of the working electrode in an open circuit, η is the overpotential, Eappl is the applied potential and E is the new potential value of the working electrode. Under conditions where iRs is small (less than 1-2 mV), the two electrode set-up can be used to determine the i-E curve. On the other hand, when currents or solution resistance are high (e.g., in large scale, electrolytic cells or galvanic cells or in experiments involving non-aqueous solutions with low conductivities), the iRs term may be much larger. In experiments where iRs may be high, a three electrode set-up is preferable in order to minimise the iRs (Scheme 2).
Power supply
I
Auxiliary electrode Working electrode Reference electrode V In cell notation
Working electrode
Reference electrode
Auxiliary electrode
Scheme 2 . Three-electrode cell and notation for the different electrodes.
In this setup, the current is passed between the working electrode and auxiliary (so-called counter) electrode. The auxiliary electrode can be any electrode desired, because its electrochemical properties do not influence the behaviour of the electrode of interest. It is usually chosen to be an electrode that does not produce substances by electrolysis which can reach the working electrode surface and cause interfering reactions there. The potential of the working electrode is measured relatively to a separate reference electrode. The device used to
18 Theoretical Information
measure or monitor the difference in potential between the working and reference electrodes has a high input impedance so that a negligible current is passed through the reference electrode. In the three electrode set up, the current which is caused from the high input impedance of the device is passed not through the reference electrode but through the auxiliary electrode, so that the potential of the reference electrode remains constant and, the iRs contribution to the measurement will be small.
2.1.8 Mass Transport35, 36, 38
The Nernst Equation is limited to the surface region of the electrode. For a more realistic description of real redox experiments, the mass transport of the redox pair species between the bulk solution and the surface area has to be considered. Mass transfer is the movement of material from one location within a solution to another. It arises either from differences in electrical or chemical potential between the two locations, or from movement of a volume element of the solution. The modes of mass transfer are diffusion, convection and migration.
The flux (J) is a common measure for the mass transport at a fixed point. It is defined as the number of molecules penetrating a unit area of an imaginary plane in a unit of time, and has -2 -1 the units of mol cm s . The flux of species i (Ji) at a distance x from the surface is governed by the Nernst-Planck equation, written for one dimensional mass transfer along the x-axis as:
∂C ( x ) z F ∂φ ( x ) J ( x ) = − D i − i D C + C v( x ) (13) i i ∂x RT i i ∂x i
2 where Di is the diffusion coefficient (cm /sec), ∂Ci (x)/ ∂x is the concentration gradient at distance x, ∂φ()x / ∂x is the potential gradient, zi and Ci are the charge and concentration of species I, respectively and v(x) is the velocity (m/sec) with which a volume element in solution moves along the axis.
Diffusion
Diffusion is the movement of a species under the influence of a concentration gradient from regions of high concentrations to regions of lower ones. The aim is to compensate the concentration differences. It occurs in all solutions and arises from local uneven concentrations of reactants. Entropic forces act to smooth out these uneven concentration distributions and are therefore the main driving force for this process.
Theoretical Information 19
The rate of diffusion can be predicted within a solution of constant viscosity using Fick's First Law (for linear diffusion):
∂[ c ] ⎛ ∂ 2 [ c ] ⎞ = D ⎜ ⎟ (14) c ⎜ 2 ⎟ ∂t ⎝ ∂x ⎠
The rate of change in the concentration as a function of time is related to the change in the concentration gradient. So the steeper the change in concentration the greater the rate of diffusion. In practice diffusion is the most significant transport process for the majority of electrolysis reactions.
Convection (stirring or hydrodynamic transport)
Convection is the transport to the electrode by a gross physical movement. The fluid flow occurs by stirring or flowing the solution and by rotating or vibrating the electrode (forced convection) or because of density gradients (natural convection).
The natural convection is generated by small thermal or density differences and mixes the solution in a random and therefore unpredictable manner. In the case of electrochemical measurements, these effects tend to lead to problems for longer measurement periods. It is possible to drown out the natural convection effects from an electrochemical experiment by deliberately introducing convection into the cell. This form of convection is termed forced convection. It is typically several orders of magnitude greater than any natural convection effects and therefore effectively removes the random aspect from the experimental measurements. This, of course, is only true if the convection is introduced in a well defined and quantitative manner.
Migration Migration is the movement of charged particles along an electrical field. This is essentially an electrostatic effect which arises due the application of a voltage on the electrodes. This effectively creates a charged interface (the electrodes). Any charged species near that interface will either be attracted or repelled from it by electrostatic forces. Due to ion solvation effects and diffuse layer interactions in solution, migration is notoriously difficult to calculate accurately for real solutions. Consequently, most voltammetric measurements are performed in solutions which contain a background electrolyte (e.g. KCl) that does not undergo electrolysis itself but helps to shield the reactants from migratory effects. By adding a large quantity of the electrolyte (relative to the reactants) it is possible to ensure that the
20 Theoretical Information
electrolysis reaction is not significantly effected by migration. The purpose of introducing a background electrolyte into a solution is not, however, solely to remove migration effects as it also acts as a conductor.
2.1.9 Overpotential36, 40, 41
The overpotential (η) is the difference between the electrode potential and the equilibrium potential at open circuit when a current (i) passes between the electrodes. An overpotential is generally caused by a kinetic inhibition of one reaction step of the electrochemical process. There are different overpotential contributions associated with different reaction steps:
1) Charge transfer overpotential ()ηct
The charge transfer through the Helmholtz layer is a rate determining step.
2) Mass transport overpotential ()ηmt
Mass transport is a rate determining step. The mass transport overpotential can be considered as a sum of different overpotentials which are observed in case of the diffusion (D), convection (C) and migration (M) modes of mass transport.
η mt = η D + η M + η C (15)
3) Reaction overpotential ()ηR
Reactions proceeding or following the electrode reaction are rate determining.
The total overpotential can be considered as a sum of different contributions.
η = η CT + η MT + η R (16)
For a given overpotential, the magnitude of current flow can depend on a number of factors, including the mass transfer by diffusion, convection or migration, as well as the charge transfer rate between solution species and the electrode (called electrode kinetics). Positive overpotentials (i.e. potentials more positive than the equilibrium potential) cause oxidation reactions at the electrode, whereas negative overpotentials cause reduction reactions to occur.
If the solution is well stirred or currents are kept so low that the surface concentrations do not differ appreciably from the bulk values (kinetics-limited regime), the current-potential relationship is given by the Butler-Volmer Equation (15):
Theoretical Information 21
αnF −()1−α nF − ⎛ η η ⎞ for a reaction ne + Ox ⇔ Red (17) j = j ⎜e RT − e RT ⎟ 0 ⎜ ⎟ ⎝ ⎠
2 where j is the current density (current per unit area, A/cm ), j0 is the exchange current density (A/cm2), α is the transfer coefficient and n is the number of electrons transferred.
Since mass transfer effects are not included here, the overpotential associated with any given current serves solely as activation energy. It is required to drive the heterogeneous process at the rate reflected by the current. The lower the exchange current, the more sluggish the kinetics are and hence the larger is the activation overpotential for any particular net current. If the exchange current is very large, then the system can supply large currents, perhaps even the mass transfer limited current, with insignificant activation overpotential. In that case, any observed overpotential is associated with changing surface concentrations of species Ox and Red. It is called a concentration overpotential and can be viewed as activation energy required to drive mass transfer at the rate needed to support the current.
2.1.10 Controlled Potential Techniques
The basis of all controlled potential techniques is the measurement of the current response to an applied potential. A multitude of potential excitations (including a ramp, potential steps, pulse trains, a sine wave, and various combinations thereof) exist.