{"id":8054,"date":"2026-09-15T08:23:39","date_gmt":"2026-09-15T07:23:39","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-4-acids\/typical-reactions-of-acids\/"},"modified":"2026-09-19T20:35:47","modified_gmt":"2026-09-19T19:35:47","slug":"typical-reactions-of-acids","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-4-acids\/typical-reactions-of-acids\/","title":{"rendered":"Typical Reactions of Acids"},"content":{"rendered":"\n<!--\n===============================================================================\nONLINE LEARNING SYSTEM COPYRIGHT NOTICE\n\u00a9 Online Learning System. All rights reserved.\n\nThis WordPress revision page HTML, CSS, content sequence, educational wording,\nlayout structure, schema structure and embedded design logic are protected\nintellectual property of Online Learning System.\n\nUnauthorised copying, redistribution, resale, modification, republication,\nscraping, extraction, derivative reuse, automated harvesting or removal of\ncopyright notices is strictly prohibited.\n\nBackend copyright marker:\nOLS-T5-TYPICAL-REACTIONS-OF-ACIDS-REVISION-PAGE-2026\n\nPage:\nTypical Reactions of Acids\nOCR A Level Chemistry A\nUnit: Paper 1\nAmount of Substance\nH432\/01\n\nCopyright enforcement notes:\n- The visible student page is a free OLS revision resource.\n- The backend HTML structure, CSS architecture, card sequencing, schema graph,\n  revision wording, responsive table behaviour and embedded learning pathway are\n  proprietary OLS production assets.\n- Do not remove this notice.\n===============================================================================\n-->\n\n<section class=\"ols-revision-page ols-typical-reactions-of-acids-page\" data-owner=\"Online Learning System\" data-copyright=\"\u00a9 Online Learning System. 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href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-4-acids\/acids-and-alkalis\/\">Acids and Alkalis<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-4-acids\/typical-reactions-of-acids\/\">Typical Reactions of Acids<\/a><\/li>\n<li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-4-acids\/standard-solutions-and-titration-technique\/\">Standard Solutions and Titration Technique<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-4-acids\/titration-calculations\/\">Titration Calculations<\/a><\/li>\n    <\/ul>\n  <\/div>\n  <div class=\"ols-topic-group\">\n    <h4>Other OCR Sections<\/h4>\n    <ul class=\"ols-topic-list\">\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-1-atomic-structure-and-isotopes\/\">2.1.1 Atomic Structure and Isotopes<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/\">2.1.2 Compounds, Formulae and Equations<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-3-amount-of-substance\/\">2.1.3 Amount of Substance<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-2-1-electron-structure\/\">2.2.1 Electron Structure<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-2-2-bonding-and-structure\/\">2.2.2 Bonding and Structure<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/3-1-1-periodicity\/\">3.1.1 Periodicity<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-1-1-basic-concepts-of-organic-chemistry\/\">4.1.1 Basic Concepts of Organic Chemistry<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-1-2-alkanes\/\">4.1.2 Alkanes<\/a><\/li>\n      <li><a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/4-1-3-alkenes\/\">4.1.3 Alkenes<\/a><\/li>\n    <\/ul>\n  <\/div>\n<\/aside>\n<script>\r\n(function() {\r\n  function normalisePath(path) {\r\n    return String(path || '')\r\n      .split('?')[0]\r\n      .split('#')[0]\r\n      .replace(\/\\\/+$\/, '')\r\n      .toLowerCase();\r\n  }\r\n\r\n  function highlightActive() {\r\n    var sidebar = document.querySelector('.ols-sidebar');\r\n 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href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/\">OCR A<\/a> \/\n<a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-4-acids\/\">2.1.4 Acids<\/a> \/\n<span>Typical Reactions of Acids<\/span>\n<\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Typical Reactions of Acids<\/h1>\n        <p class=\"ols-page-intro\">A concise revision guide to the common reactions of acids, including acid-base neutralisation, acid-metal reactions, acid-carbonate reactions and the ionic equations that show the particles actually reacting.<\/p>\n\n        <div class=\"ols-badges\">\n<div class=\"ols-badge\">Paper 1 and 2<\/div>\n<div class=\"ols-badge\">2.1.4 Acids<\/div>\n<div class=\"ols-badge\">H432\/01 and H432\/02<\/div>\n<\/div>\n\n        <div class=\"ols-author\">\n          <img decoding=\"async\" class=\"ols-author-avatar-img\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/05\/Author-Profile.jpeg\" alt=\"Dr. Mohammed Al-Fatah\">\n          <div class=\"ols-author-content\">\n            <h2 class=\"ols-author-title\">Written by:<br><span>Dr. Mohammed Al-Fatah<\/span><\/h2>\n            <p class=\"ols-author-description\">Chemistry specialist revision notes for A Level Chemistry.<\/p>\n            <a class=\"ols-linkedin-pill\" href=\"https:\/\/www.linkedin.com\/in\/doctormohammedfatah\/\" target=\"_blank\" rel=\"noopener noreferrer\">\n              <svg class=\"ols-linkedin-icon\" viewBox=\"0 0 24 24\" fill=\"currentColor\" aria-hidden=\"true\"><path d=\"M4.98 3.5C4.98 4.88 3.86 6 2.48 6S0 4.88 0 3.5 1.12 1 2.48 1s2.5 1.12 2.5 2.5zM.5 8h4V24h-4V8zm7 0h3.8v2.2h.1c.5-.9 1.8-2.2 3.9-2.2 4.2 0 5 2.8 5 6.4V24h-4v-7.6c0-1.8 0-4.2-2.6-4.2s-3 2-3 4v7.8h-4V8z\"><\/path><\/svg>\n              View LinkedIn Profile\n            <\/a>\n          <\/div>\n        <\/div>\n      <\/header>\n\n      <section class=\"ols-h5p-card ols-h5p-inline ols-h5p-recap\">\n<span class=\"ols-h5p-kicker\">Before you start<\/span>\n<h2>GCSE Recap: Ions, Formulae and State Symbols<\/h2>\n<p>Before you start, check that you can build a formula from its ions and use state symbols.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"288\"><\/div><\/div>\n<\/section>\n<article class=\"ols-note-card soft\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">1<\/div><h2>What Acids Do in Reactions<\/h2><\/div>\n        <p>In aqueous solution, acids provide <strong>H<sup>+<\/sup> ions<\/strong>. These hydrogen ions are responsible for the typical reactions of acids.<\/p>\n        <p>The common strong acids used in many school-level reactions are <strong>hydrochloric acid, HCl<\/strong>, <strong>sulfuric acid, H<sub>2<\/sub>SO<sub>4<\/sub><\/strong>, and <strong>nitric acid, HNO<sub>3<\/sub><\/strong>.<\/p>\n        <div class=\"ols-definition-box\"><p><strong>Acid reaction pattern:<\/strong> the acid supplies H<sup>+<\/sup> ions, while the other reactant determines the type of product formed.<\/p><\/div>\n        <div class=\"ols-key-box\"><p><strong>Key idea:<\/strong> acid reactions often look different as full equations, but their ionic equations can reveal the same underlying particle change.<\/p><\/div>\n      <\/article>\n\n      <article class=\"ols-note-card\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">2<\/div><h2>Acids, Bases and Alkalis<\/h2><\/div>\n        <p>A <strong>base<\/strong> neutralises an acid. Common bases include <strong>metal oxides<\/strong>, <strong>metal hydroxides<\/strong> and <strong>ammonia<\/strong>.<\/p>\n        <p>An <strong>alkali<\/strong> is a soluble base that releases <strong>OH<sup>&#8211;<\/sup> ions<\/strong> in aqueous solution. Common alkalis include sodium hydroxide, NaOH, potassium hydroxide, KOH, and aqueous ammonia, NH<sub>3<\/sub>.<\/p>\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Term<\/th>\n                <th>Meaning<\/th>\n                <th>Examples<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Term\">Base<\/td>\n                <td data-label=\"Meaning\">A substance that neutralises an acid.<\/td>\n                <td data-label=\"Examples\">Metal oxides, metal hydroxides and ammonia.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Term\">Alkali<\/td>\n                <td data-label=\"Meaning\">A soluble base that releases OH<sup>&#8211;<\/sup> ions in water.<\/td>\n                <td data-label=\"Examples\">NaOH, KOH and aqueous NH<sub>3<\/sub>.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Term\">Salt<\/td>\n                <td data-label=\"Meaning\">A compound formed when the H<sup>+<\/sup> ion of an acid is replaced by a metal ion or ammonium ion.<\/td>\n                <td data-label=\"Examples\">NaCl, MgSO<sub>4<\/sub> and NH<sub>4<\/sub>Cl.<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n      <\/article>\n\n      <article class=\"ols-note-card purple\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">3<\/div><h2>Neutralisation Reactions Form Salts<\/h2><\/div>\n        <p><strong>Neutralisation<\/strong> is the reaction between an acid and a base. The acid is neutralised because the H<sup>+<\/sup> ions are removed by reacting with basic particles such as OH<sup>&#8211;<\/sup> ions.<\/p>\n        <p>When an acid reacts with a metal hydroxide, the products are usually a <strong>salt<\/strong> and <strong>water<\/strong>.<\/p>\n        <div class=\"ols-definition-box\"><p><strong>General equation:<\/strong> acid + metal hydroxide \u2192 salt + water<\/p><\/div>\n        <div class=\"ols-definition-box\"><p><strong>Example:<\/strong> HCl(aq) + NaOH(aq) \u2192 NaCl(aq) + H<sub>2<\/sub>O(l)<\/p><\/div>\n        <p>The ionic equation for neutralisation is the same for many acid-alkali reactions because H<sup>+<\/sup> ions react with OH<sup>&#8211;<\/sup> ions to form water.<\/p>\n        <div class=\"ols-key-box\"><p><strong>Ionic equation:<\/strong> H<sup>+<\/sup>(aq) + OH<sup>&#8211;<\/sup>(aq) \u2192 H<sub>2<\/sub>O(l)<\/p><\/div>\n      <\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Which Substances Are Bases?<\/h2>\n<p>Click every substance in the list that would neutralise an acid.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-327\" class=\"h5p-iframe\" data-content-id=\"327\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Acids and Bases Mark the Words: Pick Out Every Base\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card orange\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">4<\/div><h2>Acids Reacting with Metals<\/h2><\/div>\n        <p>Reactive metals such as magnesium react with dilute acids to form a <strong>salt<\/strong> and <strong>hydrogen gas<\/strong>. The hydrogen gas is observed as fizzing or effervescence.<\/p>\n        <div class=\"ols-definition-box\"><p><strong>General equation:<\/strong> acid + metal \u2192 salt + hydrogen<\/p><\/div>\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Reaction<\/th>\n                <th>Full equation<\/th>\n                <th>Main observation<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Reaction\">Magnesium with hydrochloric acid<\/td>\n                <td data-label=\"Full equation\">Mg(s) + 2HCl(aq) \u2192 MgCl<sub>2<\/sub>(aq) + H<sub>2<\/sub>(g)<\/td>\n                <td data-label=\"Main observation\">Fizzing as hydrogen gas forms.<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Reaction\">Magnesium with sulfuric acid<\/td>\n                <td data-label=\"Full equation\">Mg(s) + H<sub>2<\/sub>SO<sub>4<\/sub>(aq) \u2192 MgSO<sub>4<\/sub>(aq) + H<sub>2<\/sub>(g)<\/td>\n                <td data-label=\"Main observation\">The metal disappears if the acid is in excess.<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n        <p>The ionic equation is the same in both cases because chloride ions and sulfate ions are spectator ions. They do not change during the reaction.<\/p>\n        <div class=\"ols-key-box\"><p><strong>Ionic equation:<\/strong> Mg(s) + 2H<sup>+<\/sup>(aq) \u2192 Mg<sup>2+<\/sup>(aq) + H<sub>2<\/sub>(g)<\/p><\/div>\n      <\/article>\n\n      <div class=\"ols-zoom-card\">\n        <div class=\"ols-zoom-card-image\">\n          <img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/05\/Ionic-equations-for-acid-metal-reactions.webp\" alt=\"Ionic equations for reactions between acids and metals showing spectator ions\" class=\"ols-zoomable-img ols-lightbox-target\" draggable=\"false\">\n        <\/div>\n        <div class=\"ols-zoom-card-caption\">\n          <p>Different full equations can simplify to the same ionic equation when the spectator ions are removed.<\/p>\n        <\/div>\n      <\/div>\n\n      <article class=\"ols-note-card soft\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">5<\/div><h2>Acids Reacting with Metal Carbonates<\/h2><\/div>\n        <p>Metal carbonates react with dilute acids to form a <strong>salt<\/strong>, <strong>carbon dioxide<\/strong> and <strong>water<\/strong>. The carbon dioxide gas causes fizzing.<\/p>\n        <div class=\"ols-definition-box\"><p><strong>General equation:<\/strong> acid + metal carbonate \u2192 salt + carbon dioxide + water<\/p><\/div>\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Reaction<\/th>\n                <th>Full equation<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Reaction\">Calcium carbonate with hydrochloric acid<\/td>\n                <td data-label=\"Full equation\">CaCO<sub>3<\/sub>(s) + 2HCl(aq) \u2192 CaCl<sub>2<\/sub>(aq) + CO<sub>2<\/sub>(g) + H<sub>2<\/sub>O(l)<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Reaction\">Magnesium carbonate with nitric acid<\/td>\n                <td data-label=\"Full equation\">MgCO<sub>3<\/sub>(s) + 2HNO<sub>3<\/sub>(aq) \u2192 Mg(NO<sub>3<\/sub>)<sub>2<\/sub>(aq) + CO<sub>2<\/sub>(g) + H<sub>2<\/sub>O(l)<\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Reaction\">Sodium carbonate with sulfuric acid<\/td>\n                <td data-label=\"Full equation\">Na<sub>2<\/sub>CO<sub>3<\/sub>(aq) + H<sub>2<\/sub>SO<sub>4<\/sub>(aq) \u2192 Na<sub>2<\/sub>SO<sub>4<\/sub>(aq) + CO<sub>2<\/sub>(g) + H<sub>2<\/sub>O(l)<\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n        <p>For many acid-carbonate reactions, the useful ionic equation is:<\/p>\n        <div class=\"ols-key-box\"><p><strong>Ionic equation:<\/strong> CO<sub>3<\/sub><sup>2-<\/sup>(s or aq) + 2H<sup>+<\/sup>(aq) \u2192 CO<sub>2<\/sub>(g) + H<sub>2<\/sub>O(l)<\/p><\/div>\n      <\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Acids with Metals and Carbonates<\/h2>\n<p>Answer three short questions that use observations and products for reactions this page has not shown you.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"634\"><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card purple\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">6<\/div><h2>Choosing the Correct Salt Formula<\/h2><\/div>\n        <p>The name of the salt depends on the acid used and the positive ion supplied by the base, metal or carbonate.<\/p>\n        <div class=\"ols-table-wrap\">\n          <table class=\"ols-table\">\n            <thead>\n              <tr>\n                <th>Acid used<\/th>\n                <th>Salt type formed<\/th>\n                <th>Example salt<\/th>\n              <\/tr>\n            <\/thead>\n            <tbody>\n              <tr>\n                <td data-label=\"Acid used\">Hydrochloric acid, HCl<\/td>\n                <td data-label=\"Salt type formed\">Chloride<\/td>\n                <td data-label=\"Example salt\">MgCl<sub>2<\/sub><\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Acid used\">Sulfuric acid, H<sub>2<\/sub>SO<sub>4<\/sub><\/td>\n                <td data-label=\"Salt type formed\">Sulfate<\/td>\n                <td data-label=\"Example salt\">MgSO<sub>4<\/sub><\/td>\n              <\/tr>\n              <tr>\n                <td data-label=\"Acid used\">Nitric acid, HNO<sub>3<\/sub><\/td>\n                <td data-label=\"Salt type formed\">Nitrate<\/td>\n                <td data-label=\"Example salt\">Mg(NO<sub>3<\/sub>)<sub>2<\/sub><\/td>\n              <\/tr>\n            <\/tbody>\n          <\/table>\n        <\/div>\n        <div class=\"ols-key-box\"><p><strong>Exam focus:<\/strong> do not just memorise the word equation. Use the ions present to write a correct salt formula, then balance the full equation.<\/p><\/div>\n      <\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Name That Salt<\/h2>\n<p>Pick the correct salt formula for five new acid reactions.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-635\" class=\"h5p-iframe\" data-content-id=\"635\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Salt Formulae Single Choice Set: Which Salt Forms?\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <div class=\"ols-zoom-card\">\n        <div class=\"ols-zoom-card-image\">\n          <img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/05\/Chemical-reactions-of-acids-infographic.webp\" alt=\"Summary infographic showing typical chemical reactions of acids\" class=\"ols-zoomable-img ols-lightbox-target\" draggable=\"false\">\n        <\/div>\n        <div class=\"ols-zoom-card-caption\">\n          <p>Use the acid to identify the negative ion in the salt, then use the reacting metal, base or carbonate to identify the positive ion.<\/p>\n        <\/div>\n      <\/div>\n\n      <article class=\"ols-note-card orange\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">7<\/div><h2>How to Write Ionic Equations for Acid Reactions<\/h2><\/div>\n        <p>To write an ionic equation, show aqueous ionic substances as their ions, then remove any ions that appear unchanged on both sides. These unchanged ions are called <strong>spectator ions<\/strong>.<\/p>\n        <ol>\n          <li>Start from a correct balanced full equation.<\/li>\n          <li>Split aqueous acids, soluble salts and soluble alkalis into ions.<\/li>\n          <li>Keep solids, liquids, gases and covalent substances together.<\/li>\n          <li>Cancel spectator ions that are unchanged on both sides.<\/li>\n          <li>Check that atoms and charges are balanced.<\/li>\n        <\/ol>\n        <div class=\"ols-definition-box\"><p><strong>Spectator ion:<\/strong> an ion present in the reaction mixture that does not change during the chemical reaction.<\/p><\/div>\n        <div class=\"ols-key-box\"><p><strong>Useful summary:<\/strong> acid-metal reactions often reduce to metal + H<sup>+<\/sup> ions, while acid-carbonate reactions often reduce to carbonate ions + H<sup>+<\/sup> ions.<\/p><\/div>\n      <\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Spot the Spectator Ions<\/h2>\n<p>In each round, pick the one accurate statement about the ions in the reaction.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-289\" class=\"h5p-iframe\" data-content-id=\"289\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Spectator Ions Summary: Which Ions Do Not Change?\"><\/iframe><\/div><\/div>\n<\/section>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Quick Check: Ionic Equations for Acid Reactions<\/h2>\n<p>Write the full and ionic equations on paper before you flip each card.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-640\" class=\"h5p-iframe\" data-content-id=\"640\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Acid Reactions Flip Cards: Write the Ionic Equation\"><\/iframe><\/div><\/div>\n<\/section>\n\n      <article class=\"ols-note-card soft\">\n        <div class=\"ols-note-title\"><div class=\"ols-note-icon\">8<\/div><h2>Common Exam Points<\/h2><\/div>\n        <ul>\n          <li>A salt forms when the H<sup>+<\/sup> ion of an acid is replaced by a metal ion or ammonium ion.<\/li>\n          <li>Bases neutralise acids. Alkalis are soluble bases that release OH<sup>&#8211;<\/sup> ions in water.<\/li>\n          <li>Acid + metal produces a salt and hydrogen gas.<\/li>\n          <li>Acid + metal carbonate produces a salt, carbon dioxide and water.<\/li>\n          <li>Acid + metal hydroxide produces a salt and water.<\/li>\n          <li>Hydrochloric acid forms chlorides, sulfuric acid forms sulfates and nitric acid forms nitrates.<\/li>\n          <li>Fizzing in acid-metal reactions is usually hydrogen gas.<\/li>\n          <li>Fizzing in acid-carbonate reactions is carbon dioxide gas.<\/li>\n          <li>When writing ionic equations, remove spectator ions that appear unchanged on both sides.<\/li>\n          <li>Always check both atom balance and charge balance in an ionic equation.<\/li>\n        <\/ul>\n      <\/article>\n\n      \n\n      <section class=\"ols-quicksnap-card\">\n        <h2>QuickSnap<\/h2>\n        <p>This text summary condenses the page into the essential exam ideas.<\/p>\n        <ul class=\"ols-quicksnap-list\">\n          <li><strong>Acids supply H<sup>+<\/sup> ions:<\/strong> these ions drive typical acid reactions in aqueous solution.<\/li>\n          <li><strong>Neutralisation:<\/strong> H<sup>+<\/sup>(aq) reacts with OH<sup>&#8211;<\/sup>(aq) to form H<sub>2<\/sub>O(l).<\/li>\n          <li><strong>Metals:<\/strong> acid + metal \u2192 salt + hydrogen.<\/li>\n          <li><strong>Carbonates:<\/strong> acid + carbonate \u2192 salt + carbon dioxide + water.<\/li>\n          <li><strong>Salt names:<\/strong> HCl forms chlorides, H<sub>2<\/sub>SO<sub>4<\/sub> forms sulfates and HNO<sub>3<\/sub> forms nitrates.<\/li>\n          <li><strong>Ionic equations:<\/strong> split aqueous ionic substances into ions, then cancel spectator ions.<\/li>\n        <\/ul>\n      <\/section>\n\n      <div class=\"ols-image-lightbox\" id=\"olsImageLightboxTypicalAcids001\" aria-hidden=\"true\" role=\"dialog\" aria-modal=\"true\" aria-label=\"Expanded revision image\">\n        <div class=\"ols-image-lightbox-inner\">\n          <button class=\"ols-image-lightbox-close\" type=\"button\" aria-label=\"Close enlarged image\">\u00d7<\/button>\n          <img decoding=\"async\" class=\"ols-image-lightbox-img\" src=\"\" alt=\"\">\n        <\/div>\n      <\/div>\n\n      <script>\n        (function(){\n          var page = document.querySelector(\".ols-typical-reactions-of-acids-page\");\n          if (!page) {\n            return;\n          }\n\n          var lightbox = page.querySelector(\"#olsImageLightboxTypicalAcids001\");\n          if (!lightbox) {\n            return;\n          }\n\n          var lightboxImage = lightbox.querySelector(\".ols-image-lightbox-img\");\n          var closeButton = lightbox.querySelector(\".ols-image-lightbox-close\");\n          var clickableImages = page.querySelectorAll(\"img.ols-lightbox-target\");\n\n          function openLightbox(image) {\n            lightboxImage.src = image.currentSrc || image.src;\n            lightboxImage.alt = image.alt || \"Expanded revision image\";\n            lightbox.classList.add(\"is-open\");\n            lightbox.setAttribute(\"aria-hidden\", \"false\");\n\n            if (!document.body.dataset.olsPreviousOverflow) {\n              document.body.dataset.olsPreviousOverflow = document.body.style.overflow || \"default\";\n            }\n\n            document.body.style.overflow = \"hidden\";\n          }\n\n          function closeLightbox() {\n            lightbox.classList.remove(\"is-open\");\n            lightbox.setAttribute(\"aria-hidden\", \"true\");\n            lightboxImage.src = \"\";\n\n            if (document.body.dataset.olsPreviousOverflow) {\n              document.body.style.overflow = document.body.dataset.olsPreviousOverflow === \"default\" ? \"\" : document.body.dataset.olsPreviousOverflow;\n              delete document.body.dataset.olsPreviousOverflow;\n            }\n          }\n\n          clickableImages.forEach(function(image){\n            image.addEventListener(\"click\", function(event){\n              event.preventDefault();\n              event.stopPropagation();\n              openLightbox(image);\n            });\n          });\n\n          closeButton.addEventListener(\"click\", closeLightbox);\n\n          lightbox.addEventListener(\"click\", function(event){\n            if (event.target === lightbox) {\n              closeLightbox();\n            }\n          });\n\n          document.addEventListener(\"keydown\", function(event){\n            if (event.key === \"Escape\" && lightbox.classList.contains(\"is-open\")) {\n              closeLightbox();\n            }\n          });\n        })();\n      <\/script>\n\n      <section class=\"ols-faq-card\">\n        <h2>FAQs<\/h2>\n        <p>These questions address the most common mistakes students make when learning typical reactions of acids.<\/p>\n        <div class=\"ols-faq-list\">\n          <div class=\"ols-faq-item\">\n            <h3>What is formed when an acid reacts with a metal?<\/h3>\n            <p>An acid reacts with a suitable metal to form a salt and hydrogen gas. For example, magnesium reacts with hydrochloric acid to form magnesium chloride and hydrogen.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>What is formed when an acid reacts with a metal carbonate?<\/h3>\n            <p>An acid reacts with a metal carbonate to form a salt, carbon dioxide and water. The carbon dioxide causes fizzing and can be tested using limewater.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>What is the difference between a base and an alkali?<\/h3>\n            <p>A base neutralises an acid. An alkali is a soluble base that releases OH<sup>&#8211;<\/sup> ions in aqueous solution.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>How do I know whether a salt is a chloride, sulfate or nitrate?<\/h3>\n            <p>The acid used determines the negative ion in the salt. Hydrochloric acid forms chlorides, sulfuric acid forms sulfates and nitric acid forms nitrates.<\/p>\n          <\/div>\n          <div class=\"ols-faq-item\">\n            <h3>Why do different acid reactions sometimes have the same ionic equation?<\/h3>\n            <p>Different full equations can contain spectator ions. When these unchanged ions are removed, the net ionic equation may be the same because the same reacting particles are involved.<\/p>\n          <\/div>\n        <\/div>\n      <\/section>\n\n      <section class=\"ols-related-card\">\n        <h2>Related Topics<\/h2>\n        <p>Use these pages next to strengthen the surrounding skills needed for equations, ionic equations and quantitative chemistry.<\/p>\n        <div class=\"ols-related-grid\">\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-3-amount-of-substance\/atoms-elements-and-molecules\/\">Atoms, Elements and Molecules<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/equations-and-reaction-types\/writing-chemical-equations\/\">Writing Chemical Equations<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-2-compounds-formulae-and-equations\/equations-and-reaction-types\/\">Displacement Reactions<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-4-acids\/ionic-and-full-equations\/\">Ionic Equations<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-3-amount-of-substance\/mole-calculations\/\">Mole Calculations<\/a>\n          <a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-2-2-bonding-and-structure\/ionic-bonding\/\">Ionic Bonding<\/a>\n        <\/div>\n      <\/section>\n\n      <section class=\"ols-attribution-card\">\n        <p><strong>Copyright notice:<\/strong> This OLS revision content, including the explanations, layout, diagrams, tables and embedded learning structure, is authored for Online Learning System by Dr. Mohammed Al-Fatah. It may not be copied, reproduced, redistributed or adapted without written permission.<\/p>\n      <\/section>\n\n      <script type=\"application\/ld+json\">\n{\n  \"@context\": \"https:\/\/schema.org\",\n  \"@graph\": [\n    {\n      \"@type\": \"WebPage\",\n      \"@id\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-4-acids\/typical-reactions-of-acids\/#webpage\",\n      \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/ocr-a\/2-1-4-acids\/typical-reactions-of-acids\/\",\n      \"name\": \"Typical Reactions of Acids - OCR A Level Chemistry A Revision Notes\",\n      \"description\": \"Revision notes covering typical reactions of acids, including neutralisation, acid-metal reactions, acid-carbonate reactions, salts and ionic equations.\",\n      \"inLanguage\": \"en-GB\",\n      \"isPartOf\": {\n        \"@type\": \"WebSite\",\n        \"@id\": 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