{"id":66488,"date":"2026-10-06T17:30:18","date_gmt":"2026-10-06T14:30:18","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66488"},"modified":"2026-10-06T17:30:18","modified_gmt":"2026-10-06T14:30:18","slug":"freezing-point-depression-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/freezing-point-depression-calculator\/","title":{"rendered":"Freezing Point Depression 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 Freezing Point of a Solution<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66488\" data-favorite-title=\"Freezing Point Depression\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/freezing-point-depression-calculator\/\" data-favorite-excerpt=\"Calculate the freezing point of a solution from molality, the cryoscopic constant (Kf), and the van &#039;t Hoff factor. Enter your values to get the depression \u0394Tf and the new freezing 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\/freezing-point-depression-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66488\" data-post=\"66488\"><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\" min=\"0\" value=\"1\"\/><div class=\"unit\" id=\"calc-unit-1\">mol\/kg<\/div><small id=\"calc-info-1\">Moles of solute per kilogram of solvent (not molarity!)<\/small><\/div><div class=\"field has-term\" id=\"input-2\"><label for=\"field-2\">Freezing Point Depression Constant (Kf)<\/label><div class=\"term\">Kf<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"freezing_point_depression_constant_kf\" id=\"field-2\" aria-describedby=\"calc-unit-2 calc-info-2\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 1.86\" min=\"0.0001\" value=\"1.86\"\/><div class=\"unit\" id=\"calc-unit-2\">\u00b0C\u00b7kg\/mol<\/div><small id=\"calc-info-2\">Cryoscopic constant of the solvent (water: 1.86 \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=\"0.1\" value=\"2\"\/><small id=\"calc-info-3\">Particles formed per formula unit (\u22481 for sugar, \u22482 for NaCl, \u22483 for CaCl\u2082)<\/small><\/div><div class=\"field has-term\" id=\"input-4\"><label for=\"field-4\">Freezing Point of Pure Solvent (Tf\u2070)<\/label><div class=\"term\">Tf\u2070<\/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=\"freezing_point_of_pure_solvent_tf\" id=\"field-4\" aria-describedby=\"calc-info-4\" placeholder=\"e.g. 0\" step=\"0.01\" value=\"0\"\/><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\">Freezing point of the pure solvent (water: 0 \u00b0C \/ 32 \u00b0F)<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66488\">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> Freezing Point Results<\/h3><div class=\"result-box\"><div class=\"field-result\" id=\"output-1\"><span class=\"field-title\"><span>Freezing Point Depression (\u0394Tf)<\/span><span class=\"result-term\">\u0394Tf<\/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>Freezing Point of the Solution<\/span><span class=\"result-term\">Tf<\/span><\/span><span class=\"field-value\" id=\"result-2\" 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-3\"><span class=\"field-title\"><span>Freezing Point of the Solution<\/span><span class=\"result-term\">Tf<\/span><\/span><span class=\"field-value\" id=\"result-3\" 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=\"66488\" 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 cursor-pointer transition-transform hover:scale-105\" data-reaction=\"confused\"><span class=\"reaction-count\" data-reaction-count=\"confused\">0<\/span><span class=\"reaction text-3xl\" aria-hidden=\"true\">\ud83d\ude15 <\/span><span class=\"reaction-description font-medium\">Confused <\/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=\"disappointed\"><span class=\"reaction-count\" data-reaction-count=\"disappointed\">0<\/span><span class=\"reaction text-3xl\" aria-hidden=\"true\">\ud83d\ude1e <\/span><span class=\"reaction-description font-medium\">Disappointed <\/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=\"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>Freezing Point Depression 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_f = i \\cdot K_f \\cdot m \\\\ T_f = T_f^0 - \\Delta T_f \\\\[4pt] T_f = T_f^0 - i \\cdot K_f \\cdot m\n\\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(\\Delta T_f\\) \u2014 freezing point depression, the number of degrees the freezing point drops (\u00b0C)<\/li>\n<li>\\(i\\) \u2014 van 't Hoff factor: particles produced per formula unit of solute (\u22481 for non-electrolytes, \u22482 for NaCl, \u22483 for CaCl\u2082)<\/li>\n<li>\\(K_f\\) \u2014 cryoscopic (freezing point depression) constant of the solvent (\u00b0C\u00b7kg\/mol; water = 1.86)<\/li>\n<li>\\(m\\) \u2014 molality of the solution (mol solute per kg solvent)<\/li>\n<li>\\(T_f^0\\) \u2014 freezing point of the pure solvent (\u00b0C; water = 0 \u00b0C)<\/li>\n<li>\\(T_f\\) \u2014 freezing point of the solution (\u00b0C)<\/li>\n<\/ul>\n<p>The formula expresses a colligative property: the freezing point drops in direct proportion to the concentration of dissolved particles, regardless of their chemical identity.<\/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>Freezing Point Depression \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> table salt (NaCl) is dissolved in water to make a 1 mol\/kg solution. Water has \\(K_f = 1.86\\) \u00b0C\u00b7kg\/mol and freezes at 0 \u00b0C; NaCl dissociates into Na\u207a and Cl\u207b, so \\(i \\approx 2\\).<\/p>\n<p>\\[ \\Delta T_f = i \\cdot K_f \\cdot m = 2 \\times 1.86 \\times 1 = 3.72\\ \\text{\u00b0C} \\\\ T_f = T_f^0 - \\Delta T_f = 0 - 3.72 = -3.72\\ \\text{\u00b0C} \\\\ T_f = -3.72 \\times \\tfrac{9}{5} + 32 = 25.30\\ \\text{\u00b0F}<br \/>\n\\]<\/p>\n<p><strong>Result:<\/strong> the freezing point drops by 3.72 \u00b0C, so the saltwater freezes at \u22123.72 \u00b0C (25.30 \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. This is moles of solute per kilogram of <em>solvent<\/em>, not per litre of solution \u2014 if you only know molarity, convert first (see the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/molality-calculator\/\">molality calculator<\/a>).<\/li>\n<li>Enter the <strong>Freezing Point Depression Constant (Kf)<\/strong> of your solvent in \u00b0C\u00b7kg\/mol. Use 1.86 for water; other common values are listed below.<\/li>\n<li>Enter the <strong>van 't Hoff Factor (i)<\/strong>: about 1 for sugar or ethanol, 2 for NaCl, 3 for CaCl\u2082. Ideal values are only approximations for real salts.<\/li>\n<li>Enter the <strong>Freezing Point of Pure Solvent (Tf\u2070)<\/strong> and choose \u00b0C or \u00b0F from the unit dropdown. Water is 0 \u00b0C (32 \u00b0F).<\/li>\n<li>Read the results: the depression \\(\\Delta T_f\\), the solution's freezing point in \u00b0C, and the same value converted to \u00b0F.<\/li>\n<\/ol>\n<h2>What Is Freezing Point Depression?<\/h2>\n<p>Freezing point depression is a colligative property: when a solute is dissolved in a liquid, the liquid freezes at a lower temperature than the pure solvent. The effect depends only on <em>how many<\/em> dissolved particles are present, not on what they are. A mole of sugar molecules and a mole of alcohol molecules dissolved in the same amount of water lower the freezing point by exactly the same amount.<\/p>\n<p>The reason is thermodynamic. A pure solvent freezes when its solid and liquid phases have equal chemical potential. Dissolved solute lowers the chemical potential of the liquid phase (it increases entropy), but leaves the solid phase \u2014 into which the solute does not fit \u2014 unchanged. The balance is therefore restored at a lower temperature, where the solid is less stable. The same entropy argument explains why dilute solutions boil higher (boiling point elevation) and generate <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/osmotic-pressure-calculator\/\">osmotic pressure<\/a> across a membrane.<\/p>\n<p>For electrolytes, each formula unit breaks into several ions, so the effective particle count is multiplied by the van 't Hoff factor \\(i\\). NaCl ideally gives \\(i = 2\\) (Na\u207a + Cl\u207b) and CaCl\u2082 gives \\(i = 3\\), which is why calcium chloride is a more effective road de-icer per mole than rock salt. In real solutions ion pairing reduces \\(i\\) slightly below the ideal integer, especially at higher concentrations.<\/p>\n<p>Interpreting the result is simple: the calculator returns how many degrees the freezing point drops (\\(\\Delta T_f\\)) and the actual new freezing point. A larger molality, a more dissociated solute, or a solvent with a bigger \\(K_f\\) all push the freezing point further down.<\/p>\n<h2>Cryoscopic Constants of Common Solvents<\/h2>\n<table>\n<thead>\n<tr>\n<th>Solvent<\/th>\n<th>Normal freezing point (\u00b0C)<\/th>\n<th>Kf (\u00b0C\u00b7kg\/mol)<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>Water<\/td>\n<td>0.0<\/td>\n<td>1.86<\/td>\n<\/tr>\n<tr>\n<td>Benzene<\/td>\n<td>5.5<\/td>\n<td>5.12<\/td>\n<\/tr>\n<tr>\n<td>Chloroform<\/td>\n<td>\u221263.5<\/td>\n<td>4.68<\/td>\n<\/tr>\n<tr>\n<td>Acetic acid<\/td>\n<td>16.6<\/td>\n<td>3.90<\/td>\n<\/tr>\n<tr>\n<td>Cyclohexane<\/td>\n<td>6.6<\/td>\n<td>20.0<\/td>\n<\/tr>\n<tr>\n<td>Camphor<\/td>\n<td>179.8<\/td>\n<td>39.7<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h2>Assumptions, Limitations and Practical Tips<\/h2>\n<ul>\n<li><strong>Use molality, not molarity.<\/strong> Colligative formulas require moles per kilogram of solvent, which is temperature-independent. If your concentration is in mol\/L, use the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/molarity-calculator\/\">molarity calculator<\/a> together with the solution's density to convert.<\/li>\n<li><strong>The formula is exact only for dilute solutions.<\/strong> At high concentrations, ion pairing, solute\u2013solvent interactions and non-ideal behaviour make the real freezing point deviate from the prediction.<\/li>\n<li><strong>Real van 't Hoff factors are lower than ideal.<\/strong> Seawater-strength NaCl behaves as if \\(i \\approx 1.8\\)\u20131.9 rather than 2. For precise work, use a measured value.<\/li>\n<li><strong>Check the solubility.<\/strong> The calculation assumes all the solute stays dissolved. If salt precipitates out at low temperature, the molality stops at the saturation limit and the freezing point can't drop further from that solute.<\/li>\n<li><strong>Watch units for non-aqueous solvents.<\/strong> \\(K_f\\) values in tables are almost always in \u00b0C\u00b7kg\/mol and normal freezing points in \u00b0C; enter them in \u00b0C for consistency.<\/li>\n<li><strong>Classic application:<\/strong> this equation is also run backwards to determine molar masses of unknown solutes, and Kf values are themselves measured from known solutions.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the freezing point of a solution from molality, the cryoscopic constant (Kf), and the van 't Hoff factor. Enter your values to get the depression \u0394Tf and the new freezing 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-66488","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\/66488","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=66488"}],"version-history":[{"count":1,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66488\/revisions"}],"predecessor-version":[{"id":66489,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66488\/revisions\/66489"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66488"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66488"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66488"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}