\u2022 The value of the potential of a given electrode under standard conditions measured relative to the standard hydrogen electrode (SHE) is its standard electrode potential.<\/p>\n
\u2022 The following diagram illustrates a set up that can be used for measuring the standard electrode potential of the Zn2+<\/sup> (aq)|Zn(s) electrode.<\/p>\n <\/p>\n <\/p>\n \u2022 When the standard electrode potentials (reduction potential) of different electrodes are arranged in the ascending order, the electrochemical series is obtained.<\/p>\n Factors affecting the electrode potential<\/strong> \u2022 Electromotive force (e.m.f.) is defined as the potential difference between the two electrodes when no current flows through the cell.<\/p>\n \u2022 Temperature, concentration of the electrolyte, electrode type and the nature of the electrolyte are the factors that affect the electromotive force. It is independent of the distance betweenthe electrodes and the surface area of the electrodes.<\/p>\n \u2022 Electrolytes in the two electrodes of an electrochemical cell are connected to complete the internal circuit through a salt bridge or a permeable membrane\/diaphragm\/porous partition.A tube filled with a solution of a salt such as KCl or NH4<\/sub>NO3<\/sub> which is gelified with agar is used as a salt bridge. Such an electrochemical cell is known as a cell with a liquid junction.<\/p>\n \u2022 In a cell, when both electrodes are not separated by a salt bridge or a permeable membrane\/diaphragm\/porous partition is referred as a cell without a liquid junction.<\/p>\n \u2022 According to the international convention, electrode potentials are measured relative to the standard hydrogen electrode. On this standard, the electrode potential of the standard silver-silver chloride electrode is 0.22 V. Similarly, the electrode potentials of other standard electrodes can also be calculated. Show that in arranging these in the ascending order, electrochemical series is obtained.<\/p>\n Ecell<\/sub> = Ecathode<\/sub> – Eanode<\/sub><\/strong><\/p>\n","protected":false},"excerpt":{"rendered":" \u2022 The potential difference in the double layer of a given electrode is considered its electrode potential. This absolute difference cannot be measured. It can only be measured relative to another electrode. \u2022 An electrode with a known or a defined potential used to measure the potential of a given electrode is called a reference […]<\/p>\n","protected":false},"author":842,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"_monsterinsights_skip_tracking":false,"_monsterinsights_sitenote_active":false,"_monsterinsights_sitenote_note":"","_monsterinsights_sitenote_category":0,"footnotes":""},"categories":[14,1678],"tags":[],"class_list":["post-6046","post","type-post","status-publish","format-standard","hentry","category-chemistry","category-unit-14"],"acf":[],"yoast_head":"\n![](\"http:\/\/www.chemhume.co.uk\/A2CHEM\/Unit%202c\/2%20Electrode%20pots\/measuring_standard_electrode_potential.jpg\")
<\/p>\n
\n\u2022 Temperature
\n\u2022 Concentration of the electrolyte
\n\u2022 Nature of electrolyte
\n\u2022 Pressure (of a gas)
\n\u2022 Type of electrode<\/p>\n