(a) Calculate the electrode potential of silver electrode dipped in 0.1 M solution of silver nitrate at 298 K assumimg AgNO3 to be completely dissociated. The standard electrode potential of Ag+/Ag is 0.80 V at 298 K.
(a) Ag++e-→ Ag(s) EAg+/Ag = 0or 0.80-0.05911log1Ag+=0or log[Ag+] = 0.800.0591or Ag+ = 3.438 × 1013M. A silver chloride electrode is a type of reference electrode, commonly used in electrochemical measurements. For environmental reasons it has widely replaced the saturated calomel electrode. For example, it is usually the internal reference electrode in pH meters and it is often used as reference in reduction potential measurements. As an example of the latter, 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 reversible redox electrode and the equilibrium is between the solid (s) silver metal (Ag(s)) and its solid salt—silver chloride (AgCl(s), also called silver(I) chloride) in a chloride solution of a given concentration. In electrochemical cell notation, the silver chloride electrode is written as, e.g., for an electrolyte solution of KCl 3 M: Ag ( s ) | AgCl ( s ) | KCl ( 3 M ) {\displaystyle {\ce {{Ag(s)}\ |\ {AgCl(s)}\ |\ KCl\ (3M)}}} The corresponding half-reactions can be presented as follows: Ag + + e − ↽ − − ⇀ Ag ( s ) {\displaystyle {\ce {Ag+ + e^- <=> Ag(s)}}}or, can be written together:[why?][clarification needed][citation needed] AgCl ( s ) + Ag ( s ) + e − ↽ − − ⇀ Ag ( s ) + e − + Cl − + Ag + {\displaystyle {\ce {AgCl(s) + Ag(s) + e^- <=> Ag(s) + e^- + Cl^- + Ag+}}}which can be simplified: AgCl ( s ) ↽ − − ⇀ Ag + + Cl − {\displaystyle {\ce {AgCl(s) <=> Ag+ + Cl^-}}}This reaction is a reversible reaction and is characterized by fast electrode kinetics, meaning that a sufficiently high current can be passed through the electrode with 100% efficiency of the redox reaction (anodic oxidation and dissolution of the Ag metal along with cathodic reduction and deposition of the Ag+ 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: The standard electrode potential E0 against standard hydrogen electrode (SHE) is 0.230 V ± 10 mV.[citation needed] 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] Commercial reference electrodes consist of a glass or plastic tube electrode body. The electrode consists of a metallic silver wire (Ag(s)) coated with a thin layer of silver chloride (AgCl), either physically by dipping the wire in molten silver chloride, chemically by electroplating the wire in concentrated hydrochloric acid (HCl)[2] or electrochemically by oxidising the silver at an anode in a chloride solution. A porous (or fibrous) filter located at/near the tip of the reference electrode allows to establishing a liquid contact between the solution to be measured and the electrolyte solution in equilibrium with the silver chloride (AgCl) coating the Ag(s) surface. An insulated electrical wire connects the silver rod with the measuring instrument. The voltmeter negative terminal is connected to the test wire. The electrode body contains potassium chloride to stabilize the silver chloride concentration. When working in seawater, this body can be removed and the chloride concentration is fixed by the stable salinity of seawater. The potential of a silver:silver chloride reference electrode with respect to the standard hydrogen electrode depends on the composition of the electrolyte solution and on temperature.
Notes to this table: The electrode has many features making it suitable for use in the field:
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 systemsTab 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 pure silver, or from metals such as tin, nickel, or brass (an alloy of copper and zinc) coated with a thin film of silver. 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 while 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 an electrical wire to the measurement instrument. An important component of the operation is the electrolyte gel applied between the electrode and the tissues. The gel contains free chloride ions such that the ion charge can be carried through the electrolyte solution. Therefore, the electrolyte solution has the same conductivity for the ion current as the human tissues. When the ion current develops, the metallic silver atoms (Ag(s)) of the electrode oxidize and it releases Ag+ 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 direct current (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 common choice of biological electrodes due to its low half-cell potential of about +222 mV (SHE), low impedance, with a toxicity lower than that of the calomel electrode containing mercury.[8] 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]
Bard et al.[11] give the following correlations for the standard potential of the silver chloride electrode between 0 and 95°C as a function of temperature (where t is temperature in °C): E 0 ( V ) = 0.23659 − ( 4.8564 × 10 − 4 ) t − ( 3.4205 × 10 − 6 ) t 2 − ( 5.869 × 10 − 9 ) t 3 {\displaystyle E^{0}(V)=0.23659-\left(4.8564\times 10^{-4}\right)t-\left(3.4205\times 10^{-6}\right)t^{2}-\left(5.869\times 10^{-9}\right)t^{3}}The same source also gives the fit to the high-temperature potential between 25 and 275°C, which reproduces the data in the table above: E 0 ( V ) = 0.23735 − ( 5.3783 × 10 − 4 ) t − ( 2.3728 × 10 − 6 ) t 2 {\displaystyle E^{0}(V)=0.23735-\left(5.3783\times 10^{-4}\right)t-\left(2.3728\times 10^{-6}\right)t^{2}}The extrapolation to 300°C gives E 0 ( V ) = − 0.138 V {\displaystyle E^{0}(V)=-0.138\ \mathrm {V} } . Farmer[12] gives the following correction for the potential of the silver chloride electrode with 0.1 mol/kg KCl solution between 25 and 275°C, accounting for the activity of Cl− at the elevated temperature: E 0.1 mol / kg KCl ( V ) = 0.23735 − ( 5.3783 × 10 − 4 ) t − ( 2.3728 × 10 − 6 ) t 2 + ( 2.2671 × 10 − 4 ) ( t + 273 ) {\displaystyle E^{0.1\ {\ce {mol/kg\ KCl}}}(V)=0.23735-\left(5.3783\times 10^{-4}\right)t-\left(2.3728\times 10^{-6}\right)t^{2}+\left(2.2671\times 10^{-4}\right)(t+273)}
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.
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What is the electrode potential of silver?
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