Glass electrode

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Glass electrode is potentiometric sensor made from glass of a specific composition. Almost all commercial electrodes related to ion-selective sensors with electrode function for single charged ions, like H⁺, Na⁺, Ag⁺. Only few chalcogenide glass electrodes have electrode function for double-charged ions, like Pb²⁺, Cd²⁺ and some other.
There are two main glass-forming systems:

silicate matrix based on molecular network of silicon dioxide (SiO₂) with additions of other metal oxides, such as Na, K, Li, Al, B, Ca, etc.
chalcogenide matrix based on molecular network of AsS, AsSe, AsTe.

Corresponding general electrode function usually marked as pH glass electrode, pNa glass electrode. Usually one glass electrode has only one general electrode function, for example pH or pNa, and such electrodes called ion-selective electrodes. But parameters of any ion-selective electrodes depend on concentrations of interfering ions. Because of the ion-exchange nature of glass membrane, it is possible for some other ions concurrently interact with ion-exchange centers of glass and to distort linear dependence of measured electrode potential on pH or other general electrode function. In some cases it is possible to change electrode function from one ion to another. One of this case is a some silicate pNa electrodes with can be changed to pAg function after soaking it into silver salt solutions.

Dependence of the electrode potential of pH glass electrode on composition of studied solution can be represented by follow equation (also known as Nikolsky equation):

$E=E^0 + \frac{RT}{F} ln \left ( a_{H^+} + K_{HNa}*a_{Na^+} \right ),$ when electrode has "general" pH electrode function with interfering influence of Na-ions.
a_H+, a_Na+ - activity of hydrogen and sodium ions;

In more common case for series of single charged ions:
$E=E^0 + \frac{RT}{F} ln \left ( a_{H^+} + \sum_{j}^N K_{Hj}*a_{j} \right )$

K_HNa - selectivity coefficient, shows magnitute of interference influence. For example, K_HNa=10^-12 means that selectivity of the glass electrode for Na-ion in 10^-12 less than for H⁺.

As one can see the range of the dependence electrode potential on pH at constant concentration of interfering ions divided into 3 parts.

Scheme of the typical dependence E-pH for ion-selective electrode

Complete realization of general electrode function, where dependence of potential on pH has linear behavior and within which such electrode really works as ion-selective electrode for pH.

$E=E^0 - \frac{2.303RT}{F} pH,$

Alkali error range - at low concentration of hydrogen-ions (high values of pH) contributions of interfering alkali metals (like Li, Na, K) are comparable with one of hydrogen-ions. In this situation dependence of the potential on pH become non-linear.
Acidic error range - at very high concentration of hydrogen-ions (low values of pH) it can be detected the influence of the anions of corresponding acid solution as well as destruction of the glass matrix.

There are different types of pH glass electrode, some of them have improved characteristics for working in alkaline or vice versa, acidic medium. But almost all electrodes have sufficient properties for working in the most popular pH range from pH=1 till pH=12. Special electrodes should be used only for working in aggressive conditions.

Most of text written above is also correct for any ion-exchange electrodes.

1 Construction
2 Storage
3 See also
4 References

[edit] Construction

Scheme of typical pH glass electrode

a sensing part of electrode, a bulb made from a specific glass
sometimes the electrode contains a small amount of AgCl precipitate inside the glass electrode
internal solution, usually 0.1M HCl for pH electrodes or 0.1M MeCl for pMe electrodes
internal electrode, usually silver chloride electrode or calomel electrode
body of electrode, made from non-conductive glass or plastics.
reference electrode, usually the same type as 4
junction with studied solution, usually made from ceramics or capillary with asbestos or quartz fiber.

A typical modern pH probe is a combination electrode, which combines both the glass and reference electrodes into one body. The bottom of a pH electrode balloons out into a round thin glass bulb. The pH electrode is best thought of as a tube within a tube. The inside most tube (the inner tube) contains an unchanging saturated KCl and a 0.1M HCl solution. Also inside the inner tube is the cathode terminus of the reference probe. The anodic terminus wraps itself around the outside of the inner tube and ends with the same sort of reference probe as was on the inside of the inner tube. Both the inner tube and the outer tube contain a reference solution but only the outer tube has contact with the solution on the outside of the pH probe by way of a porous plug that serves as a salt bridge.

This device is essentially a galvanic cell. The reference end is essentially the inner tube of the pH meter, which for obvious reasons cannot lose ions to the surrounding environment (as a reference is good only so long as it stays static through the duration of the measurement). The outer tube contains the medium, which is allowed to mix with the outside environment (and as a consequence this tube must be replenished with a solution of KCl due to ion loss and evaporation).

The measuring part of the electrode, the glass bulb on the bottom, is coated both inside and out with a ~10nm layer of a hydrated gel. These two layers are separated by a layer of dry glass. The silica glass structure (that is, the conformation of its atomic structure) is shaped in such a way that it allows Na⁺ ions some mobility. The metal cations (Na⁺) in the hydrated gel diffuse out of the glass and into solution while H⁺ from solution can diffuse into the hydrated gel. It is the hydrated gel, which makes the pH electrode an ion selective electrode.

H⁺ does not cross through the glass membrane of the pH electrode, it is the Na⁺ which crosses and allows for a change in free energy. When an ion diffuses from a region of activity to another region of activity, there is a free energy change and this is what the pH meter actually measures. The hydrated gel membrane is connected by Na⁺ transport and thus the concentration of H⁺ on the outside of the membrane is 'relayed' to the inside of the membrane by Na⁺.

All glass pH electrodes have extremely high electric resistance from 50 to 500 MOhm. Therefore, the glass electrode can be used only with a high impedance measuring device like a pH meter, or a more universal measuring device - ionometer.

[edit] Storage

Between measurements any glass and membrane electrodes should be kept in the solution of its own ion (Ex. pH glass electrode should be kept in 0.1M HCl or 0.1M H₂SO₄). It is necessary to prevent the glass membrane from drying out.