{"id":66492,"date":"2026-10-06T17:30:36","date_gmt":"2026-10-06T14:30:36","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66492"},"modified":"2026-10-06T17:30:36","modified_gmt":"2026-10-06T14:30:36","slug":"boiling-point-elevation-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/boiling-point-elevation-calculator\/","title":{"rendered":"Boiling Point Elevation Calculator"},"content":{"rendered":"<section class=\"not-prose calculator-box\" aria-labelledby=\"calculator-title\"><div class=\"flex items-baseline sm:items-center justify-between gap-2 sm:gap-3\"><div class=\"flex flex-col sm:flex-row sm:items-center gap-2\"><span class=\"icon icon-calculator text-primary-700! text-base! dark:text-primary-300!\" aria-hidden=\"true\"><\/span><h2 id=\"calculator-title\" class=\"text-lg font-display font-bold\">Find the Boiling Point of a Solution<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66492\" data-favorite-title=\"Boiling Point Elevation\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/boiling-point-elevation-calculator\/\" data-favorite-excerpt=\"Calculate the boiling point elevation of a solution from molality, the ebullioscopic constant Kb, and the van &#039;t Hoff factor. Enter the pure solvent&#039;s boiling point to get the new boiling point in \u00b0C and \u00b0F.\" aria-label=\"Add to Favorites\" data-favorite-icon=\"icon icon-chemistry\">\n    <span class=\"icon icon-shape-star-empty\" aria-hidden=\"true\"><\/span>\n  <\/button>\n  <div class=\"calcdash-favorite__tip\" aria-hidden=\"true\">\n   <span class=\"favorite-tooltip\" id=\"favorite-tooltip\"><\/span>\n  <\/div>\n  <span class=\"sr-only\" role=\"status\" id=\"favorite-status\"><\/span>\n<\/div><\/div><form action=\"https:\/\/wpcalc.com\/en\/chemistry\/boiling-point-elevation-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66492\" data-post=\"66492\"><fieldset class=\"fieldset-input is-1\"><legend class=\"sr-only\">Input Fields<\/legend><div class=\"field has-term\" id=\"input-1\"><label for=\"field-1\">Molality (m)<\/label><div class=\"term\">m<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"molality_m\" id=\"field-1\" aria-describedby=\"calc-unit-1 calc-info-1\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 1.5\" min=\"0\" value=\"1.5\"\/><div class=\"unit\" id=\"calc-unit-1\">mol\/kg<\/div><small id=\"calc-info-1\">Moles of solute per kilogram of solvent (not per litre of solution)<\/small><\/div><div class=\"field has-term\" id=\"input-2\"><label for=\"field-2\">Boiling Point Elevation Constant (Kb)<\/label><div class=\"term\">Kb<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"boiling_point_elevation_constant_kb\" id=\"field-2\" aria-describedby=\"calc-unit-2 calc-info-2\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 0.512\" min=\"0\" value=\"0.512\"\/><div class=\"unit\" id=\"calc-unit-2\">\u00b0C\u00b7kg\/mol<\/div><small id=\"calc-info-2\">Molal boiling point constant of the solvent: water 0.512, ethanol 1.22, benzene 2.53, chloroform 3.63 (\u00b0C\u00b7kg\/mol)<\/small><\/div><div class=\"field has-term\" id=\"input-3\"><label for=\"field-3\">van &#039;t Hoff Factor (i)<\/label><div class=\"term\">i<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"van_t_hoff_factor_i\" id=\"field-3\" aria-describedby=\"calc-info-3\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 1\" min=\"1\" value=\"1\"\/><small id=\"calc-info-3\">Number of particles the solute splits into: 1 for sucrose, ~2 for NaCl, ~3 for CaCl\u2082<\/small><\/div><div class=\"field has-term\" id=\"input-4\"><label for=\"field-4\">Pure Solvent Boiling Point (Tb\u00b0)<\/label><div class=\"term\">Tb\u00b0<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><div class=\"field-group\"><input type=\"number\" name=\"pure_solvent_boiling_point_tb\" id=\"field-4\" aria-describedby=\"calc-info-4\" placeholder=\"e.g. 100\" step=\"any\" value=\"100\"\/><div class=\"grid grid-cols-1\"><select id=\"field-5\" name=\"unit\" aria-label=\"Unit\"><option value=\"c\" selected>\u00b0C<\/option><option value=\"f\">\u00b0F<\/option><\/select><svg class=\"pointer-events-none col-start-1 row-start-1 mr-2 size-5 self-center justify-self-end text-gray-500 sm:size-4\" viewBox=\"0 0 16 16\" fill=\"currentColor\" aria-hidden=\"true\" data-slot=\"icon\">\n              <path fill-rule=\"evenodd\" d=\"M4.22 6.22a.75.75 0 0 1 1.06 0L8 8.94l2.72-2.72a.75.75 0 1 1 1.06 1.06l-3.25 3.25a.75.75 0 0 1-1.06 0L4.22 7.28a.75.75 0 0 1 0-1.06Z\" clip-rule=\"evenodd\" \/>\n            <\/svg><\/div><\/div><small id=\"calc-info-4\">Boiling point of the pure solvent with no solute dissolved (water boils at 100 \u00b0C \/ 212 \u00b0F)<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66492\">Calculate<\/button><button type=\"reset\">Reset<\/button><\/div><div class=\"field is-checkbox hidden!\" id=\"field-auto-calc\"><input type=\"checkbox\" id=\"auto-calc\"><label for=\"auto-calc\">Calculate automatically<\/label><small>If enabled, the result will update automatically when you change any value.<\/small><\/div><div class=\"fieldset-result is-hidden\" aria-labelledby=\"result-title\" aria-live=\"polite\" role=\"region\"> <h3 class=\"result-title bg-gradient-to-r from-primary-50 to-gray-50 dark:from-primary-900 dark:to-gray-800\" id=\"result-title\"><span class=\"icon icon-s-pulse\" aria-hidden=\"true\"><\/span> Boiling Point Results<\/h3><div class=\"result-box\"><div class=\"field-result\" id=\"output-1\"><span class=\"field-title\"><span>Boiling Point Elevation<\/span><span class=\"result-term\">\u0394Tb<\/span><\/span><span class=\"field-value\" id=\"result-1\" data-unit=\"\u00b0C\"><\/span><button type=\"button\" class=\"copy-result\" data-tooltip=\"Copy Result\" aria-label=\"Copy Result\"><span class=\"copy-icon icon icon-document-copy\" aria-hidden=\"true\"><\/span><\/button><\/div><div class=\"field-result\" id=\"output-2\"><span class=\"field-title\"><span>Boiling Point Elevation<\/span><span class=\"result-term\">\u0394Tb<\/span><\/span><span class=\"field-value\" id=\"result-2\" data-unit=\"\u00b0F\"><\/span><button type=\"button\" class=\"copy-result\" data-tooltip=\"Copy Result\" aria-label=\"Copy Result\"><span class=\"copy-icon icon icon-document-copy\" aria-hidden=\"true\"><\/span><\/button><\/div><div class=\"field-result\" id=\"output-3\"><span class=\"field-title\"><span>Solution Boiling Point<\/span><span class=\"result-term\">Tb<\/span><\/span><span class=\"field-value\" id=\"result-3\" data-unit=\"\u00b0C\"><\/span><button type=\"button\" class=\"copy-result\" data-tooltip=\"Copy Result\" aria-label=\"Copy Result\"><span class=\"copy-icon icon icon-document-copy\" aria-hidden=\"true\"><\/span><\/button><\/div><div class=\"field-result\" id=\"output-4\"><span class=\"field-title\"><span>Solution Boiling Point<\/span><span class=\"result-term\">Tb<\/span><\/span><span class=\"field-value\" id=\"result-4\" data-unit=\"\u00b0F\"><\/span><button type=\"button\" class=\"copy-result\" data-tooltip=\"Copy Result\" aria-label=\"Copy Result\"><span class=\"copy-icon icon icon-document-copy\" aria-hidden=\"true\"><\/span><\/button><\/div><\/div><div class=\"result-actions\"><button type=\"button\" class=\"copy-link\"><svg viewBox=\"0 0 20 20\" fill=\"currentColor\" aria-hidden=\"true\"><path d=\"M12.232 4.232a2.5 2.5 0 0 1 3.536 3.536l-1.225 1.224a.75.75 0 0 0 1.061 1.06l1.224-1.224a4 4 0 0 0-5.656-5.656l-3 3a4 4 0 0 0 .225 5.865.75.75 0 0 0 .977-1.138 2.5 2.5 0 0 1-.142-3.667l3-3Z\"\/><path d=\"M11.603 7.963a.75.75 0 0 0-.977 1.138 2.5 2.5 0 0 1 .142 3.667l-3 3a2.5 2.5 0 0 1-3.536-3.536l1.225-1.224a.75.75 0 0 0-1.061-1.06l-1.224 1.224a4 4 0 1 0 5.656 5.656l3-3a4 4 0 0 0-.225-5.865Z\"\/><\/svg><span class=\"copy-link__text\">Copy link to this calculation<\/span><\/button><span class=\"sr-only\" role=\"status\" id=\"copy-link-status\"><\/span><\/div><\/div><a href=\"#respond\" class=\"hidden transition-opacity duration-300 opacity-0 w-50 text-sm justify-center items-center gap-2 px-4 py-2 rounded bg-gray-200 text-gray-700 hover:bg-gray-300\" id=\"leave-comment\"><span class=\"icon icon-comments\" aria-hidden=\"true\"><\/span>Leave a Comment<\/a><\/form><\/section><section id=\"calc-reactions\" class=\"not-prose hidden my-12 bg-gradient-to-r from-primary-50 to-gray-50 border border-indigo-100 rounded-xl px-6 py-4 shadow-sm\" data-post=\"66492\" aria-live=\"polite\" aria-labelledby=\"calc-reactions-title\"><p id=\"calc-reactions-title\" class=\"text-sm text-gray-500 text-center mb-2\">How did this result make you feel?<\/p><div role=\"group\" aria-labelledby=\"calc-reactions-title\" class=\"grid grid-cols-3 sm:flex sm:flex-row sm:justify-around gap-4 sm:items-center sm:flex-wrap\"><button type=\"button\" aria-pressed=\"false\" class=\"reaction-btn flex flex-col items-center gap-1 text-sm text-gray-700 hover:text-primary-600 cursor-pointer transition-transform hover:scale-105\" data-reaction=\"like\"><span class=\"reaction-count\" data-reaction-count=\"like\">0<\/span><span class=\"reaction text-3xl\" aria-hidden=\"true\">\ud83d\ude00 <\/span><span class=\"reaction-description font-medium\">Like <\/span><\/button><button type=\"button\" aria-pressed=\"false\" class=\"reaction-btn flex flex-col items-center gap-1 text-sm text-gray-700 hover:text-primary-600 cursor-pointer transition-transform hover:scale-105\" data-reaction=\"helpful\"><span class=\"reaction-count\" data-reaction-count=\"helpful\">0<\/span><span class=\"reaction text-3xl\" aria-hidden=\"true\">\ud83d\udca1 <\/span><span class=\"reaction-description font-medium\">Helpful <\/span><\/button><button type=\"button\" aria-pressed=\"false\" class=\"reaction-btn flex flex-col items-center gap-1 text-sm text-gray-700 hover:text-primary-600 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data-reaction=\"inaccurate\"><span class=\"reaction-count\" data-reaction-count=\"inaccurate\">0<\/span><span class=\"reaction text-3xl\" aria-hidden=\"true\">\u274c <\/span><span class=\"reaction-description font-medium\">Inaccurate <\/span><\/button><\/div><div id=\"reaction-message\" class=\"hidden mt-8 rounded-md border border-primary-100 bg-white\/50 backdrop-blur-sm px-4 py-2 text-sm text-center shadow-sm\"><\/div><\/section><div class=\"calcdash-ad not-prose calcdash-ad--calc_result calcdash-ad--in-article\"><ins class=\"adsbygoogle\" style=\"display:block\" data-ad-client=\"ca-pub-1721569815777345\" data-ad-slot=\"6317458308\" data-ad-layout=\"in-article\" data-ad-format=\"fluid\"><\/ins><script>(adsbygoogle = window.adsbygoogle || []).push({});<\/script><\/div>\n<style id=\"wpcoderpro-inline-1\">.formula-box {\r\n\tborder-bottom: none !important;\r\n}<\/style><section class=\"formula-box\" aria-labelledby=\"formula-title\">\r\n\t<div id=\"formula-title\" class=\"not-prose font-display mb-4\"><span class=\"icon icon-formula\" aria-hidden=\"true\"><\/span><h2>Boiling Point Elevation Formula<\/h2><\/div>\r\n\t<figure class=\"not-prose formula\">\r\n\t\t<figcaption class=\"formula-title\">Formula<\/figcaption>\r\n\t\t<div class=\"text-base text-gray-800\" id=\"formula\">\n\\[ \\Delta T_b = i \\cdot K_b \\cdot m \\]\n\\[ T_b = T_b^\\circ + \\Delta T_b \\]<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(\\Delta T_b\\) \u2014 boiling point elevation (\u00b0C)<\/li>\n<li>\\(i\\) \u2014 van 't Hoff factor (number of particles the solute forms in solution)<\/li>\n<li>\\(K_b\\) \u2014 molal boiling point elevation constant, or ebullioscopic constant, of the solvent (\u00b0C\u00b7kg\/mol)<\/li>\n<li>\\(m\\) \u2014 molality of the solution (mol solute per kg solvent)<\/li>\n<li>\\(T_b^\\circ\\) \u2014 boiling point of the pure solvent (\u00b0C)<\/li>\n<li>\\(T_b\\) \u2014 boiling point of the solution (\u00b0C)<\/li>\n<\/ul>\n<p>The elevation is proportional to the concentration of dissolved particles, not their chemical identity. Adding the elevation to the pure solvent's boiling point gives the temperature at which the solution boils.<\/p>\n<p>\r\n<\/section>\n<style id=\"wpcoderpro-inline-459\">.calculation-box {\r\n\tborder-bottom: none !important;\r\n}<\/style><section id=\"calculation\" class=\"calculation-box\" aria-labelledby=\"calculation-title\">\r\n\t<div id=\"calculation-title\" class=\"not-prose font-display\"><span class=\"icon icon-unordered-list\" aria-hidden=\"true\"><\/span><h2>Boiling Point Elevation \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> 1.5 mol of sucrose is dissolved in 1 kg of water (molality 1.5 mol\/kg). Sucrose does not dissociate, so \\(i = 1\\), and water has \\(K_b = 0.512\\) \u00b0C\u00b7kg\/mol with a normal boiling point of 100 \u00b0C.<\/p>\n<p>\\[ \\Delta T_b = i \\cdot K_b \\cdot m = 1 \\times 0.512 \\times 1.5 = 0.768 \\text{ \u00b0C} \\]<\/p>\n<p>\\[ T_b = 100 + 0.768 = 100.768 \\text{ \u00b0C} \\]<\/p>\n<p><strong>Result:<\/strong> the boiling point rises by 0.768 \u00b0C (1.382 \u00b0F), so the solution boils at 100.768 \u00b0C, or about 213.38 \u00b0F.<\/p>\n<p>\n\r\n<\/section>\n<h2>How to Use the Calculator<\/h2>\n<ol>\n<li>Enter the <strong>Molality (m)<\/strong> in mol\/kg \u2014 the moles of solute per kilogram of solvent, not per litre of solution. If you only know masses, use a <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/molality-calculator\/\">molality calculator<\/a> first.<\/li>\n<li>Enter the <strong>Boiling Point Elevation Constant (Kb)<\/strong> of the solvent in \u00b0C\u00b7kg\/mol (water: 0.512, ethanol: 1.22, benzene: 2.53, chloroform: 3.63).<\/li>\n<li>Enter the <strong>van 't Hoff Factor (i)<\/strong>: 1 for non-electrolytes like sucrose, about 2 for NaCl, about 3 for CaCl\u2082.<\/li>\n<li>Enter the <strong>Pure Solvent Boiling Point (Tb\u00b0)<\/strong> and choose \u00b0C or \u00b0F from the unit dropdown.<\/li>\n<li>Read the results: the elevation \\(\\Delta T_b\\) in \u00b0C and \u00b0F, and the boiling point of the solution in both units.<\/li>\n<\/ol>\n<h2>What Is Boiling Point Elevation?<\/h2>\n<p>Boiling point elevation is a colligative property: when a non-volatile solute is dissolved in a solvent, the solution boils at a higher temperature than the pure solvent. The effect depends only on the number of dissolved particles, not on what they are. A spoon of salt and a spoon of sugar raise the boiling point of water by the same amount if they produce the same number of particles.<\/p>\n<p>The physical reason is vapour pressure lowering. A solute dilutes the solvent at the surface, reducing how many solvent molecules escape into the vapour phase, so the solution reaches atmospheric pressure \u2014 the boiling condition \u2014 only at a higher temperature. The same principle drives freezing point depression, and both effects can be described through the temperature dependence of vapour pressure, which is the basis of the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/clausius-clapeyron-calculator\/\">Clausius\u2013Clapeyron equation<\/a>.<\/p>\n<p>The van 't Hoff factor accounts for dissociation. Sodium chloride splits into Na\u207a and Cl\u207b ions, so one formula unit gives roughly two particles and \\(i \\approx 2\\). In practice, ion pairing in real solutions makes the effective value slightly smaller: \\(i\\) for NaCl is closer to 1.9, and for CaCl\u2082 closer to 2.6 than the ideal 3. For sugar, ethanol, and other molecular solutes that do not dissociate, \\(i = 1\\) exactly.<\/p>\n<p>The result tells you the new boiling temperature, useful for cooking (salted water boils slightly hotter), for laboratory reflux and distillation set-ups, and for checking solution concentrations: since \\(\\Delta T_b\\) is proportional to molality, a measured elevation can be used backwards to determine the molar mass of an unknown solute.<\/p>\n<h2>Ebullioscopic Constants of Common Solvents<\/h2>\n<table>\n<thead>\n<tr>\n<th>Solvent<\/th>\n<th>\\(K_b\\) (\u00b0C\u00b7kg\/mol)<\/th>\n<th>Normal boiling point (\u00b0C)<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>Water<\/td>\n<td>0.512<\/td>\n<td>100.0<\/td>\n<\/tr>\n<tr>\n<td>Ethanol<\/td>\n<td>1.22<\/td>\n<td>78.4<\/td>\n<\/tr>\n<tr>\n<td>Benzene<\/td>\n<td>2.53<\/td>\n<td>80.1<\/td>\n<\/tr>\n<tr>\n<td>Chloroform<\/td>\n<td>3.63<\/td>\n<td>61.2<\/td>\n<\/tr>\n<tr>\n<td>Carbon tetrachloride<\/td>\n<td>5.03<\/td>\n<td>76.8<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h2>Assumptions and Limitations<\/h2>\n<ul>\n<li><strong>The solute must be non-volatile.<\/strong> Volatile solutes (e.g. ethanol in water) change the vapour pressure in both directions, and the simple formula no longer applies.<\/li>\n<li><strong>The formula is for dilute solutions.<\/strong> At high molality, deviations from ideality grow and \\(K_b\\) is no longer constant; treat results above a few mol\/kg as estimates.<\/li>\n<li><strong>Molality is used, not molarity.<\/strong> Molality does not change with temperature, which is why colligative properties use it. Do not enter a molarity value; if needed, convert via a <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/molarity-calculator\/\">molarity calculator<\/a> and the solution's density.<\/li>\n<li><strong>Use a realistic van 't Hoff factor.<\/strong> Ideal values (2 for NaCl, 3 for CaCl\u2082) overestimate the effect slightly in concentrated solutions. Experimental values are available for common salts.<\/li>\n<li><strong>Pressure matters.<\/strong> The entered pure-solvent boiling point should match your actual pressure. At high altitude, water boils well below 100 \u00b0C, so enter the local value rather than the standard one.<\/li>\n<\/ul>\n<h2>Related Colligative Properties<\/h2>\n<p>Boiling point elevation is one of four colligative properties, together with freezing point depression, vapour pressure lowering, and <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/osmotic-pressure-calculator\/\">osmotic pressure<\/a>. All four scale with the concentration of dissolved particles, so measuring one lets you predict the others.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the boiling point elevation of a solution from molality, the ebullioscopic constant Kb, and the van 't Hoff factor. Enter the pure solvent's boiling point to get the new boiling point in \u00b0C and \u00b0F.<\/p>\n","protected":false},"author":3168,"featured_media":0,"comment_status":"open","ping_status":"","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"footnotes":""},"categories":[54],"tags":[56],"class_list":["post-66492","post","type-post","status-publish","format-standard","hentry","category-chemistry","tag-stoichiometry"],"acf":[],"_links":{"self":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66492","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/users\/3168"}],"replies":[{"embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/comments?post=66492"}],"version-history":[{"count":1,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66492\/revisions"}],"predecessor-version":[{"id":66493,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66492\/revisions\/66493"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66492"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66492"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66492"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}