{"id":6042,"date":"2020-10-13T14:24:44","date_gmt":"2020-10-13T08:54:44","guid":{"rendered":"http:\/\/astan.lk\/al_virtualclassroom\/?p=6042"},"modified":"2020-10-13T14:25:34","modified_gmt":"2020-10-13T08:55:34","slug":"conductivity","status":"publish","type":"post","link":"https:\/\/astan.lk\/al_virtualclassroom\/conductivity\/","title":{"rendered":"Conductivity"},"content":{"rendered":"

\u2022 Strong electrolytes
\nStrong electrolytes are substances that are virtually fully ionized in solution, and include ionic solids and strong acids. As a result of their complete ionization, the concentration of ions in solution is proportional to the concentration of strong electrolyte added.<\/p>\n

eg. NaCl, KNO3<\/sub>, HCl in aqueous solutions<\/p>\n

\u2022 Weak electrolytes
\nWeak electrolytes are not fully ionized in solution. They include weak Bronsted acids and bases.<\/p>\n

eg. CH3<\/sub>COOH, NH3<\/sub>, H2<\/sub>O<\/p>\n

\u2022 Non-electrolytes
\nLiquids\/solutions that do not contain ions are referred as non electrolytes. They do not conduct electricity.<\/p>\n

eg. C6<\/sub>H6<\/sub>, Kerosene<\/p>\n

 <\/p>\n

Conductance and conductivity<\/h4>\n

\"\"<\/a><\/p>\n

A metal cuboid is shown on the left hand side above. A cuboid shape portion of a solution with the similar dimensions of the metal cube which is in between two electrodes is shown on the right hand side.<\/p>\n

Here l = Length of the metal cube or the selected cuboid shape portion of the solution (m)
\nA = Area of cross section (m2<\/sub>)
\nR = Resistance (\u03a9 )
\n\u03c1= Resistivity (\u03a9m )
\n1\/R = Conductance ( \u03a9-1<\/sup> or S )<\/p>\n

Regarding the above cuboids,<\/p>\n

R\u221dl \u00a0 \u00a0 and \u00a0 \u00a0R\u221d (1\/A)<\/p>\n

\u2234 R\u221d(l\/A)<\/p>\n

R =\u00a0\u03c1l\/A<\/p>\n

\u03c1 = RA\/l<\/p>\n

k =1\/\u03c1 = l\/AR<\/p>\n

\u2022 Coherent SI unit of conductivity is and the most practical unit is\u00a0\u03a9-1<\/sup>m-1<\/sup><\/p>\n

\u2022 Conductivity and resistivity are constants for the particular substance (metal or solution with a given concentration) and it changes with temperature (about 2% per one degree Celsius in solution).<\/p>\n

Factors affecting conductivity of a solution<\/h4>\n

\u2022 Nature of the solute (aqueous solutions of strong, weak and non electrolytes, molten electrolytes)
\n\u2022 Concentration of the solute
\n\u2022 Temperature<\/p>\n

\"\"<\/a><\/p>\n

\u2022 For dilute solutions decrease in conductivity is approximately proportional to the concentration and this is very correct for very dilute solutions. The reason is the decrease of interactions among ions in dilution.<\/p>\n

\u2022 Current = Charge \/ Time.
\nCurrent carried by an ion at a given temperature in a given electric field depends on the concentration of ions and their speed. Speed of an ion depends on its charge, size and potential gradient of the applied electric field.<\/p>\n

\u2022 H+<\/sup> and OH–<\/sup> ions have the highest speeds. So those ions contributes a lot for the conductance. For example, H+<\/sup> ions contribute about 80% for the conductance of dilute HCl solution.<\/p>\n","protected":false},"excerpt":{"rendered":"

\u2022 Strong electrolytes Strong electrolytes are substances that are virtually fully ionized in solution, and include ionic solids and strong acids. As a result of their complete ionization, the concentration of ions in solution is proportional to the concentration of strong electrolyte added. eg. NaCl, KNO3, HCl in aqueous solutions \u2022 Weak electrolytes Weak electrolytes […]<\/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-6042","post","type-post","status-publish","format-standard","hentry","category-chemistry","category-unit-14"],"acf":[],"yoast_head":"\nConductivity - Learning & Education Portal<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/astan.lk\/al_virtualclassroom\/conductivity\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Conductivity - Learning & Education Portal\" \/>\n<meta property=\"og:description\" content=\"\u2022 Strong electrolytes Strong electrolytes are substances that are virtually fully ionized in solution, and include ionic solids and strong acids. As a result of their complete ionization, the concentration of ions in solution is proportional to the concentration of strong electrolyte added. eg. 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