{"id":8139,"date":"2026-09-16T17:24:23","date_gmt":"2026-09-16T16:24:23","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/choosing-solvents\/"},"modified":"2026-10-14T09:13:57","modified_gmt":"2026-10-14T08:13:57","slug":"choosing-solvents","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/choosing-solvents\/","title":{"rendered":"Choosing Solvents"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-imf-page\">\n  <style>\n    .ols-revision-page {\n      --navy: #1C244B;\n      --blue: #2563eb;\n      --soft-blue: #eef4ff;\n      --soft-red: #fff7f7;\n      --soft-purple: #f7f0ff;\n      --soft-green: #f0f7f1;\n      --gold: #c9973a;\n      --grey-text: #667085;\n      --body-text: #1f2937;\n      --border: rgba(28, 36, 75, 0.14);\n      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 font-size: 14px;\n      line-height: 1;\n      font-weight: 700;\n      letter-spacing: 0.01em;\n      box-shadow: 0 10px 22px rgba(10, 102, 194, 0.24);\n      position: relative;\n      overflow: hidden;\n      transition: transform 0.22s ease, box-shadow 0.22s ease;\n    }\n    .ols-linkedin-pill:hover {\n      transform: translateY(-3px) scale(1.03);\n      box-shadow: 0 16px 34px rgba(10, 102, 194, 0.34), 0 0 0 6px rgba(10, 102, 194, 0.10);\n    }\n    .ols-linkedin-icon { width: 18px; height: 18px; display: block; flex-shrink: 0; }\n    .ols-attribution-card {\n      background: linear-gradient(135deg, #ffffff, #f8fbff);\n      border: 1px solid rgba(28, 36, 75, 0.14);\n      border-radius: 28px;\n      box-shadow: 0 18px 45px rgba(28, 36, 75, 0.10);\n      padding: 34px;\n      margin-bottom: 24px;\n      overflow: hidden;\n      box-sizing: border-box;\n    }\n    .ols-attribution-card p {\n      margin: 0;\n      font-size: 14px;\n      line-height: 1.65;\n      font-weight: 300;\n      color: #667085;\n    }\n    .ols-attribution-card strong { font-weight: 700; color: #1C244B; }\n      .ols-note-card h3 { margin: 22px 0 8px; font-size: 18px; line-height: 1.25; font-weight: 500; color: var(--navy); }\n  \n    .ols-figure-placeholder .ols-placeholder-box { border: 2px dashed #c9973a; background: #fffaf0; border-radius: 16px; padding: 26px 22px; font-weight: 700; color: #7a4b12; text-align: center; line-height: 1.6; }\n    .ols-figure-placeholder .ols-figure-image { background: transparent; }\n    .ols-figure-placeholder { background: #ffffff; border: 1px solid rgba(28, 36, 75, 0.12); border-radius: 22px; padding: 14px; margin: 18px 0 6px; }\n    .ols-figure-placeholder .ols-figure-caption p { margin: 10px 0 0; font-size: 14px; color: #667085; text-align: center; }\n<\/style>\n\n    <aside class=\"ols-sidebar\">\n  <div class=\"ols-sidebar-header\">\n    <h3>Revision Notes<\/h3>\n    <p>A Level Chemistry<\/p>\n  <\/div>\n\n  <div class=\"ols-topic-group\">\n    <h4>Topic 7 Intermolecular Forces<\/h4>\n\n    <ul class=\"ols-topic-list\">\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/\">Topic 7 Overview<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/london-forces\/\">London Forces<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/permanent-dipole-dipole-forces\/\">Permanent Dipole-Dipole Forces<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/hydrogen-bonding\/\">Hydrogen Bonding<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/anomalous-properties-of-water\/\">Anomalous Properties of Water<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/boiling-temperature-trends\/\">Boiling Temperature Trends<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/choosing-solvents\/\">Choosing Solvents<\/a>\n      <\/li>\n    <\/ul>\n  <\/div>\n\n  <div class=\"ols-topic-group\">\n    <h4>Other Topics<\/h4>\n\n    <ul class=\"ols-topic-list\">\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-3-bonding-structure\/\">Bonding &amp; Structure<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-5-alkenes\/\">Alkenes<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-6-energetics\/\">Energetics<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-8A-redox-chemistry\/\">Redox Chemistry<\/a>\n      <\/li>\n    <\/ul>\n  <\/div>\n<\/aside>\n\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    if (!sidebar) return false;\r\n\r\n    var 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href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/\">Edexcel International<\/a> \/\n<a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/\">Topic 7 Intermolecular Forces<\/a> \/\n<span>Choosing Solvents<\/span>\n<\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Choosing Solvents<\/h1>\n        <p class=\"ols-page-intro\">A concise revision guide to how intermolecular forces decide the choice of solvent: hydration of ions, alcohols dissolving in water by hydrogen bonding, why water is a poor solvent for halogenoalkanes, and like-dissolves-like for non-aqueous solvents, for Edexcel International A Level Chemistry.<\/p>\n        <div class=\"ols-badges\">\n<div class=\"ols-badge\">Exam board: Edexcel International<\/div>\n<div class=\"ols-badge\">Unit 2: WCH12\/01<\/div>\n<div class=\"ols-badge\">Topic 7: Intermolecular Forces<\/div>\n<\/div>\n      <\/header>\n\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: Solutes, Solvents and Layers<\/h2>\n<p>Three quick questions on the GCSE ideas about dissolving that this page builds on.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"779\"><\/div><\/div>\n<\/section>\n<article class=\"ols-note-card soft\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">1<\/div>\n<h2>What Decides Whether Something Dissolves<\/h2>\n<\/div>\n<p>A substance dissolves in a solvent when the attractions <strong>formed<\/strong> between solute and solvent particles are strong enough to compensate for the attractions <strong>broken<\/strong> within the solute and within the solvent.<\/p><p>Dissolving is therefore a balance of intermolecular forces. The rule of thumb &#8220;like dissolves like&#8221; simply means that the new solute-solvent attractions must be of a similar kind and strength to the ones being lost.<\/p><p>The two do not have to balance exactly: a small energy cost can still be paid. That is why solids such as ammonium nitrate dissolve even though the solution gets colder as they do.<\/p>\n<p>Three questions decide the outcome: what holds the solute together (ionic lattice, hydrogen bonds, permanent dipoles or London forces), what holds the solvent together, and what the two can form with each other.<\/p>\n<div class=\"ols-key-box\">\n<p><strong>Key idea:<\/strong> Energy is needed to break solute-solute and solvent-solvent attractions; energy is released when solute-solvent attractions form. Dissolving happens when the two roughly balance.<\/p>\n<\/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: What Holds the Solute Together?<\/h2>\n<p>Pick the strongest attraction holding each solute together.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-780\" class=\"h5p-iframe\" data-content-id=\"780\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Choosing Solvents Quick Fire: What Holds Each Solute Together\"><\/iframe><\/div><\/div>\n<\/section>\n\n<article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">2<\/div>\n<h2>Water Dissolving Ionic Compounds: Hydration of Ions<\/h2>\n<\/div>\n<p>Water is polar: its oxygen is \u03b4- and its hydrogens \u03b4+.<\/p><p>When an ionic solid such as sodium chloride is placed in water, the \u03b4- oxygen atoms of water molecules are attracted to the Na\u207a ions and the \u03b4+ hydrogen atoms to the Cl\u207b ions.<\/p><p>Each ion that leaves the lattice becomes surrounded by a shell of correctly oriented water molecules. This is <strong>hydration<\/strong>, and the attractions formed are called <strong>ion-dipole attractions<\/strong>.<\/p>\n<p>The energy released by hydrating the ions is comparable to the energy needed to break up the lattice, so sodium chloride dissolves.<\/p>\n<p>Magnesium oxide does not dissolve appreciably. Its ions carry 2+ and 2- charges and are small, so they pull on each other far more strongly than Na\u207a and Cl\u207b do.<\/p>\n<p>Breaking that lattice costs far more energy than hydrating the ions can release.<\/p>\n<div class=\"ols-figure-card ols-zoom-pop\">\n<div class=\"ols-figure-image\">\n<a class=\"ols-image-fullscreen-link\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/dissolving-sodium-chloride-hydration-and-ion-dipole-attractions.jpg\" target=\"_blank\" rel=\"noopener\" aria-label=\"Open image fullscreen\">\n<img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/dissolving-sodium-chloride-hydration-and-ion-dipole-attractions.jpg\" alt=\"Sodium chloride dissolving: water molecules orient their oxygen atoms towards sodium ions and their hydrogen atoms towards chloride ions\" data-fullscreen-src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/dissolving-sodium-chloride-hydration-and-ion-dipole-attractions.jpg\">\n<\/a>\n<\/div>\n<div class=\"ols-figure-caption\"><p>Hydration: water molecules orient their \u03b4- oxygens towards cations and their \u03b4+ hydrogens towards anions, and the attractions formed pay for breaking the lattice.<\/p><\/div>\n<\/div>\n<div class=\"ols-key-box\">\n<p><strong>Exam sentence:<\/strong> Sodium chloride dissolves in water because the \u03b4- oxygen atoms of water molecules attract the Na\u207a ions and the \u03b4+ hydrogen atoms attract the Cl\u207b ions; the energy released when the ions are hydrated compensates for the energy needed to break the ionic lattice.<\/p>\n<\/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: One Salt Dissolves, One Does Not<\/h2>\n<p>Drag the words into the gaps to explain why one salt dissolves and the other does not.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-542\" class=\"h5p-iframe\" data-content-id=\"542\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Choosing Solvents Drag: Calcium Nitrate and Barium Sulfate\"><\/iframe><\/div><\/div>\n<\/section>\n\n<article class=\"ols-note-card purple\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">3<\/div>\n<h2>Water Dissolving Alcohols: Hydrogen Bonding<\/h2>\n<\/div>\n<p>Methanol, ethanol and propan-1-ol mix with water in all proportions because the O-H group of the alcohol forms hydrogen bonds with water molecules.<\/p>\n<p>The hydrogen bonds formed between alcohol and water are similar in strength to the hydrogen bonds broken within the water and within the alcohol, so there is no barrier to mixing.<\/p>\n<p>As the carbon chain grows the alcohol becomes less soluble. Methanol, ethanol and propan-1-ol mix in all proportions; butan-1-ol dissolves only to about 7 g per 100 g of water and hexan-1-ol to less than 1 g.<\/p><p>The long non-polar chain can only form London forces with water. To make room for it, water must break hydrogen bonds that the chain cannot replace.<\/p><p>The hydrocarbon part outweighs the single O-H group.<\/p>\n<div class=\"ols-figure-card\">\n<div class=\"ols-figure-image\"><img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/skel-79-ethanol-chloroethane-water-a.svg\" alt=\"Ethanol forming hydrogen bonds with water molecules\" width=\"1381\" height=\"944\">\n<img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/skel-79-ethanol-chloroethane-water-b.svg\" alt=\"Chloroethane next to water molecules, showing that it does not form hydrogen bonds with water\" width=\"1359\" height=\"752\"><\/div>\n<div class=\"ols-figure-caption\"><p>Ethanol dissolves because its O-H group replaces the water hydrogen bonds it disrupts; chloroethane cannot form hydrogen bonds with water, so it does not dissolve.<\/p><\/div>\n<\/div>\n<div class=\"ols-key-box\">\n<p><strong>Key idea:<\/strong> Small alcohols are miscible with water because they hydrogen bond with it; solubility falls as the non-polar chain lengthens.<\/p>\n<\/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: Two Alcohols, Same Electrons<\/h2>\n<p>Choose the statement that explains the difference in solubility.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-543\" class=\"h5p-iframe\" data-content-id=\"543\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Choosing Solvents MCQ: Three O-H Groups Against a Long Chain\"><\/iframe><\/div><\/div>\n<\/section>\n\n<article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">4<\/div>\n<h2>Why Water Is a Poor Solvent for Halogenoalkanes<\/h2>\n<\/div>\n<p>Halogenoalkanes such as chloroethane are polar molecules: the C-Cl bond has a permanent dipole. Yet they are almost insoluble in water.<\/p><div class=\"ols-key-box\"><p><strong>Key idea:<\/strong> The reason is that a halogenoalkane <strong>cannot form hydrogen bonds<\/strong> with water: it has no hydrogen bonded to N, O or F, and the halogen atom is a poor acceptor of hydrogen bonds.<\/p><\/div><p>To dissolve, the halogenoalkane would have to break hydrogen bonds between water molecules to make space for itself. The weak permanent dipole-permanent dipole interactions it could form with water would not pay back that energy.<\/p>\n<p>The same argument applies to many polar molecules without an O-H or N-H group, and it explains why &#8220;polar&#8221; does not automatically mean &#8220;soluble in water&#8221;.<\/p><p>The question is always whether the solute can form hydrogen bonds with water, or at least attractions comparable to the ones it disrupts.<\/p><div class=\"ols-key-box\"><p><strong>Key idea:<\/strong> A solute does not have to <strong>donate<\/strong> a hydrogen bond to dissolve: <strong>accepting<\/strong> one is enough.<\/p><\/div><p>Propanone has no O-H, but the lone pairs on its C=O oxygen accept hydrogen bonds from the \u03b4+ hydrogens of water. This is why it mixes with water in all proportions.<\/p><p>A halogen atom accepts far too weakly for that.<\/p>\n<div class=\"ols-table-wrap\">\n<table class=\"ols-table\">\n<thead>\n<tr><th>Solute<\/th><th>Polar?<\/th><th>Can hydrogen bond with water?<\/th><th>Soluble in water?<\/th><\/tr>\n<\/thead>\n<tbody>\n<tr><td><strong>Ethanol, C\u2082H\u2085OH<\/strong><\/td><td>yes<\/td><td>yes, O-H<\/td><td>miscible<\/td><\/tr>\n<tr><td><strong>Propanone, CH\u2083COCH\u2083<\/strong><\/td><td>yes<\/td><td>yes, C=O accepts from water<\/td><td>miscible<\/td><\/tr>\n<tr><td><strong>Chloroethane, C\u2082H\u2085Cl<\/strong><\/td><td>yes<\/td><td>no<\/td><td>almost insoluble<\/td><\/tr>\n<tr><td><strong>Hexane, C\u2086H\u2081\u2084<\/strong><\/td><td>no<\/td><td>no<\/td><td>insoluble<\/td><\/tr>\n<tr><td><strong>Sodium chloride<\/strong><\/td><td>ionic<\/td><td>ions are hydrated<\/td><td>soluble<\/td><\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<div class=\"ols-key-box\">\n<p><strong>Exam sentence:<\/strong> Chloroethane does not dissolve in water because chloroethane molecules cannot form hydrogen bonds with water molecules; the hydrogen bonds between water molecules that would have to be broken are not replaced by attractions of similar strength.<\/p>\n<\/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: Pick the Accurate Statement<\/h2>\n<p>Choose the one accurate statement about polar solutes and water in each round.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-545\" class=\"h5p-iframe\" data-content-id=\"545\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Choosing Solvents Summary: Polar Does Not Mean Soluble\"><\/iframe><\/div><\/div>\n<\/section>\n\n<article class=\"ols-note-card soft\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">5<\/div>\n<h2>Non-Aqueous Solvents: Like Dissolves Like<\/h2>\n<\/div>\n<p>Substances that water cannot dissolve usually dissolve in a solvent whose intermolecular forces match their own.<\/p>\n<p>A <strong>non-polar solute<\/strong> dissolves in a <strong>non-polar solvent<\/strong> because the London forces broken between solute molecules and between solvent molecules are replaced by London forces of similar strength between solute and solvent.<\/p>\n<p>Iodine dissolves readily in hexane or cyclohexane but only slightly in water. Grease and candle wax dissolve in hexane; halogenoalkanes dissolve in hexane and in ethanol.<\/p>\n<div class=\"ols-table-wrap\">\n<table class=\"ols-table\">\n<thead>\n<tr><th>Solute<\/th><th>Forces within the solute<\/th><th>Good solvent<\/th><th>Poor solvent<\/th><\/tr>\n<\/thead>\n<tbody>\n<tr><td><strong>Iodine, I\u2082<\/strong><\/td><td>London forces<\/td><td>hexane, cyclohexane<\/td><td>water<\/td><\/tr>\n<tr><td><strong>Candle wax (long alkanes)<\/strong><\/td><td>London forces<\/td><td>hexane, white spirit<\/td><td>water<\/td><\/tr>\n<tr><td><strong>Chloroethane<\/strong><\/td><td>permanent dipole-permanent dipole interactions and London forces<\/td><td>hexane, ethanol<\/td><td>water<\/td><\/tr>\n<tr><td><strong>Sodium chloride<\/strong><\/td><td>ionic lattice<\/td><td>water<\/td><td>hexane<\/td><\/tr>\n<tr><td><strong>Sugar (sucrose)<\/strong><\/td><td>hydrogen bonds (many O-H)<\/td><td>water<\/td><td>hexane<\/td><\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<p>The choice of solvent matters in practical chemistry. An organic product is extracted from an aqueous mixture with a non-polar solvent in a separating funnel.<\/p>\n<p>The product dissolves in the organic layer and the ionic impurities stay in the water.<\/p>\n<p>Two layers form because neither liquid dissolves in the other: the water molecules hold on to each other by hydrogen bonds that a non-polar solvent cannot replace.<\/p>\n<p>The organic layer is usually the upper one, because most organic solvents are less dense than water. You can identify the layers by adding a little more water and seeing which one grows.<\/p>\n<p>The lower layer is run out of the tap first.<\/p>\n<p>Ethanol is useful because it is both at once: the O-H group hydrogen bonds like water, while the ethyl group sits happily among non-polar molecules. Ethanol therefore dissolves some ionic solids and many organic ones, which is why it appears in the table as a solvent for chloroethane.<\/p>\n<div class=\"ols-key-box\">\n<p><strong>Exam focus:<\/strong> When asked to choose or justify a solvent, name the strongest force in the solute, name the strongest force in the candidate solvent, and say whether the solute-solvent attractions formed can replace those broken.<\/p>\n<\/div>\n<div class=\"ols-figure-card ols-zoom-pop\">\n<div class=\"ols-figure-image\">\n<a class=\"ols-image-fullscreen-link\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/t17x-s3likedissolves.jpg\" target=\"_blank\" rel=\"noopener\" aria-label=\"Open image fullscreen\">\n<img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/t17x-s3likedissolves.jpg\" alt=\"Table matching five solutes to good and poor solvents, with a separating funnel showing organic and aqueous layers.\" data-fullscreen-src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/t17x-s3likedissolves.jpg\">\n<\/a>\n<\/div>\n<div class=\"ols-figure-caption\"><p>A solute dissolves in a solvent whose intermolecular forces match its own, which is why an organic product can be extracted into a non-polar layer away from ionic impurities.<\/p><\/div>\n<\/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: Choose the Solvent<\/h2>\n<p>Click every substance that dissolves better in a non-polar solvent than in water.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-544\" class=\"h5p-iframe\" data-content-id=\"544\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Choosing Solvents Mark the Words: Which Solutes Prefer a Non-Polar Solvent\"><\/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: Dissolving from Start to Finish<\/h2>\n<p>Pick the one accurate statement in each round to check the whole page.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-1340\" class=\"h5p-iframe\" data-content-id=\"1340\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Choosing Solvents Summary: Broken, Formed and Which Layer\"><\/iframe><\/div><\/div>\n<\/section>\n\n<article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">6<\/div>\n<h2>Common Exam Points<\/h2>\n<\/div>\n<h3>Explain why sodium chloride dissolves in water<\/h3><p>\u03b4- oxygen of water attracts Na\u207a, \u03b4+ hydrogen attracts Cl\u207b; the energy released on hydrating the ions compensates for the energy needed to break the lattice.<\/p>\n<h3>Explain why ethanol mixes with water but hexane does not<\/h3><p>Ethanol forms hydrogen bonds with water; hexane can only form London forces, which cannot replace the hydrogen bonds broken in water.<\/p>\n<h3>Explain why a polar halogenoalkane is insoluble in water<\/h3><p>It cannot hydrogen bond with water; the attractions it forms do not compensate for the water hydrogen bonds broken.<\/p>\n<h3>Suggest a solvent for iodine<\/h3><p>A non-polar solvent such as hexane, because both are held by London forces only.<\/p>\n<\/article>\n\n<section class=\"ols-faq-card\">\n<h2>FAQs<\/h2>\n<p>Use these quick answers to check how intermolecular forces decide what dissolves in what.<\/p>\n\n<div class=\"ols-faq-list\">\n<div class=\"ols-faq-item\">\n<h3>Why does sodium chloride dissolve in water?<\/h3>\n<p>The \u03b4- oxygen atoms of water molecules are attracted to the Na\u207a ions and the \u03b4+ hydrogen atoms to the Cl\u207b ions, so the ions become hydrated. The energy released by hydration compensates for the energy needed to break up the ionic lattice.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Why do small alcohols mix with water?<\/h3>\n<p>The O-H group of the alcohol forms hydrogen bonds with water molecules that are similar in strength to the ones being broken, so there is no barrier to mixing. Solubility falls as the carbon chain lengthens.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Why does a polar halogenoalkane not dissolve in water?<\/h3>\n<p>It has no hydrogen bonded to N, O or F, so it cannot form hydrogen bonds with water. The water-water hydrogen bonds that must be broken to make room for it are not replaced by attractions of similar strength.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>What does &#8220;like dissolves like&#8221; actually mean?<\/h3>\n<p>It means the solute-solvent attractions formed must be of the same kind and strength as the solute-solute and solvent-solvent attractions broken. Iodine dissolves in hexane because both are held only by London forces.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Does polar always mean water-soluble?<\/h3>\n<p>No. Chloroethane is polar but almost insoluble in water, because its dipole is not enough to replace the hydrogen bonds it disrupts. The question to ask is whether the solute can hydrogen bond with water.<\/p>\n<\/div>\n<\/div>\n<\/section>\n\n      <!-- author card (moved to the end, 10 Oct 2026) -->\n      <div class=\"ols-author\">\n\n    <img decoding=\"async\"\n      class=\"ols-author-avatar-img\"\n      src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/05\/Author-Profile.jpeg\"\n      alt=\"Dr. Mohammed Al-Fatah\"\n    >\n\n    <div class=\"ols-author-content\">\n\n      <h2 class=\"ols-author-title\">\n        Written by: Dr. Mohammed Al-Fatah\n      <\/h2>\n\n      <p class=\"ols-author-description\">\n        Chemistry specialist revision notes for A Level Chemistry.\n      <\/p>\n\n      <a\n        class=\"ols-linkedin-pill\"\n        href=\"https:\/\/www.linkedin.com\/in\/doctormohammedfatah\/\"\n        target=\"_blank\"\n        rel=\"noopener noreferrer\"\n      >\n        <svg class=\"ols-linkedin-icon\" viewBox=\"0 0 24 24\" fill=\"currentColor\" aria-hidden=\"true\">\n          <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\"\/>\n        <\/svg>\n        View LinkedIn Profile\n      <\/a>\n\n    <\/div>\n\n  <\/div>\n\n<section class=\"ols-related-card\">\n<h2>Related Topic 7 Pages<\/h2>\n<p>Use these pages to connect the three intermolecular forces with the physical properties they explain.<\/p>\n<div class=\"ols-related-grid\">\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/london-forces\/\">London Forces<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/permanent-dipole-dipole-forces\/\">Permanent Dipole-Dipole Forces<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/hydrogen-bonding\/\">Hydrogen Bonding<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/anomalous-properties-of-water\/\">Anomalous Properties of Water<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/boiling-temperature-trends\/\">Boiling Temperature Trends<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-3-bonding-structure\/polar-and-non-polar-molecules\/\">Polar &amp; Non-Polar Molecules<\/a>\n<\/div>\n<\/section>\n<section class=\"ols-attribution-card ols-attr-std\" aria-label=\"Copyright notice\">\n<style id=\"ols-attribution-card-css\">.ols-attribution-card.ols-attr-std{background:linear-gradient(135deg,#ffffff,#f8fbff);border:1px solid rgba(28,36,75,0.14);border-radius:28px;box-shadow:0 18px 45px rgba(28,36,75,0.10);padding:34px;margin:24px 0;overflow:hidden;font-family:Poppins,Arial,sans-serif;box-sizing:border-box}.ols-attribution-card.ols-attr-std *{box-sizing:border-box}.ols-attribution-card.ols-attr-std p{margin:0;font-size:14px;line-height:1.65;font-weight:300;color:#667085}.ols-attribution-card.ols-attr-std strong{font-weight:700;color:#1C244B}@media (max-width:760px){.ols-attribution-card.ols-attr-std{padding:24px 18px;border-radius:22px}}<\/style>\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    <\/main>\n  \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\/edexcel-international\/topic-7-intermolecular-forces\/choosing-solvents\/#webpage\",\n      \"url\": \"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/choosing-solvents\/\",\n      \"name\": \"Choosing Solvents | Topic 7 Intermolecular Forces | Online Learning System\",\n      \"description\": \"Choosing solvents for Edexcel International A Level Chemistry: hydration of ions, alcohols and hydrogen bonding, halogenoalkanes in water, non-aqueous solvents and like dissolves like.\",\n      \"isPartOf\": {\n        \"@id\": 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