Silver chloride electrode

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Ag-AgCl reference electrode

A silver chloride electrode is a type of reference electrode, commonly used in electrochemical measurements. For example, it is usually the internal reference electrode in pH meters. As another example, the silver chloride electrode is the most commonly used reference electrode for testing cathodic protection corrosion control systems in sea water environments.

The electrode functions as a redox electrode and the reaction is between the silver metal (Ag) and its salt — silver chloride (AgCl, also called silver(I) chloride).

The corresponding equations can be presented as follows:

 Ag^+ + e^- \leftrightharpoons Ag(s)
 AgCl(s) \leftrightharpoons Ag^+ + Cl^-

or an overall reaction can be written:

 AgCl(s)+ e^- \leftrightharpoons Ag(s)+ Cl^-

This reaction is characterized by fast electrode kinetics, meaning that a sufficiently high current can be passed through the electrode with the 100% efficiency of the redox reaction (dissolution of the metal or cathodic deposition of the silver-ions). The reaction has been proven to obey these equations in solutions of pH values between 0 and 13.5.

The Nernst equation below shows the dependence of the potential of the silver-silver(I) chloride electrode on the activity or effective concentration of chloride-ions:

E= E^0 - \frac{RT}{F} \ln a_{Cl^{-}}

The standard electrode potential E0 against standard hydrogen electrode (SHE) is 0.230V ± 10mV. The potential is however very sensitive to traces of bromide ions which make it more negative. (The more exact standard potential given by an IUPAC review paper is 0.22249 V, with a standard deviation of 0.13 mV at 25 °C.[1])

Applications[edit]

Commercial reference electrodes consist of a plastic tube electrode body. The electrode is a silver wire that is coated with a thin layer of silver chloride, either physically by dipping the wire in molten silver chloride, or chemically by electroplating the wire in concentrated hydrochloric acid.[2]

A porous plug on one end allows contact between the field environment with the silver chloride electrolyte. An insulated lead wire connects the silver rod with measuring instruments. A voltmeter negative lead is connected to the test wire. The reference electrode contains potassium chloride to stabilize the silver chloride concentration.

The potential of a silver:silver chloride reference electrode with respect to the standard hydrogen electrode depends on the electrolyte composition.

Reference Electrode Potentials
Electrode Potential E0+Elj Temperature Coef.
(V) at 25 °C (mV/°C) at around 25 °C
SHE 0.000 0.000 [3]
Ag/AgCl/Sat. KCl +0.197 -1.01[citation needed]
Ag/AgCl/3.5 mol/kg KCl[4] +0.205 -0.73
Ag/AgCl/3.0 mol/kg KCl +0.210  ?
Ag/AgCl/1.0 mol/kg KCl +0.235 +0.25[citation needed]
Ag/AgCl/0.6 mol/kg KCl +0.25
Ag/AgCl (Seawater) +0.266

Notes to the Table: (1) The table data source is,[5] except where a separate reference is given. (2) Elj is the potential of the liquid junction between the given electrolyte and the electrolyte with the activity of chloride of 1 mol/kg.

The electrode has many features making is suitable for use in the field:

  • Simple construction
  • Inexpensive to manufacture
  • Stable potential
  • Non-toxic components

They are usually manufactured with saturated potassium chloride electrolyte, but can be used with lower concentrations such as 1 mol/kg potassium chloride. As noted above, changing the electrolyte concentration changes the electrode potential. Silver chloride is slightly soluble in strong potassium chloride solutions, so it is sometimes recommended the potassium chloride be saturated with silver chloride to avoid stripping the silver chloride off the silver wire.

Biological electrode systems[edit]

Tab electrode using silver/silver chloride sensing for electrocardiography (ECG)[6]

Silver chloride electrodes are also used by many applications of biological electrode systems such as biomonitoring sensors as part of electrocardiography (ECG) and electroencephalography (EEG), and in transcutaneous electrical nerve stimulation (TENS) to deliver current. Historically, the electrodes were fabricated from solid materials such as silver, brass coated with silver, tin and nickel. In today's applications, most biomonitoring electrodes are silver/silver chloride sensors which are fabricated by coating a thin layer of silver on plastic substrates and the outer layer of silver is converted to silver chloride.[7]

The principle of silver/silver chloride sensors operation is the conversion of ion current at the surface of human tissues to electron current to be delivered through the lead wire to the instrument to read. An important part of the operation is electrolyte gel which is applied between the electrode and tissues. The gel contains free chloride ions such that the charge can be carried through the electrolyte, therefore the electrolyte can be considered as conductive for ion current as the human tissues. When the ion current exists, the silver atoms in the electrode oxidize and discharge cations to the electrolyte and the electrons carry charge through the lead wire. At the same time, the chloride ions which are anions in the electrolyte travel toward the electrode and they are reduced as they bond with silver of the electrode resulting in silver chloride and free electrons to deliver to the lead wire. The reaction allows current to pass from electrolyte to electrode and the electron current passes through the lead wire for the instrument to read.[8][9]

When there is an uneven distribution of cations and anions, there will be a small voltage called half-cell potential associated with the current. In the DC system that is used by the ECG and EEG instruments, the difference between the half-cell potential and the zero potential is shown as DC offset which is an undesirable characteristic. Silver/silver chloride is a popular choice of biological electrodes due to its low half-cell potential of approximately 220 mV and the lower of the impedance of the electrode by silver chloride.[8]

Elevated temperature application[edit]

When appropriately constructed, the silver chloride electrode can be used up to 300 °C. The standard potential (i.e., the potential when the chloride activity is 1 mol/kg) of the silver chloride electrode is a function of temperature as follows:[10]

Temperature Dependence of the Standard Potential of the Silver/Silver Chloride Electrode
Temperature Potential E0
°C V versus SHE at the same temperature
25 0.22233
60 0.1968
125 0.1330
150 0.1032
175 0.0708
200 0.0348
225 -0.0051
250 -0.054
275 -0.090

Bard et al.[11] give the following correlations for the standard potential of the silver chloride electrode as a function of temperature (where t is temperature in °C):

E0(V) = 0.23695 - 4.8564x10−4t - 3.4205x10−6t2 - 5.869 x 10−9t3 for 0 < t < 95 °C.

The same source also gives the fit to the high-temperature potential, which reproduces the data in the table above:

E0(V) = 0.23735 - 5.3783x10−4t - 2.3728x10−6t2 for 25 < t < 275 °C.

The extrapolation to 300 °C gives E0 of -0.138 V.

Farmer[12] gives the following correlation for the potential of the silver chloride electrode with 0.1 mol/kg KCl solution, accounting for the activity of Cl- at the elevated temperature:

E0.1 mol/kg KCl(V) = 0.23735 - 5.3783x10−4t - 2.3728x10−6t2 + 2.2671x10−4(t+273) for 25 < t < 275 °C.

See also[edit]

For use in soil they are usually manufactured with saturated potassium chloride electrolyte, but can be used with lower concentrations such as 1 M potassium chloride. In seawater or chlorinated potable water they are usually directly immersed with no separate electrolyte. As noted above, changing the electrolyte concentration changes the electrode potential. Silver chloride is slightly soluble in strong potassium chloride solutions, so it is sometimes recommended that the potassium chloride be saturated with silver chloride.

References[edit]

  1. ^ R.G. Bates and J.B. MacAskill, "Standard Potential of the Silver-Silver Chloride Electrode", Pure & Applied Chem., Vol. 50, pp. 1701—1706, http://www.iupac.org/publications/pac/1978/pdf/5011x1701.pdf
  2. ^ Detail of Making and Setting up a Microelectrode, University of Denver, http://carbon.cudenver.edu/~bstith/detailelectrode.doc (link is obsolete)
  3. ^ Bratsch, Steven G. (1989), "Standard Electrode Potentials and Temperature Coefficients in Water at 298.15 K", J. Phys. Chem. Ref. Data 18 (1): 1–21, Bibcode:1989JPCRD..18....1B, doi:10.1063/1.555839 
  4. ^ D.T. Sawyer, A. Sobkowiak, J.L. Roberts, "Electrochemistry for Chemists", 2nd edition, J. Wiley and Sons Inc., 1995.
  5. ^ "NACE International CP Specialist Course Manual"
  6. ^ "CARDEX Electrodes". CARDEX. Retrieved 21 August 2014. 
  7. ^ Emma, Salvatore Jr. (8 August 2011). "A Brief Look at ECG Sensor Technology". Medical Design Technology Magazine. Retrieved 20 August 2014. 
  8. ^ a b Lee, Stephen; Kruse, John. "Biopotential Electrode Sensors in ECG/EEG/EMG Systems". Analog Devices, Inc. Retrieved 21 August 2014. 
  9. ^ Dickter, Cheryl L; Kieffaber, Paul D (20 December 2013). SAGE. pp. 14–15. ISBN 9781446296745 http://books.google.com/books?id=IQSgAgAAQBAJ&printsec=frontcover#v=onepage&q&f=false. Retrieved 21 August 2014.  Missing or empty |title= (help)
  10. ^ R.S. Greeley, J. Phys. Chemistry, 64, 652, 1960.
  11. ^ A.J. Bard, R. Parson, J. Jordan, "Standard Potentials in Aqueous Solution", Marcel Dekker, Inc., 1985.
  12. ^ Joseph Farmer, "Waste Package Degradation Expert Elicitation Panel: Input on the Corrosion of CRM Alloy C-22", Lawrence Livermore National Laboratory, report UCRL-ID-130064 Information Bridge: DOE Scientific and Technical Information - Sponsored by OSTI (pdf)

External links[edit]