{"id":50395,"date":"2023-12-07T14:12:51","date_gmt":"2023-12-07T08:27:51","guid":{"rendered":"https:\/\/thechemistrynotes.com\/?p=50395"},"modified":"2023-12-07T14:12:55","modified_gmt":"2023-12-07T08:27:55","slug":"potassium-permanganate-preparation-reaction","status":"publish","type":"post","link":"https:\/\/thechemistrynotes.com\/potassium-permanganate-preparation-reaction\/","title":{"rendered":"Potassium Permanganate: \u00a0Preparation, Structure, Properties, Reactions, Health effects"},"content":{"rendered":"\n<figure class=\"wp-block-image size-large\"><img loading=\"lazy\" decoding=\"async\" width=\"1024\" height=\"536\" src=\"https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/12\/potassium-permanganate-1024x536.jpg\" alt=\"potassium permanganate\" class=\"wp-image-50398\" srcset=\"https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/12\/potassium-permanganate-1024x536.jpg 1024w, https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/12\/potassium-permanganate-300x157.jpg 300w, https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/12\/potassium-permanganate-768x402.jpg 768w, https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/12\/potassium-permanganate.jpg 1205w\" sizes=\"(max-width: 1024px) 100vw, 1024px\" \/><\/figure>\n\n\n\n<p>Potassium permanganate is a chemical compound with the chemical formula KMnO<sub>4<\/sub>. It is a manganic acid potassium salt. It is&nbsp;also known as Condy&#8217;s crystals or potash permanganate.<\/p>\n\n\n\n<p>Johann Rudolf Glauber, a German-Dutch chemist, was the first to discover the &nbsp;KMnO<sub>4<\/sub> in 1659. This water-soluble molecule is made up of two ions: permanganate ion and potassium ion. In its physical state, it is a dark purple odorless solid.<\/p>\n\n\n\n<p>When potassium permanganate crystals are dissolved in water, a purple solution is generated. It is a potent oxidizing agent that does not produce harmful byproducts. It&#8217;s frequently made from other minerals like manganese oxide. Firstly, It was invented as a disinfectant. It has since been widely used to treat a wide range of skin diseases, including fungal infections.<\/p>\n\n\n\n<div id=\"ez-toc-container\" class=\"ez-toc-v2_0_65 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\/potassium-permanganate-preparation-reaction\/#preparation-of-potassium-permanganate\" title=\"Preparation of potassium permanganate\">Preparation of potassium permanganate<\/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\/potassium-permanganate-preparation-reaction\/#structure-of-potassium-permanganate\" title=\"Structure of potassium permanganate\">Structure of potassium permanganate<\/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\/potassium-permanganate-preparation-reaction\/#physical-properties-of-potassium-permanganate\" title=\"Physical properties of potassium permanganate\">Physical properties of potassium permanganate<\/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\/potassium-permanganate-preparation-reaction\/#chemical-properties-of-potassium-permanganate\" title=\"Chemical properties of potassium permanganate\">Chemical properties of potassium permanganate<\/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\/potassium-permanganate-preparation-reaction\/#reactions-of-potassium-permanganate\" title=\"Reactions of potassium permanganate\">Reactions of potassium permanganate<\/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\/potassium-permanganate-preparation-reaction\/#uses-of-potassium-permanganate\" title=\"Uses of potassium permanganate\">Uses of potassium permanganate<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-7\" href=\"https:\/\/thechemistrynotes.com\/potassium-permanganate-preparation-reaction\/#health-effects-of-potassium-permanganate\" title=\"Health effects of Potassium permanganate\">Health effects of Potassium permanganate<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-8\" href=\"https:\/\/thechemistrynotes.com\/potassium-permanganate-preparation-reaction\/#references\" title=\"References\">References<\/a><\/li><\/ul><\/nav><\/div>\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"preparation-of-potassium-permanganate\"><\/span><strong>Preparation of potassium permanganate<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<p>Potassium manganate is made by mixing a solution of potassium hydroxide and powdered manganese oxide with oxidizing agents such as potassium chlorate. After boiling and evaporating this mixture, the residue is heated in iron pans until it becomes pasty.<\/p>\n\n\n\n<p class=\"has-text-align-center has-accent-color has-text-color has-link-color wp-elements-f1ce4e3ff79e0b0b21e2d519cd69032b\">6 KOH + 3 MnO<sub>2<\/sub>\u00a0+ 6 KClO<sub>3<\/sub>\u00a0\u2192 3 K<sub>2<\/sub>MnO<sub>4<\/sub>\u00a0+ 6 KCl + 3 H<sub>2<\/sub>O<\/p>\n\n\n\n<ul>\n<li>The resulting potassium manganate (green) is heated in a large amount of water, and a current of chlorine, CO<sub>2<\/sub>, and ozonized air is pushed through the liquid until it is transformed into permanganate. The generated MnO2 is continuously removed to prevent it from degrading the permanganate.<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-accent-color has-text-color has-link-color wp-elements-1aa51a8adf49679029d2279b74cd8dbf\">6 K<sub>2<\/sub>MnO<sub>4<\/sub>\u00a0+ 3 Cl<sub>2<\/sub>\u00a0\u2192\u00a06 KMnO<sub>4\u00a0<\/sub>\u00a0+ 6 KCl3<\/p>\n\n\n\n<ul>\n<li>Reaction of potassium manganate with HCl to form potassium permanganate.<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-accent-color has-text-color has-link-color wp-elements-f576263cf9d5e581f97e206bddaa9a28\">2K<sub>2<\/sub>MnO<sub>4<\/sub>&nbsp;+ 4HCl&nbsp; \u2192&nbsp; 2KMnO<sub>4<\/sub>&nbsp; + H<sub>2<\/sub>O + MnO<sub>2<\/sub>&nbsp;+ 4KCl<strong><\/strong><\/p>\n\n\n\n<ul>\n<li>Reaction of potassium manganate with H<sub>2<\/sub>SO<sub>4<\/sub> to form potassium permanganate.<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-accent-color has-text-color has-link-color wp-elements-9e814ee921d4b083fd18a9128e65770e\">3 K<sub>2<\/sub>MnO<sub>4<\/sub>&nbsp;+ 2H<sub>2<\/sub>SO<sub>4<\/sub>&nbsp; &nbsp; \u2192&nbsp; 2KMnO<sub>4<\/sub>&nbsp; + 2H<sub>2<\/sub>O + MnO<sub>2<\/sub>&nbsp;+ 2K<sub>2<\/sub>SO<sub>4<\/sub><strong><\/strong><\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"structure-of-potassium-permanganate\"><\/span><strong>Structure of potassium permanganate<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<p>KMnO<sub>4<\/sub> is an inorganic ionic compound composed of the ions K<sup>+<\/sup> and MnO<sub>4<\/sub><sup>&#8211;<\/sup>. In the permanganate anionMnO<sup>4-<\/sup> three double bonds and one single link connect the manganese atom to four oxygen atoms. Manganese has an oxidation state of + 7 in this salt. MnO<sup>4-<\/sup> ion hybridisation yields d<sup>3<\/sup>s (orbitals used are 3dxy, 3dyz, 3dzx, and 4s).<\/p>\n\n\n\n<p>Tetrahedral geometry results from d<sup>3<\/sup>s hybridization. As a result, the Tetrahedral geometry of MnO<sup>4-<\/sup> can be expressed as<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"283\" height=\"240\" src=\"https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/12\/image-24.png\" alt=\"\" class=\"wp-image-50396\" \/><\/figure><\/div>\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"physical-properties-of-potassium-permanganate\"><\/span><strong>Physical properties of potassium permanganate<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li>It is a crystalline solid that ranges in color from purple to magenta and has no odor.<\/li>\n\n\n\n<li>It is soluble in water, acetone, acetic acid, methanol, and pyridine.<\/li>\n\n\n\n<li>It is soluble in ethanol as well as organic solvents.<\/li>\n\n\n\n<li>It occurs as monoclinic prisms that are almost opaque and have a blue metallic luster.<\/li>\n\n\n\n<li>It has no odor and a sweetish astringent taste in its aqueous solution. It is water-soluble and becomes more soluble in boiling water.<\/li>\n\n\n\n<li>It has a density of 2.7g\/ml and its molar mass is 158.034g\/mol.<\/li>\n\n\n\n<li>It has a high melting point of 240<sup>0<\/sup> C.<\/li>\n\n\n\n<li>Potassium permanganate has a boiling point of 100\u00b0C.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"chemical-properties-of-potassium-permanganate\"><\/span><strong>Chemical properties of potassium permanganate<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li>Potassium permanganate is a powerful oxidizing agent that can be utilized in a wide range of chemical processes.<\/li>\n\n\n\n<li>During a redox reaction, the dark purple solution turns colorless and eventually brown, demonstrating potassium permanganate&#8217;s oxidizing power.<\/li>\n\n\n\n<li>This reaction might take place in an acidic or basic media.<\/li>\n\n\n\n<li>It is not combustible but aids in the combustion of other chemicals.<\/li>\n\n\n\n<li>It is a highly stable chemical under normal conditions, but upon heating it decomposes to generate MnO2 and liberates oxygen.<\/li>\n\n\n\n<li>It explodes when it comes into contact with sulfuric acid.<\/li>\n\n\n\n<li>It instantly interacts with glycerol and simple <a href=\"https:\/\/thechemistrynotes.com\/alcohols\/\">alcohol<\/a>s, producing flame and smoke.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"reactions-of-potassium-permanganate\"><\/span><strong>Reactions of potassium permanganate<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li><strong>Decomposition reaction<\/strong><\/li>\n<\/ul>\n\n\n\n<p>When heated, potassium permanganate undergoes thermal decomposition.<\/p>\n\n\n\n<p class=\"has-text-align-center has-accent-color has-text-color has-link-color wp-elements-4ae9280f035fc450a5639c98c62088ba\">2 KMnO<sub>4<\/sub> \u2192 K<sub>2<\/sub>MnO<sub>4<\/sub> + MnO<sub>2<\/sub> + O<sub>2<\/sub><\/p>\n\n\n\n<ul>\n<li><strong>Reaction with acid<\/strong><\/li>\n<\/ul>\n\n\n\n<p>When permanganate combines with strong hydrochloric acid, chlorine is formed. When potassium permanganate is reduced to an alkaline solution, it transforms into green K<sub>2<\/sub>MnO<sub>4<\/sub><strong>.<\/strong><\/p>\n\n\n\n<p class=\"has-text-align-center has-accent-color has-text-color has-link-color wp-elements-9241ed40cfc917514762dd30fa239ddb\">2 KMnO4 + 16 HCl \u2192 2 KCl + 2 MnCl<sub>2<\/sub> + 5 H<sub>2<\/sub>O + 8Cl<sub>2<\/sub><\/p>\n\n\n\n<ul>\n<li><strong>Reaction with alkali<\/strong><\/li>\n<\/ul>\n\n\n\n<p>When potassium permanganate is heated with alkalies, it transforms into manganate and emits oxygen gas.<\/p>\n\n\n\n<p class=\"has-text-align-center has-accent-color has-text-color has-link-color wp-elements-1bdcb99b5528e30a392be0a373f665d1\">4 KMnO<sub>4<\/sub> + 4 KOH \u2192 4 K<sub>2<\/sub>MnO<sub>4<\/sub> + 2 H<sub>2<\/sub>O + O<sub>2<\/sub><\/p>\n\n\n\n<ul>\n<li><strong>Oxidising properties<\/strong><\/li>\n<\/ul>\n\n\n\n<p>In acidic, neutral, and alkaline conditions, KMnO<sub>4<\/sub> is a potent oxidizing agent. The following equations represent oxidation in certain media:<\/p>\n\n\n\n<p><strong>In an acidic medium:<\/strong><\/p>\n\n\n\n<p class=\"has-text-align-center has-accent-color has-text-color has-link-color wp-elements-8b68ae89d474eef4ce4707a7ed96032f\">2KMnO<sub>4<\/sub>&nbsp;+ H<sub>2<\/sub>SO<sub>4<\/sub>&nbsp;\u2192 K<sub>2<\/sub>SO<sub>4<\/sub>&nbsp;+ 2MnSO<sub>4<\/sub>&nbsp;+ 3H<sub>2<\/sub>O + 5[O] MnO<sub>4<\/sub><sup>\u2013<\/sup>&nbsp;+ 8H<sup>+<\/sup>&nbsp;+ 5e<sup>\u2013<\/sup>&nbsp;\u2192 Mn<sup>2+<\/sup>&nbsp;+ 4H<sub>2<\/sub>O<\/p>\n\n\n\n<p><strong>In a neutral or alkaline medium:<\/strong><\/p>\n\n\n\n<p class=\"has-text-align-center has-accent-color has-text-color has-link-color wp-elements-8dc1a824c876a087158e506a5b938699\">2KMnO<sub>4<\/sub>&nbsp;+ H<sub>2<\/sub>O \u2192 2KOH + 2MnO<sub>2<\/sub>&nbsp;+ 3[O] MnO<sub>4<\/sub><sup>\u2013<\/sup>&nbsp;+ 2H<sub>2<\/sub>O + 3e<sup>\u2013<\/sup>&nbsp;\u2192 MnO<sub>2<\/sub>&nbsp;+ 4OH<sup>\u2013<\/sup><\/p>\n\n\n\n<ul>\n<li><strong>Other reactions<\/strong><\/li>\n<\/ul>\n\n\n\n<p><strong>With sulphuric acid<\/strong><\/p>\n\n\n\n<p class=\"has-text-align-center has-accent-color has-text-color has-link-color wp-elements-ec625be92d69ee65a19531e9774e7637\">2 KMnO<sub>4<\/sub>+ H<sub>2<\/sub>SO<sub>4<\/sub> \u2192 Mn<sub>2<\/sub>O<sub>7<\/sub> + K<sub>2<\/sub>SO\u2084 + H<sub>2<\/sub>O<\/p>\n\n\n\n<p><strong>With hydrogen peroxide<\/strong><\/p>\n\n\n\n<p class=\"has-text-align-center has-accent-color has-text-color has-link-color wp-elements-8fcfe8f4238fa46c55e8535afcff6134\">2 KMnO<sub>4<\/sub> + 3 H<sub>2<\/sub>O<sub>2 <\/sub>\u2192 2 KOH + 2 MnO<sub>2<\/sub> + 3 O<sub>2<\/sub>+ 2 H<sub>2<\/sub>O<\/p>\n\n\n\n<p><strong>With alkene<\/strong><\/p>\n\n\n\n<p>In a weak alkaline or neutral media, it can also oxidize carbon atoms with double bonds.<\/p>\n\n\n\n<p class=\"has-text-align-center has-accent-color has-text-color has-link-color wp-elements-8ce5436b6de87c331b58eaef79223e9c\">\u0421H<sub>2 <\/sub>= \u0421\u041d<sub>2<\/sub> + 2 KMnO<sub>4<\/sub>+ 2 H<sub>2<\/sub>O \u2192 CH<sub>2<\/sub>OH\u2013CH<sub>2<\/sub>OH + 2 MnO<sub>2<\/sub> + 2 KOH (with cooling).<\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"uses-of-potassium-permanganate\"><\/span><strong>Uses<\/strong> <strong>of potassium permanganate<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li>It is useful in leather tanning and fabric printing.&nbsp;<\/li>\n\n\n\n<li>It&#8217;s a bleaching agent, an antiseptic, and a pesticide.<\/li>\n\n\n\n<li>Acts as an oxidizing agent and aids in the synthesis of a variety of essential chemicals. Potassium permanganate has disinfectant properties. It can be used as a disinfectant to treat skin infections such as dermatitis, canker sores, ulcers, eczema, and fungal infections due to its oxidizing properties. When administered to minor wounds, it affects the microorganism&#8217;s outer cell membrane, oxidizing it and destroying its structure.<\/li>\n\n\n\n<li>It is used in water treatment plants to eliminate pollutants and remove unpleasant odors from water. It oxidizes iron, hydrogen sulfide, and manganese into solid particles, which are subsequently filtered out. Because the treatment does not produce any hazardous substances, it is quite safe to use.<\/li>\n\n\n\n<li>Because of its bright color and oxidizing properties, potassium permanganate is employed as a reagent in chemical labs to quantify the quantity of a&nbsp;substance that can be oxidized in a sample. This value is known as the permanganate value.&nbsp;<\/li>\n\n\n\n<li>It is useful for removing snails from plants before transferring them to an aquarium.<\/li>\n\n\n\n<li>It is a vital component of survival kits, along with glycerine\/glucose tablets, and can be used to start fires. A fire can be started by rubbing glucose tablets with permanganate powder. It can also be used to clean wounds and water.<\/li>\n\n\n\n<li>It can be used as an antidote in cases of phosphorus poisoning.<\/li>\n\n\n\n<li>It&#8217;s frequently used to treat parasitic diseases in fish.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"health-effects-of-potassium-permanganate\"><\/span><strong>Health effects<\/strong> <strong>of Potassium permanganate<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li>When inhaled, it can irritate the nose and throat. Even the lungs can be damaged, resulting in coughing, shortness of breath, and pulmonary edema (fluid buildup in the lungs).<\/li>\n\n\n\n<li>KMnO<s>4<\/s> may also affect&nbsp;the liver and kidneys.<\/li>\n\n\n\n<li>Long-term exposure may have an impact on fertility.<\/li>\n\n\n\n<li>Potassium permanganate, in concentrated form, is irritating to the eyes and skin. It can react with a wide range of reducing agents and organic materials, however,&nbsp;it is flammable.<\/li>\n\n\n\n<li>The antibacterial effect of KMnO<sub>4<\/sub> is based on the oxidation of bacteria or tissue proteins by this molecule. It stains the skin and tissues. Because it operates on all organic matter through a destructive oxidation process, its application is limited to external uses exclusively.<\/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>Lee, J.D. (1996) Concise Inorganic Chemistry. 5th Edition, Chapman and Hall Ltd., London, 619-621.<\/li>\n\n\n\n<li>https:\/\/byjus.com\/chemistry\/kmno4\/<\/li>\n\n\n\n<li>https:\/\/www.vedantu.com\/chemistry\/potassium-permanganate<\/li>\n\n\n\n<li>https:\/\/testbook.com\/chemistry\/kmno4<\/li>\n\n\n\n<li>https:\/\/unacademy.com\/content\/neet-ug\/study-material\/chemistry\/preparation-of-potassium-permanganate-kmno4\/<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Potassium permanganate is a chemical compound with the chemical formula KMnO4. It is a manganic acid potassium salt. It is&nbsp;also known as Condy&#8217;s crystals or potash permanganate. Johann Rudolf Glauber, &#8230; <a title=\"Potassium Permanganate: \u00a0Preparation, Structure, Properties, Reactions, Health effects\" class=\"read-more\" href=\"https:\/\/thechemistrynotes.com\/potassium-permanganate-preparation-reaction\/\" aria-label=\"Read more about Potassium Permanganate: \u00a0Preparation, Structure, Properties, Reactions, Health effects\">Read more<\/a><\/p>\n","protected":false},"author":4,"featured_media":50398,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[24,29],"tags":[3115,3109,3110,3113,3112,3111,3114],"_links":{"self":[{"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/posts\/50395"}],"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=50395"}],"version-history":[{"count":2,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/posts\/50395\/revisions"}],"predecessor-version":[{"id":50399,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/posts\/50395\/revisions\/50399"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/media\/50398"}],"wp:attachment":[{"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/media?parent=50395"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/categories?post=50395"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/tags?post=50395"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}