{"id":965,"date":"2019-10-14T15:03:03","date_gmt":"2019-10-14T15:03:03","guid":{"rendered":"http:\/\/chemdictionary.org\/?p=965"},"modified":"2019-10-14T15:04:18","modified_gmt":"2019-10-14T15:04:18","slug":"strong-acid","status":"publish","type":"post","link":"https:\/\/chemdictionary.org\/strong-acid\/","title":{"rendered":"Strong Acid"},"content":{"rendered":"\n<h2><strong>Definition<\/strong><\/h2>\n\n\n\n<p>An acid that is completely dissociated in an aqueous solution and loses a proton, which is captured by water to produce hydronium ion [1].<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; HA <sub>(aq)<\/sub>\n\u2192 H<sup>+<\/sup> + A<sup>&#8211;<\/sup><\/p>\n\n\n\n<p>HA=\nprotonated acid<\/p>\n\n\n\n<p>H+\n= free acidic proton<\/p>\n\n\n\n<p>A-\n= conjugate base<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; HA <sub>(aq)<\/sub> +\nH<sub>2<\/sub>O \u2192 H<sub>3<\/sub>O<sup>+<\/sup><sub>(aq)<\/sub> + A<sup>&#8211;<\/sup><sub>(aq)<\/sub><\/p>\n\n\n\n<p>Strong\nacid produces weak conjugate bases. For example, when sulfuric acid dissociate\nwhich is strong acid it produces HSO<sub>4<\/sub>, a conjugate base and gains a negative\ncharge. <\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; H<sub>2<\/sub>SO<sub>4<\/sub>\n\u2192 H<sup>+<\/sup> + HSO<sub>4<\/sub><sup>&#8211;<\/sup><\/p>\n\n\n\n<p><strong>Arrhenius Concept of Acids<\/strong><\/p>\n\n\n\n<p>According\nto Arrhenius concept (1787):<\/p>\n\n\n\n<p>Acid\nis a substance which dissociates in aqueous solution to give hydrogen ions. For\nexample, substances such as HCl, HNO<sub>3<\/sub>, CH<sub>3<\/sub>COOH, HCN, etc.\nare acids because they ionize in aqueous solution to provide H<sup>+<\/sup>\nions.<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; HCl <sub>(aq) <\/sub>\u21cb H<sup>+ <\/sup><sub>(aq) <\/sub>+\nCl<sup>&#8211;<\/sup><sub>(aq)<\/sub><\/p>\n\n\n\n<p><strong>Bronsted- Lowry Concept<\/strong><\/p>\n\n\n\n<p>In\n1923 the Danish chemist Bronsted and the English chemist Lowry independently\npresent their theories of acids and base on the base of proton transfer.\nAccording to this concept:<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; An acid is a substance (molecule or\nion) that can denote a proton (H<sup>+<\/sup>)to another substance.<\/p>\n\n\n\n<p>A\nbase is a substance that can accept a proton (H<sup>+<\/sup>)from\nanother substance.<\/p>\n\n\n\n<p>For\nexample, HCl acts as an acid while Nh<sub>3<\/sub> act as a base. <\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; HCl <sub>(aq)<\/sub>\n+&nbsp;&nbsp; NH<sub>3<\/sub> <sub>(aq)<\/sub>&nbsp;&nbsp;&nbsp; \u21cb&nbsp;&nbsp; NH<sub>4<\/sub><sup>+<\/sup>&nbsp;&nbsp;&nbsp; +&nbsp;&nbsp;\nCl<sup>&#8211;<\/sup> <sub>(aq)<\/sub><\/p>\n\n\n\n<p>Similarly\nwhen HCl dissolves in water, HCl act as an acid and H<sub>2<\/sub>O as a base.<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; HCl <sub>(aq) <\/sub>+\n&nbsp;&nbsp;H<sub>2<\/sub>O&nbsp;&nbsp;&nbsp; \u21cb&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; &nbsp;H<sub>3<\/sub>O<sup>+ <\/sup><sub>(aq)<\/sub> +\nCl<sup>&#8211;<\/sup><\/p>\n\n\n\n<p>Strong\nacid have small pka (logarithmic constant) and large ka (acid dissociation\nconstant). An acid which have less than -2 pka value they are called as strong\nacid. The pka value of acid cannot be measured experimentally. The pka value of\nstrong acids as follow:<\/p>\n\n\n\n<ul><li>Hydroiodic\nacid (HI): pka = -9.3<\/li><li>Hydrobromic\nacid (HBr): pka = -8.7<\/li><li>Perchloroic\nacid (HCIO<sub>4<\/sub>) : pka \u2248 -8<\/li><li>Hydrochloric\nacid (HCl) : pka 1\u2248 -3 (first dissociation only)<\/li><li>\u03a1-\nToluenesulfonic acid : pka =-2.8<\/li><li>Nitric\nacid (HNO<sub>3<\/sub>) : pka \u2248 -1.4<\/li><li>Chloric\nacid (HCIO<sub>3<\/sub>) : pka \u2248 1.0<\/li><\/ul>\n\n\n\n<h2><strong>Factors of Acid strength\ndetermination<\/strong><\/h2>\n\n\n\n<p>There\nare some factors on which strong acid dissociate in water so well and weak acid\ndo not completely dissociate [2]. These factors are as follow:<\/p>\n\n\n\n<p><strong>Atomic radius<\/strong><\/p>\n\n\n\n<p>Acidity\nof an acid increases with the increase in atomic radius. Like: HI is strong\nacid than HCl.<\/p>\n\n\n\n<p><strong>Electronegativity<\/strong><\/p>\n\n\n\n<p>Acidity\nof an acid is increases from left to right in the periodic table.<\/p>\n\n\n\n<p><strong>Electrical charge<\/strong><\/p>\n\n\n\n<p>The\natom which have positive charge has higher acidity as compare to the atom which\ncarry negative charge.<\/p>\n\n\n\n<p><strong>Resonance<\/strong><\/p>\n\n\n\n<p>An\nanions which have resonance structure are more acidic in nature than anion\nwhich don\u2019t have.<\/p>\n\n\n\n<p><strong>Hybridization <\/strong><\/p>\n\n\n\n<p>Strong\nacid follows the following hybridization sequence sp \u02c3 sp<sup>2<\/sup> \u02c3 sp<sup>3<\/sup>.\nIf arrangement of electron is different it will affect the acidity.<\/p>\n\n\n\n<p><strong>Solvent<\/strong><\/p>\n\n\n\n<p>Mostly\nstrong acid dissociate in water but acetic acid ionize completely in liquid\nammonia as compare to water, it is weak acid in water.<\/p>\n\n\n\n<p><strong>Hydroiodic Acid <\/strong><\/p>\n\n\n\n<p>It is a highly acidic aqueous solution of hydrogen and iodide. It is strong acid that ionize completely in an aqueous solution. Hydroiodic acid quickly reacts with oxygen in the air and produce water and iodide. It is also carried out addition reactions with unsaturated hydrocarbons i.e alkene like halogens. Hydroiodic acid is major component of cativa process which is used as co-catalyst for the production of acetic acid through carbonylation of methanol [3]. It is also used as a reducing agent in the production of methamphetamine from pseudoephedrine.<\/p>\n\n\n\n<p><strong>Hydrobromic Acid<\/strong><\/p>\n\n\n\n<p>It\nis formed by dissolving hydrogen bromide in water. Due to constant boiling in\naqueous solution at 124.3<sup>o<\/sup> C it contain 47.6% HBr by mass. It is\nalso known as mineral acid. It is used for the production of inorganic bromides\nlike bromides of calcium, zinc and sodium. It also carried out catalyzation of\nalkylation and used in extraction of ores. It is main reagent for preparation\nof organobromine compounds. It is prepared by reacting bromine with either\nsulfur or phosphorus and water [4]. It can be prepared by diluting sulfuric\nacid and potassium bromide.<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; H<sub>2<\/sub>SO<sub>4<\/sub>\n+KBr \u2192 KHSO<sub>4<\/sub> + HBr<\/p>\n\n\n\n<p><strong>Perchloric Acid<\/strong><\/p>\n\n\n\n<p>It\nis also mineral acid. It is colorless and stronger than sulfuric acid and\nnitric acid. When hot it is a strong powerful oxidizer. But in aqueous\nsolutions it shows only strong acid features and no oxidizing properties. It is\nuseful in preparation of perchlorate salts like ammonium perchlorate. It is\ndangerously corrosive in nature and form explosive mixtures. It is prepared by\ntwo methods one is traditional method in which aqueous solubility of sodium\nperchlorate is treated with hydrochloric acid which gives perchloric acid and\nsodium chloride. Other method is anodic oxidation of aqueous chlorine at\nplatinum electrode. It is used in rocket fuel. It is also useful in etching of\nchrome.<\/p>\n\n\n\n<p><strong>Hydrochloric Acid<\/strong><\/p>\n\n\n\n<p>It\nis a colorless inorganic compound. It has distinctive pungent smell. It is main\ncomponent of gastric acid which is produced in digestive system of animal\nspecies including human being. It is used in leather processing. Hydrochloric\nacid was discovered by Jabir ibn Hayyan in 800 AD. It is prepared by dissolving\nhydrogen chloride in water. It is used in industrial processes like refining\nmetal. It is also used in purification of common salt. In concentrated form it\nforms acidic mist which has corrosive effect on human tissue, respiratory\norgans, eyes, skin and intestines.<\/p>\n\n\n\n<p><strong>\u03c1- Toluenesulfonic acid <\/strong><\/p>\n\n\n\n<p>It\nis white solid soluble in water, alcohol and polar organic solvent. TsOH is one\nmillion times stronger than benzoic acid. It is prepared on industrial scale\nthrough sulfonation of toluene. It is used in esterification of carboxylic\nacid. Also used in Trans- esterification of an ester. Tosylates is used for\nprotection for alcohols. Reduction of toyslate ester produce hydrocarbons [5]. <\/p>\n\n\n\n<p><strong>Nitric Acid <\/strong><\/p>\n\n\n\n<p>It\nis also known as <em>aqua fortis<\/em> (strong\nwater). Nitric acid is highly corrosive mineral acid. In pure form it is\ncolorless but acquire a yellow cast in older sample due to decomposition into\noxides of nitrogen and water. Commercially its concentration in water is 68%.\nWhen its concentration is 68% in a solution it is called as fuming nitric acid\nIt is primary reagent for nitration, some nitro compounds are stable enough so\ncan be used in munitions and demolition. While some are sensitive shock and\nthermally explosives, other are more stable to be used as pigments, inks and\ndyes. Nitric acid react with metals like magnesium, manganese and zinc liberate\nH<sub>2<\/sub>. Some metals gold and platinum do not react with nitric acid.\nNitric acid is prepared by reacting nitrogen dioxide with water. Its main use\nis production of fertilizers. Nitric acid give ammonium nitrate through\nneutralization with ammonia. Also used in production of explosives, nylon\nprecursors and organic compounds. It is used as oxidizer in liquid fueled\nrockets. Nitric acid used in food finishing. Its strong corrosive nature and\noxidizing power it produce acid hydrolysis with protein and fats which\ndecompose living tissue like skin and flesh.<\/p>\n\n\n\n<p><strong>Chloric Acid<\/strong><\/p>\n\n\n\n<p>Chloric\nacid is strong unstable oxidizing acid in nature. It is oxoacids of chlorine.\nChloric acid is colorless and its density is similar with water but it has\npungent smell. It is strong acid, react with base and form chlorate salts.\nChloric acid is prepared by reacting barium chloride with sulfuric acid.\nReducing agents like sodium or potassium metabisulfite is used to neutralize\nchloric acid. Chloric acid is used to perchloric acid. It is also used for\nfireworks i.e. strontium chlorate for red, calcium chlorate for orange [6].<\/p>\n\n\n\n<p><strong>pH Scale <\/strong><\/p>\n\n\n\n<p>Concentration\nof hydrogen ion [H<sup>+<\/sup>] in pure water is the basis for the pH scale.\nWater is a weak electrolyte because it ionizes very slightly into ions in a\nprocess called auto-ionization or self-ionization.<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; H<sub>2<\/sub>O&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; \u21cb&nbsp;&nbsp;&nbsp; H<sup>+<\/sup>&nbsp;&nbsp;&nbsp; +&nbsp;&nbsp;&nbsp;&nbsp;\nOH<sup>_<\/sup><\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; The equilibrium expression of this\nreaction may be written as <\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; K<sub>C<\/sub>\n=&nbsp;&nbsp;&nbsp; [H<sup>+<\/sup>] [OH<sup>&#8211;<\/sup>]<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;\n[H<sub>2<\/sub>O]&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; <\/p>\n\n\n\n<p><strong>Reference <\/strong><\/p>\n\n\n\n<p>1.\n<a href=\"https:\/\/www.thoughtco.com\/definition-of-strong-acid-604663\" target=\"_blank\" rel=\"noopener\">https:\/\/www.thoughtco.com\/definition-of-strong-acid-604663<\/a><\/p>\n\n\n\n<p>2.<a href=\"http:\/\/cssac.unc.edu\/programs\/learning-center\/Resources\/Study\/Guides\/topics-and-concepts-of-organic-chemistry-262\/factors-that-affect-acidity\" target=\"_blank\" rel=\"noopener\">http:\/\/cssac.unc.edu\/programs\/learning-center\/Resources\/Study\/Guides\/topics-and-concepts-of-organic-chemistry-262\/factors-that-affect-acidity<\/a><\/p>\n\n\n\n<p>3.\nJones, J.\nH. (2000).&nbsp;<a href=\"http:\/\/www.platinummetalsreview.com\/pdf\/pmr-v44-i3-094-105.pdf\" target=\"_blank\" rel=\"noopener\">&#8220;The Cativa<sup>TM<\/sup>&nbsp;Process for the\nManufacture of Acetic Acid&#8221;<\/a>&nbsp;(PDF).&nbsp;<a href=\"https:\/\/en.wikipedia.org\/wiki\/Platinum_Metals_Rev.\" target=\"_blank\" rel=\"noopener\"><em>Platinum Metals Rev.<\/em><\/a>&nbsp;<strong>44<\/strong>&nbsp;(3):\n94\u2013105.<\/p>\n\n\n\n<p>4. <a href=\"https:\/\/en.wikipedia.org\/wiki\/Hydrobromic_acid\" target=\"_blank\" rel=\"noopener\">https:\/\/en.wikipedia.org\/wiki\/Hydrobromic_acid<\/a><\/p>\n\n\n\n<p>5.\nhttps:\/\/en.wikipedia.org\/wiki\/P-Toluenesulfonic_acid<\/p>\n\n\n\n<p>6.\nhttp:\/\/www.sciencemadness.org\/smwiki\/index.php\/Chloric_acid<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Definition An acid that is completely dissociated in an aqueous solution and loses a proton, which is captured by water to produce hydronium ion [1]. &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; HA (aq) \u2192 H+ + A&#8211; HA= protonated acid H+ = free acidic proton A- = conjugate base &nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; HA (aq) + H2O \u2192 H3O+(aq) + A&#8211;(aq) Strong acid &#8230; <a title=\"Strong Acid\" class=\"read-more\" href=\"https:\/\/chemdictionary.org\/strong-acid\/\" aria-label=\"More on Strong Acid\">Read more<\/a><\/p>\n","protected":false},"author":6,"featured_media":0,"comment_status":"closed","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"rating_form_position":"","rating_results_position":"","mr_structured_data_type":""},"categories":[2],"tags":[],"multi-rating":{"mr_rating_results":[{"adjusted_star_result":0,"star_result":0,"total_max_option_value":5,"adjusted_score_result":0,"score_result":0,"percentage_result":0,"adjusted_percentage_result":0,"count":0,"post_id":965}]},"_links":{"self":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/965"}],"collection":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/users\/6"}],"replies":[{"embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/comments?post=965"}],"version-history":[{"count":3,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/965\/revisions"}],"predecessor-version":[{"id":990,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/965\/revisions\/990"}],"wp:attachment":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/media?parent=965"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/categories?post=965"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/tags?post=965"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}