{"id":50521,"date":"2023-12-02T20:53:00","date_gmt":"2023-12-02T15:08:00","guid":{"rendered":"https:\/\/thechemistrynotes.com\/?p=50521"},"modified":"2023-12-20T21:04:38","modified_gmt":"2023-12-20T15:19:38","slug":"perchloric-acid-preparation-properties-uses","status":"publish","type":"post","link":"https:\/\/thechemistrynotes.com\/perchloric-acid-preparation-properties-uses\/","title":{"rendered":"Perchloric Acid: Preparation, Properties, Uses, Health Hazards"},"content":{"rendered":"\n<figure class=\"wp-block-image size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"1205\" height=\"631\" src=\"https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/12\/Perchloric-acid.jpg\" alt=\"Perchloric acid\" class=\"wp-image-50524\" srcset=\"https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/12\/Perchloric-acid.jpg 1205w, https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/12\/Perchloric-acid-300x157.jpg 300w, https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/12\/Perchloric-acid-1024x536.jpg 1024w, https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/12\/Perchloric-acid-768x402.jpg 768w\" sizes=\"(max-width: 1205px) 100vw, 1205px\" \/><\/figure>\n\n\n\n<p>Perchloric acid is the chemical name for chlorine oxoacid. It is also known as hydroxidotrioxidochlorine or hyperchloric acid (HClO<sub>4<\/sub>). Acid is a transparent, colorless, and odorless aqueous solution with a concentration ranging from 50% to 72%. It corrodes metals and tissues. Closed containers can violently rupture when exposed to heat for an extended period.<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"107\" height=\"115\" src=\"https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/12\/image-43.png\" alt=\"\" class=\"wp-image-50523\" \/><\/figure><\/div>\n\n\n<p>HClO<sub>4<\/sub> is a chemical that is similar to sulfuric acid in many ways. It is a strong acid with a high boiling point that is particularly stable in solution. It has several advantages over sulfuric acid, such as being monobasic and having a low concentration of insoluble ions.<\/p>\n\n\n\n<p>It is a colorless, odorless, and oily corrosive inorganic liquid. It is miscible with water, has a boiling temperature of 203 <sup>O<\/sup>C, a melting point of 19 degrees Celsius, and a low vapor pressure of 6.8 mm Hg at 25 <sup>O<\/sup>C. A cool 70% aqueous perchloric acid solution is a strong acid or superacid (stronger than sulfuric and nitric acids), however,&nbsp;it is not always a strong oxidizing agent. However, when perchloric acid concentration and temperature rise, so does its oxidizing power.<\/p>\n\n\n\n<p>Because perchloric acid is highly reactive, it must be stored apart from other chemicals, especially organic solvents, organic acids, and reducing agents. All Perchloric acid containers should be tested regularly&nbsp;for container integrity and discoloration. Perchloric acid that has become discolored should be disposed of&nbsp;as hazardous waste. Perchloric acid should be used and kept in an area away from combustible items and wooden furniture.<\/p>\n\n\n\n<div id=\"ez-toc-container\" class=\"ez-toc-v2_0_63 counter-hierarchy ez-toc-counter ez-toc-custom ez-toc-container-direction\">\n<div class=\"ez-toc-title-container\">\n<p class=\"ez-toc-title \" >Table of Contents<\/p>\n<span class=\"ez-toc-title-toggle\"><a href=\"#\" class=\"ez-toc-pull-right ez-toc-btn ez-toc-btn-xs ez-toc-btn-default ez-toc-toggle\" aria-label=\"Toggle Table of Content\"><span class=\"ez-toc-js-icon-con\"><span class=\"\"><span class=\"eztoc-hide\" style=\"display:none;\">Toggle<\/span><span class=\"ez-toc-icon-toggle-span\"><svg style=\"fill: #0a0a0a;color:#0a0a0a\" xmlns=\"http:\/\/www.w3.org\/2000\/svg\" class=\"list-377408\" width=\"20px\" height=\"20px\" viewBox=\"0 0 24 24\" fill=\"none\"><path d=\"M6 6H4v2h2V6zm14 0H8v2h12V6zM4 11h2v2H4v-2zm16 0H8v2h12v-2zM4 16h2v2H4v-2zm16 0H8v2h12v-2z\" fill=\"currentColor\"><\/path><\/svg><svg style=\"fill: #0a0a0a;color:#0a0a0a\" class=\"arrow-unsorted-368013\" xmlns=\"http:\/\/www.w3.org\/2000\/svg\" width=\"10px\" height=\"10px\" viewBox=\"0 0 24 24\" version=\"1.2\" baseProfile=\"tiny\"><path d=\"M18.2 9.3l-6.2-6.3-6.2 6.3c-.2.2-.3.4-.3.7s.1.5.3.7c.2.2.4.3.7.3h11c.3 0 .5-.1.7-.3.2-.2.3-.5.3-.7s-.1-.5-.3-.7zM5.8 14.7l6.2 6.3 6.2-6.3c.2-.2.3-.5.3-.7s-.1-.5-.3-.7c-.2-.2-.4-.3-.7-.3h-11c-.3 0-.5.1-.7.3-.2.2-.3.5-.3.7s.1.5.3.7z\"\/><\/svg><\/span><\/span><\/span><\/a><\/span><\/div>\n<nav><ul class='ez-toc-list ez-toc-list-level-1 ' ><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-1\" href=\"https:\/\/thechemistrynotes.com\/perchloric-acid-preparation-properties-uses\/#preparation-of-perchloric-acid\" title=\"Preparation of Perchloric acid\">Preparation of Perchloric acid<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-2\" href=\"https:\/\/thechemistrynotes.com\/perchloric-acid-preparation-properties-uses\/#properties-of-perchloric-acid\" title=\"Properties of Perchloric acid\">Properties of Perchloric acid<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-3\" href=\"https:\/\/thechemistrynotes.com\/perchloric-acid-preparation-properties-uses\/#uses-of-perchloric-acid\" title=\"Uses &nbsp;of Perchloric acid\">Uses &nbsp;of Perchloric acid<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-4\" href=\"https:\/\/thechemistrynotes.com\/perchloric-acid-preparation-properties-uses\/#health-hazards-of-perchloric-acid\" title=\"Health Hazards of perchloric acid\">Health Hazards of perchloric acid<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-5\" href=\"https:\/\/thechemistrynotes.com\/perchloric-acid-preparation-properties-uses\/#precautions-to-be-taken-while-using-perchloric-acid\" title=\"Precautions to be taken while using perchloric acid\">Precautions to be taken while using perchloric acid<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-6\" href=\"https:\/\/thechemistrynotes.com\/perchloric-acid-preparation-properties-uses\/#references\" title=\"References\">References<\/a><\/li><\/ul><\/nav><\/div>\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"preparation-of-perchloric-acid\"><\/span><strong>Preparation of Perchloric acid<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<p>\u00a0Treating\u00a0sodium perchlorate solution with <a href=\"https:\/\/thechemistrynotes.com\/hydrochloric-acid-preparation-properties\/\">hydrochloric acid (<\/a>HCl) produces HClO<sub>4<\/sub> by precipitating solid sodium chloride. The chemical equation for the same is given as follows:<\/p>\n\n\n\n<p>NaClO<sub>4<\/sub>&nbsp;+ HCl \u2192 NaCl + HClO<sub>4<\/sub><\/p>\n\n\n\n<p>The reaction of NH<sub>4<\/sub>ClO<sub>4<\/sub> and HNO<sub>3<\/sub> also produces HClO<sub>4<\/sub>.<\/p>\n\n\n\n<p>NH<sub>4<\/sub>ClO<sub>4<\/sub>&nbsp;+ HNO<sub>3<\/sub> \u2192&nbsp; HClO<sub>4<\/sub> + NH<sub>4<\/sub>NO<sub>3<\/sub><\/p>\n\n\n\n<p>HClO<sub>4 <\/sub>is commercially available as 70% HClO<sub>4<\/sub>, Which has almost the composition of dihydrate HClO<sub>4<\/sub>. 2 H<sub>2<\/sub>O. It is only oxyacid of chlorine that can be isolated in anhydrous form. Its anhydrous form is made by dehydrating HClO<sub>4<\/sub>. 2 H<sub>2<\/sub>O with fuming sulphuric acid, other separating HClO4 by vacuum distillation.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"properties-of-perchloric-acid\"><\/span><strong>Properties of<\/strong> <strong>Perchloric acid<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li>It is the strongest acid known.<\/li>\n\n\n\n<li>The anhydrous form is a powerful oxidizing agent that explodes on contact with organic materials (wool, paper, cloth, grease rubber, or chemicals) and sometimes on its own.<\/li>\n\n\n\n<li>Hot concentrated solutions have been used for wet ashing where all organic materials in the sample are oxidized to CO<sub>2<\/sub>, leaving only the inorganic constituents for analysis.<\/li>\n\n\n\n<li>On dehydration with P<sub>2<\/sub>O<sub>5, <\/sub>it gives Cl<sub>2<\/sub>O<sub>7<\/sub>.<\/li>\n<\/ul>\n\n\n\n<p>2 HClO<sub>4<\/sub> + P<sub>2<\/sub>O<sub>5<\/sub> &nbsp;&nbsp;\u2192&nbsp;&nbsp; Cl<sub>2<\/sub>O<sub>7<\/sub> + 2 HPO<sub>3<\/sub><\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"uses-of-perchloric-acid\"><\/span><strong>Uses &nbsp;of Perchloric acid<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li>The primary application of HClO<sub>4<\/sub> is as a precursor to ammonium perchlorate, an inorganic chemical that is an essential part of rocket fuel. As a result, perchloric acid is regarded as a more critical chemical molecule in the space industry.<\/li>\n\n\n\n<li>The same compound can also be utilized in the etching of Liquid Crystal Display (LCD) systems.\u00a0As a result, HClO<sub>4<\/sub> is now widely used in the electronics\u00a0industry.<\/li>\n\n\n\n<li>HClO<sub>4<\/sub> is used as an oxidizer in the separation of sodium and potassium.<\/li>\n\n\n\n<li>It is used in the manufacture of explosives.<\/li>\n\n\n\n<li>It is used for metal plating.<\/li>\n\n\n\n<li>It is employed as a reagent in the determination of 1H-Benzotriazole.<\/li>\n\n\n\n<li>It serves as a catalyst.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"health-hazards-of-perchloric-acid\"><\/span><strong>Health Hazards of perchloric acid<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<p>Inhaling the vapors of this specific molecule induces a burning sensation in the nose and throat, as well as lung irritation and coughing. When exposed to this substance over an extended period, it produces vomiting. This can induce burning and gastrointestinal burns if consumed. When heated, this chemical emits unpleasant, corrosive, and poisonous fumes.<\/p>\n\n\n\n<p>HClO<sub>4<\/sub> is regarded as a particularly potent oxidant. Because of its highly oxidizing characteristics, this molecule has extremely high reactivities towards the majority of metals. Furthermore, this chemical is extremely reactive to organic materials. This substance is corrosive to human skin. As a result, proper precautions should be taken when handling this combination.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"precautions-to-be-taken-while-using-perchloric-acid\"><\/span><strong>Precautions to be taken while using perchloric acid<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li>HClO<sub>4<\/sub> digestions and other high-temperature treatments must be carried out in specially built perchloric acid fume hoods.<\/li>\n\n\n\n<li>Never use an open flame or an oil bath to heat perchloric acid. It is preferable to use electric hot plates, electrically or steam-heated sand baths, heating mantles, or steam baths.<\/li>\n\n\n\n<li>Allowing heated HClO<sub>4<\/sub> to come into touch with organic compounds is not recommended. Avoid using perchloric acid-incompatible greases.<\/li>\n\n\n\n<li>Do not distill HClO<sub>4<\/sub> in a vacuum because an unstable anhydride may form, resulting in a spontaneous explosion.<\/li>\n\n\n\n<li>Vacuum pumps should be fully cleansed and refilled with Kel-F or Fluorolube before using perchloric acid.<\/li>\n\n\n\n<li>Following the operating instructions provided by the maker of the perchloric acid hood, wash down perchloric acid hoods after each usage.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"references\"><\/span><strong>References<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li>https:\/\/byjus.com\/chemistry\/perchloric-acid\/.<\/li>\n\n\n\n<li>https:\/\/www.sciencedirect.com\/topics\/chemistry\/perchloric-acid.<\/li>\n\n\n\n<li>https:\/\/www.vedantu.com\/chemistry\/perchloric-acid.<\/li>\n\n\n\n<li>https:\/\/safety.fsu.edu\/safety_manual\/supporting_docs\/Perchloric%20Acid%20Safety.pdf<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Perchloric acid is the chemical name for chlorine oxoacid. It is also known as hydroxidotrioxidochlorine or hyperchloric acid (HClO4). Acid is a transparent, colorless, and odorless aqueous solution with a &#8230; <a title=\"Perchloric Acid: Preparation, Properties, Uses, Health Hazards\" class=\"read-more\" href=\"https:\/\/thechemistrynotes.com\/perchloric-acid-preparation-properties-uses\/\" aria-label=\"Read more about Perchloric Acid: Preparation, Properties, Uses, Health Hazards\">Read more<\/a><\/p>\n","protected":false},"author":4,"featured_media":50524,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[24],"tags":[3143,3140,3141,3142],"_links":{"self":[{"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/posts\/50521"}],"collection":[{"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/users\/4"}],"replies":[{"embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/comments?post=50521"}],"version-history":[{"count":2,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/posts\/50521\/revisions"}],"predecessor-version":[{"id":50525,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/posts\/50521\/revisions\/50525"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/media\/50524"}],"wp:attachment":[{"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/media?parent=50521"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/categories?post=50521"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/tags?post=50521"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}