{"id":48390,"date":"2023-09-23T14:17:08","date_gmt":"2023-09-23T08:32:08","guid":{"rendered":"https:\/\/thechemistrynotes.com\/?p=48390"},"modified":"2023-09-23T14:17:11","modified_gmt":"2023-09-23T08:32:11","slug":"sulphuric-acid-preparation-properties","status":"publish","type":"post","link":"https:\/\/thechemistrynotes.com\/sulphuric-acid-preparation-properties\/","title":{"rendered":"Sulphuric Acid: Formula, Preparations, Properties, Uses, Health Risks"},"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\/09\/Sulphuric-Acid.jpg\" alt=\"Sulphuric Acid\" class=\"wp-image-48393\" srcset=\"https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/09\/Sulphuric-Acid.jpg 1205w, https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/09\/Sulphuric-Acid-300x157.jpg 300w, https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/09\/Sulphuric-Acid-1024x536.jpg 1024w, https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/09\/Sulphuric-Acid-768x402.jpg 768w\" sizes=\"(max-width: 1205px) 100vw, 1205px\" \/><\/figure>\n\n\n\n<p>It is a well-known mineral acid that is also known as vitriol oil. It is made up of three major components: oxygen, hydrogen, and sulfur. Sulfuric acid has the chemical formula H2SO4, and it is a colorless, odorless, and viscous chemical liquid.&nbsp;In the eighth century, Jabir ibn Hayyan discovered sulphuric acid.&nbsp;Because it contains two acid protons, it is a very corrosive diprotic.<\/p>\n\n\n\n<p>Sulphuric acid is extremely acidic. As a result, it is used to clean metals, extract impurities from oil, produce chemicals such as nitric acid and hydrochloric acid, and create dye, pharmaceuticals, detergents, and explosives, among other things.<\/p>\n\n\n\n<p>At greater concentrations, it acts as an oxidizing and dehydrating agent. When dissolved in water, it generates heat. The acid is known by the following names:<\/p>\n\n\n\n<ul>\n<li>Sulphuric acid<\/li>\n\n\n\n<li>Dihydrogen sulphate<\/li>\n\n\n\n<li>Mattling acid<\/li>\n\n\n\n<li>Oil of vitriol<\/li>\n\n\n\n<li>Battery acid<\/li>\n\n\n\n<li>Dipping acid<\/li>\n\n\n\n<li>Electrolyte acid<\/li>\n<\/ul>\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\/sulphuric-acid-preparation-properties\/#structure-of-sulphuric-acid\" title=\"Structure of sulphuric acid\">Structure of sulphuric 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\/sulphuric-acid-preparation-properties\/#preparation-of-sulphuric-acid\" title=\"Preparation of sulphuric acid\">Preparation of sulphuric acid<\/a><ul class='ez-toc-list-level-3' ><li class='ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-3\" href=\"https:\/\/thechemistrynotes.com\/sulphuric-acid-preparation-properties\/#contact-process\" title=\"Contact process\">Contact process<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-4\" href=\"https:\/\/thechemistrynotes.com\/sulphuric-acid-preparation-properties\/#lead-chamber-process\" title=\"Lead chamber process\">Lead chamber process<\/a><\/li><\/ul><\/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\/sulphuric-acid-preparation-properties\/#physical-properties\" title=\"Physical properties\">Physical properties<\/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\/sulphuric-acid-preparation-properties\/#chemical-properties\" title=\"Chemical properties\">Chemical properties<\/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\/sulphuric-acid-preparation-properties\/#reactions-of-sulphuric-acid\" title=\"Reactions of sulphuric acid\">Reactions of sulphuric acid<\/a><ul class='ez-toc-list-level-3' ><li class='ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-8\" href=\"https:\/\/thechemistrynotes.com\/sulphuric-acid-preparation-properties\/#dissociation-reaction\" title=\"Dissociation reaction\">Dissociation reaction<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-9\" href=\"https:\/\/thechemistrynotes.com\/sulphuric-acid-preparation-properties\/#acidic-property\" title=\"Acidic property\">Acidic property<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-10\" href=\"https:\/\/thechemistrynotes.com\/sulphuric-acid-preparation-properties\/#reaction-with-water\" title=\"Reaction with water\">Reaction with water<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-11\" href=\"https:\/\/thechemistrynotes.com\/sulphuric-acid-preparation-properties\/#as-dehydrating-agent\" title=\"As dehydrating agent\">As dehydrating agent<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-12\" href=\"https:\/\/thechemistrynotes.com\/sulphuric-acid-preparation-properties\/#precipitation-reaction\" title=\"Precipitation reaction\">Precipitation reaction<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-13\" href=\"https:\/\/thechemistrynotes.com\/sulphuric-acid-preparation-properties\/#sulphonation-reaction\" title=\"Sulphonation reaction\">Sulphonation reaction<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-14\" href=\"https:\/\/thechemistrynotes.com\/sulphuric-acid-preparation-properties\/#reaction-with-metals\" title=\"Reaction with metals\">Reaction with metals<\/a><\/li><\/ul><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-15\" href=\"https:\/\/thechemistrynotes.com\/sulphuric-acid-preparation-properties\/#uses-of-sulphuric-acid\" title=\"Uses of sulphuric acid\">Uses of sulphuric acid<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-16\" href=\"https:\/\/thechemistrynotes.com\/sulphuric-acid-preparation-properties\/#health-risks-associated-with-exposure-to-sulphuric-acid\" title=\"Health risks associated with exposure to sulphuric acid\">Health risks associated with exposure to sulphuric acid<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-17\" href=\"https:\/\/thechemistrynotes.com\/sulphuric-acid-preparation-properties\/#references\" title=\"References\">References<\/a><\/li><\/ul><\/nav><\/div>\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"structure-of-sulphuric-acid\"><\/span><strong>Structure of sulphuric acid<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<p>Sulphuric acid is a sulfur oxoacid that contains two oxo and two hydroxyl groups that are covalently bonded to a central sulfur atom. The center of a tetrahedral molecule is sulfur. Sulphur is present at its maximal oxidation state, +6, in sulphuric acid. It is classified as a diprotic acid because it can dissociate into two H<sup>+<\/sup> ions.<\/p>\n\n\n\n<p>H<sub>2<\/sub>SO<sub>4<\/sub>&nbsp;\u21cc 2H<sup>+<\/sup>+SO<sub>4<\/sub><sup>2-<\/sup><\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"218\" height=\"196\" src=\"https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/09\/image-68.png\" alt=\"\" class=\"wp-image-48391\" \/><\/figure><\/div>\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"preparation-of-sulphuric-acid\"><\/span><strong>Preparation of sulphuric acid<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<h3 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"contact-process\"><\/span><strong>Contact process<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h3>\n\n\n\n<p>One mole of sulphuric acid is generated when one mole of sulfur trioxide reacts with water. In this reaction, vanadium oxide is used as a catalyst.<\/p>\n\n\n\n<p>SO<sub>3<\/sub>+ H<sub>2<\/sub>O \u2192 H<sub>2<\/sub>SO<sub>4<\/sub><\/p>\n\n\n\n<p><strong>Mechanism:<\/strong><\/p>\n\n\n\n<p><strong>Step I: Production of sulphur dioxide<\/strong><\/p>\n\n\n\n<p>Heating sulfur or sulfide ores produces sulfur dioxide. For example, iron pyrites in excess of air.<\/p>\n\n\n\n<p>S + O<sub>2<\/sub>&nbsp;(\u0394&nbsp;) &nbsp; \u2192&nbsp; &nbsp; SO<sub>2<\/sub><\/p>\n\n\n\n<p>4 FeS +&nbsp; &nbsp;7O<sub>2<\/sub>&nbsp;(\u0394)\u2192&nbsp; &nbsp; 2Fe<sub>2<\/sub>O<sub>3<\/sub>+&nbsp; 4SO<sub>2<\/sub><\/p>\n\n\n\n<p><strong>Step II: formation of sulfur trioxide<\/strong><\/p>\n\n\n\n<p>2SO<sub>2<\/sub> +&nbsp; &nbsp;O<sub>2<\/sub> +&nbsp; &nbsp;V<sub>2<\/sub>O<sub>5<\/sub> \u2192&nbsp; &nbsp; SO<sub>3<\/sub><sub><\/sub><\/p>\n\n\n\n<p><strong>Step III: Formation of oleum<\/strong><strong><\/strong><\/p>\n\n\n\n<p>The reaction between sulfur trioxide and sulphuric acid produces oleum.<\/p>\n\n\n\n<p>SO<sub>3<\/sub>&nbsp;+&nbsp; H<sub>2<\/sub>SO<sub>4 <\/sub>\u2192&nbsp;&nbsp;&nbsp;&nbsp;H<sub>2<\/sub>S<sub>2<\/sub>O<sub>7<\/sub><sub><\/sub><\/p>\n\n\n\n<p><strong>Step IV: Formation of sulphuric acid<\/strong><strong><\/strong><\/p>\n\n\n\n<p>oleum is diluted slowly to obtain concentrated sulphuric acid.<\/p>\n\n\n\n<p>H<sub>2<\/sub>S<sub>2<\/sub>O<sub>7 <\/sub>+&nbsp;H<sub>2<\/sub>O \u2192&nbsp; &nbsp; &nbsp;2H<sub>2<\/sub>SO<sub>4<\/sub><\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"lead-chamber-process\"><\/span><strong>Lead chamber process<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h3>\n\n\n\n<p>The lead Chamber process is one of the most used production techniques. It produces 50 to 60 B-grade acids. This technique&nbsp;uses wet SO<sub>2<\/sub> in the presence of nitrogen oxides. As a result, it combines with the oxygen in the air to generate sulfur trioxide.<\/p>\n\n\n\n<p>2 SO<sub>2<\/sub>\u00a0 \u00a0+\u00a0 \u00a0O<sub>2\u00a0\u00a0<\/sub>\u00a0 \u2192\u00a0 \u00a02SO<sub>3<\/sub><\/p>\n\n\n\n<p>Sulfur trioxide is then allowed to combine with water to form H<sub>2<\/sub>SO<sub>4<\/sub>. This reaction is represented by<\/p>\n\n\n\n<p>SO<sub>3<\/sub>&nbsp; &nbsp;+&nbsp; &nbsp;H<sub>2<\/sub>O&nbsp; &nbsp;\u2192&nbsp; &nbsp; H<sub>2<\/sub>SO<sub>4<\/sub><\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"physical-properties\"><\/span><strong>Physical properties<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li>H<sub>2<\/sub>SO<sub>4<\/sub> is an oily, viscous, thick, colorless liquid.<\/li>\n\n\n\n<li>Sulfuric acid has a density of 1.84 g\/mL, a boiling point of 337 degrees Celsius, and a melting point of 10 degrees Celsius.<\/li>\n\n\n\n<li>The most stable form is concentrated sulfuric acid, which is 98% water. Many more concentrations with different names are available for diverse purposes, such as battery acid (29-32%), chamber acid (62-70%), and tower acid (78-80%).<\/li>\n\n\n\n<li>At 298 K, it has a specific gravity of 1.84.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"chemical-properties\"><\/span><strong>Chemical properties<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li>Sulphuric acid is a powerful dibasic acid. It is also diprotic, ionizing in two steps in aqueous solution.<\/li>\n\n\n\n<li>This chemical is very corrosive, reactive, and water-soluble. It has a high oxidizing power and hence functions as a potent oxidizing agent.<\/li>\n\n\n\n<li>It is extremely volatile. As a result, it is used in the synthesis of more volatile acids from their corresponding salts.<\/li>\n\n\n\n<li>Concentrated sulfuric acid is a powerful dehydrator. As a result, this chemical is employed to dry numerous wet gases that do not react with the acid.<\/li>\n\n\n\n<li>It also removes water from natural mixtures such as starches.<\/li>\n\n\n\n<li>It can oxidize both nonmetals and metals because it is a good oxidizing agent. Furthermore, it reduces to sulfur dioxide.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"reactions-of-sulphuric-acid\"><\/span><strong>Reactions of sulphuric acid<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<h3 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"dissociation-reaction\"><\/span><strong>Dissociation reaction<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h3>\n\n\n\n<p>Sulfur trioxide and water are generated when pure water-free sulphuric acid is boiled.<\/p>\n\n\n\n<p>H<sub>2<\/sub>SO<sub>4<\/sub> \u2192 SO<sub>3<\/sub> + H<sub>2<\/sub>O<\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"acidic-property\"><\/span><strong>Acidic property<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h3>\n\n\n\n<p>A typical dibasic acid, when exposed to it, causes blue litmus to turn red.+<\/p>\n\n\n\n<p>NaOH + H<sub>2<\/sub>SO<sub>4<\/sub> \u2192 NaHSO<sub>4<\/sub> + H<sub>2<\/sub>O<\/p>\n\n\n\n<p>2NaOH + H<sub>2<\/sub>SO<sub>4<\/sub> \u2192 Na<sub>2 <\/sub>SO<sub>4<\/sub> + 2 H<sub>2<\/sub>O<\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"reaction-with-water\"><\/span><strong>Reaction with water<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h3>\n\n\n\n<p>When H<sub>2<\/sub>SO<sub>4 <\/sub>is combined with water, an exothermic reaction occurs. The reaction generates a significant quantity of heat, to the point where the solution may even boil.<\/p>\n\n\n\n<p>H<sub>2<\/sub>SO<sub>4<\/sub>&nbsp;+ H<sub>2<\/sub>O \u2192 H<sub>3<\/sub>O<sup>+<\/sup>&nbsp;+ HSO<sup>4-<\/sup><\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"as-dehydrating-agent\"><\/span><strong>As dehydrating agent<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h3>\n\n\n\n<p>It converts glucose, sugar, and starch to carbon.<\/p>\n\n\n\n<p>C<sub>12<\/sub>H<sub>22<\/sub>O<sub>11&nbsp; &nbsp;<\/sub>+&nbsp; &nbsp;(H<sub>2<\/sub>SO<sub>4<\/sub>)&nbsp; &nbsp;\u2192 12C&nbsp; &nbsp;+ &nbsp;11H<sub>2<\/sub>O<\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"precipitation-reaction\"><\/span><strong>Precipitation reaction<\/strong><strong><\/strong><span class=\"ez-toc-section-end\"><\/span><\/h3>\n\n\n\n<p>When it comes into contact with aqueous solutions of barium, lead, and other salts, it produces insoluble sulfates that precipitate.<\/p>\n\n\n\n<p>H\u2082\u00adSO\u2084 + Ba\u00adCl\u2082 \u2192 &nbsp;Ba\u00adSO\u2084 + 2HCl<\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"sulphonation-reaction\"><\/span><strong>Sulphonation reaction<\/strong><strong><\/strong><span class=\"ez-toc-section-end\"><\/span><\/h3>\n\n\n\n<p>Concentrated sulphuric acid reacts with a range of organic compounds, including <a href=\"https:\/\/thechemistrynotes.com\/benzene-preparation-reactions-uses\/\">benzene<\/a>, toluene, and others, to generate sulphonic acids.<\/p>\n\n\n\n<p>C<sub>6<\/sub>H<sub>6<\/sub> + H\u2082\u00adSO\u2084 \u2192 C<sub>6<\/sub>H<sub>5<\/sub>SO<sub>3<\/sub>H + H<sub>2<\/sub>O<\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"reaction-with-metals\"><\/span><strong>Reaction with metals<\/strong><strong><\/strong><span class=\"ez-toc-section-end\"><\/span><\/h3>\n\n\n\n<p>Concentrated sulfuric acid is a powerful oxidant. All metals except gold, iridium, platinum, rhodium, and tantalum can be oxidized by it.&nbsp;<\/p>\n\n\n\n<ul>\n<li>Hot and concentrated sul\u00adfu\u00adric acid reacts with metals such as aluminum, re\u00adducing to H2S, S, and SO2.<\/li>\n<\/ul>\n\n\n\n<p>8 Al + 15 H\u2082\u00adSO\u2084 (concentrated) \u2192&nbsp; &nbsp;4 Al\u2082 (SO\u2084)\u2083 + 12 H\u2082O + 3 H\u2082S<\/p>\n\n\n\n<ul>\n<li>When copper combines with hot, concentrated sulfuric acid, the following reaction occurs:<\/li>\n<\/ul>\n\n\n\n<p>Cu+ 2 H<sub>2<\/sub>SO<sub>4<\/sub>&nbsp;\u2192&nbsp; &nbsp;CuSO<sub>4<\/sub>&nbsp;+ SO<sub>2<\/sub>&nbsp;+2 H<sub>2<\/sub>O<\/p>\n\n\n\n<ul>\n<li>A common reaction is the action of sulfuric acid on zinc to produce hydrogen. When zinc granules are added to dilute sulfuric acid, hydrogen gas is formed while the metal dissolves.<\/li>\n<\/ul>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp; Zn + H\u2082\u00adSO\u2084 \u2192 &nbsp;Zn\u00adSO\u2084 + H\u2082<\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"uses-of-sulphuric-acid\"><\/span><strong>Uses<\/strong> <strong>of sulphuric acid<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li>93% pure sulfuric acid is employed in the refining of petroleum products.<\/li>\n\n\n\n<li>Sulfuric acid is used to pickle steel before tinning and galvanizing.<\/li>\n\n\n\n<li>Sulfuric acid is used in metallurgy to remove (float) copper, zinc, and lead from their ores. It is also used to leach ores and waste tailings for metal recovery.<\/li>\n\n\n\n<li>Sulfuric acid is a laboratory reagent used in acid-base titrations, water analysis, polymer testing, redox titration, and other applications.<\/li>\n\n\n\n<li>Under typical conditions, alcohols and aldehydes can be oxidized to carboxylic acids by employing dilute sulfuric acid.<\/li>\n\n\n\n<li>It is used in the production of superphosphate, ammonium sulfate, and other chemicals.<\/li>\n\n\n\n<li>It is used to make metal sulfates such as zinc, copper, aluminum, magnesium, and so on.<\/li>\n\n\n\n<li>It is used in the production of dyes, paints, explosives, and detergents. It is also utilized in electrochemical cells and batteries as an electrolyte.<\/li>\n\n\n\n<li>It is used to purify substances such as benzene, paraffin oil, petroleum, and others.<\/li>\n\n\n\n<li>This is commonly used to make nitroglycerin, pyroxylin, nitrobenzene, picric acid, and nitro ethers.<\/li>\n\n\n\n<li>They are mostly utilized in the distillation of fatty acids.<\/li>\n\n\n\n<li>H\u2082\u00adSO\u2084 is mostly utilized in the &#8220;wet technique&#8221; of producing phosphoric acid.<\/li>\n\n\n\n<li>It is employed in the manufacturing of chemotherapeutic drugs, as well as to damage the DNA of cancerous cells. It can be found in ointments used to treat several&nbsp;skin disorders. Debacterol, a topical ointment intended to treat cancer sores, has it as an active ingredient.<\/li>\n\n\n\n<li>It is used in the production of fertilizers.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"health-risks-associated-with-exposure-to-sulphuric-acid\"><\/span><strong>Health risks associated with exposure to sulphuric acid<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li>Skin contact might result in necrosis.<\/li>\n\n\n\n<li>It irritates the upper respiratory tract greatly.<\/li>\n\n\n\n<li>Sulfuric acid can cause severe lung damage and emergencies.<\/li>\n\n\n\n<li>It irritates the eyes and can potentially lead to blindness.<\/li>\n\n\n\n<li>It can induce fluid buildup in the lungs. Pulmonary edema is the medical term for this illness.<\/li>\n\n\n\n<li>Headaches, vomiting, and nausea can all be caused by sulfuric acid exposure.<\/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:\/\/www.toppr.com\/guides\/chemistry\/the-p-block-elements\/sulphuric-acid\/<\/li>\n\n\n\n<li>https:\/\/byjus.com\/chemistry\/sulfuric-acid\/#:~:text=Sulfuric%20Acid%20is%20a%20mineral,odourless%20and%20has%20no%20colour.<\/li>\n\n\n\n<li>https:\/\/www.aakash.ac.in\/important-concepts\/chemistry\/uses-of-sulfuric-acid<\/li>\n\n\n\n<li>https:\/\/unacademy.com\/content\/jee\/study-material\/chemistry\/reaction-with-sulphuric-acid\/<\/li>\n\n\n\n<li>https:\/\/www.geeksforgeeks.org\/sulfuric-acid\/<\/li>\n<\/ul>\n\n\n\n<p><\/p>\n","protected":false},"excerpt":{"rendered":"<p>It is a well-known mineral acid that is also known as vitriol oil. It is made up of three major components: oxygen, hydrogen, and sulfur. Sulfuric acid has the chemical &#8230; <a title=\"Sulphuric Acid: Formula, Preparations, Properties, Uses, Health Risks\" class=\"read-more\" href=\"https:\/\/thechemistrynotes.com\/sulphuric-acid-preparation-properties\/\" aria-label=\"Read more about Sulphuric Acid: Formula, Preparations, Properties, Uses, Health Risks\">Read more<\/a><\/p>\n","protected":false},"author":4,"featured_media":48393,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[29,24],"tags":[2904,2901,2902,2900,2903],"_links":{"self":[{"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/posts\/48390"}],"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=48390"}],"version-history":[{"count":2,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/posts\/48390\/revisions"}],"predecessor-version":[{"id":48394,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/posts\/48390\/revisions\/48394"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/media\/48393"}],"wp:attachment":[{"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/media?parent=48390"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/categories?post=48390"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/tags?post=48390"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}