{"id":66502,"date":"2026-10-06T17:36:00","date_gmt":"2026-10-06T14:36:00","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66502"},"modified":"2026-10-06T17:36:00","modified_gmt":"2026-10-06T14:36:00","slug":"precipitation-prediction-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/precipitation-prediction-calculator\/","title":{"rendered":"Precipitation Prediction 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\">Will a Precipitate Form When You Mix These Ions?<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66502\" data-favorite-title=\"Precipitation Prediction\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/precipitation-prediction-calculator\/\" data-favorite-excerpt=\"Enter the cation and anion concentrations, their stoichiometric exponents, and the solubility product Ksp to find out whether a precipitate forms when two solutions are mixed. The calculator compares the ion product Qsp with Ksp and predicts precipitation instantly.\" aria-label=\"Add to Favorites\" data-favorite-icon=\"icon icon-chemistry-1\">\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\/precipitation-prediction-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66502\" data-post=\"66502\"><fieldset class=\"fieldset-input\"><legend class=\"sr-only\">Input Fields<\/legend><div class=\"is-single field\" id=\"input-1\"><span class=\"font-semibold\">Cation M\u207a<\/span><\/div><div class=\"field has-term\" id=\"input-2\"><label for=\"field-2\">Cation Concentration<\/label><div class=\"term\">[M\u207a]<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"cation_concentration\" id=\"field-2\" aria-describedby=\"calc-unit-2 calc-info-2\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 0.01\" min=\"0\" value=\"0.01\"\/><div class=\"unit\" id=\"calc-unit-2\">mol\/L<\/div><small id=\"calc-info-2\">Molar concentration of the positive ion in the mixture (default: Ag\u207a)<\/small><\/div><div class=\"field has-term\" id=\"input-3\"><label for=\"field-3\">Cation Exponent (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=\"cation_exponent_m\" 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 cations in the formula unit, e.g. 2 for Ca\u00b2\u207a in Ca\u2083(PO\u2084)\u2082 it is 3<\/small><\/div><div class=\"is-single field\" id=\"input-4\"><span class=\"font-semibold\">Anion A\u207f\u207b<\/span><\/div><div class=\"field has-term\" id=\"input-5\"><label for=\"field-5\">Anion Concentration<\/label><div class=\"term\">[A\u207f\u207b]<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"anion_concentration\" id=\"field-5\" aria-describedby=\"calc-unit-5 calc-info-5\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 0.01\" min=\"0\" value=\"0.01\"\/><div class=\"unit\" id=\"calc-unit-5\">mol\/L<\/div><small id=\"calc-info-5\">Molar concentration of the negative ion in the mixture (default: Cl\u207b)<\/small><\/div><div class=\"field has-term\" id=\"input-6\"><label for=\"field-6\">Anion Exponent (n)<\/label><div class=\"term\">n<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"anion_exponent_n\" id=\"field-6\" aria-describedby=\"calc-info-6\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 1\" min=\"1\" value=\"1\"\/><small id=\"calc-info-6\">Number of anions in the formula unit, e.g. 2 for Cl\u207b in MgCl\u2082 or PbCl\u2082<\/small><\/div><div class=\"is-single field\" id=\"input-7\"><span class=\"font-semibold\">Solubility Product<\/span><\/div><div class=\"field has-term\" id=\"input-8\"><label for=\"field-8\">Solubility Product (Ksp)<\/label><div class=\"term\">Ksp<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"solubility_product_ksp\" id=\"field-8\" aria-describedby=\"calc-info-8\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 1.8e-5\" min=\"0\" value=\"1.8E-5\"\/><small id=\"calc-info-8\">Solubility product of the salt at 25 \u00b0C \u2014 scientific notation like 1.8e-5 is accepted (default: AgCl)<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66502\">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> Precipitation Prediction Results<\/h3><div class=\"result-box\"><div class=\"field-result\" id=\"output-1\"><span class=\"field-title\"><span>Ion Product<\/span><span class=\"result-term\">Qsp<\/span><\/span><span class=\"field-value\" id=\"result-1\"><\/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>Saturation Ratio<\/span><span class=\"result-term\">Qsp\/Ksp<\/span><\/span><span class=\"field-value\" id=\"result-2\"><\/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 is-column\" id=\"output-3\"><span class=\"field-title\"><span>Prediction<\/span><\/span><span class=\"field-value\" id=\"result-3\"><\/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 is-column\" id=\"output-4\"><span class=\"field-title\"><span>Calculation Details<\/span><\/span><span class=\"field-value\" id=\"result-4\"><\/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=\"66502\" 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>Precipitation Prediction<\/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\\[ Q_{sp} = [M^{+}]^{m} \\cdot [A^{n-}]^{n} \\]\n\\[ \\text{If } Q_{sp} &gt; K_{sp} \\text{ a precipitate forms; if } Q_{sp} &lt; K_{sp} \\text{ it does not.} \\]<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(Q_{sp}\\) \u2014 ion product of the salt in the mixture (mol\/L raised to the power \\(m+n\\))<\/li>\n<li>\\([M^{+}]\\) \u2014 molar concentration of the cation after mixing (mol\/L)<\/li>\n<li>\\([A^{n-}]\\) \u2014 molar concentration of the anion after mixing (mol\/L)<\/li>\n<li>\\(m\\) \u2014 number of cations in one formula unit of the salt<\/li>\n<li>\\(n\\) \u2014 number of anions in one formula unit of the salt<\/li>\n<li>\\(K_{sp}\\) \u2014 solubility product of the salt at 25 \u00b0C<\/li>\n<\/ul>\n<p>The ion product has the same mathematical form as the solubility product, but it is built from the concentrations actually present in the mixture. Comparing \\(Q_{sp}\\) with \\(K_{sp}\\) tells you whether the solution is unsaturated, exactly saturated, or supersaturated.<\/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>Precipitation Prediction \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> equal volumes of 0.020 M AgNO\u2083 and 0.020 M NaCl are mixed, so after dilution each ion is at 0.010 mol\/L. Does AgCl precipitate? Use \\(m = n = 1\\) and \\(K_{sp} = 1.8 \\times 10^{-5}\\) for AgCl.<\/p>\n<p>\\[ Q_{sp} = [Ag^{+}]^{1}[Cl^{-}]^{1} = (0.010)(0.010) = 1.0 \\times 10^{-4} \\]<\/p>\n<p>\\[ \\frac{Q_{sp}}{K_{sp}} = \\frac{1.0 \\times 10^{-4}}{1.8 \\times 10^{-5}} \\approx 5.56 \\]<\/p>\n<p><strong>Result:<\/strong> \\(Q_{sp} &gt; K_{sp}\\), so the solution is supersaturated and <strong>AgCl precipitates<\/strong>. Roughly 57.6% of both ions must leave the solution as solid AgCl before equilibrium is restored.<\/p>\n<p>\n\r\n<\/section>\n<h2>How to Use the Precipitation Prediction Calculator<\/h2>\n<ol>\n<li>Enter the <strong>Cation Concentration<\/strong> in mol\/L. This must be the concentration <em>after<\/em> mixing, not the concentration in the original solution.<\/li>\n<li>Set the <strong>Cation Exponent (m)<\/strong> \u2014 the number of cations in the salt's formula unit (e.g. 3 for Ca\u2083(PO\u2084)\u2082).<\/li>\n<li>Enter the <strong>Anion Concentration<\/strong> in mol\/L, again using the post-mixing value.<\/li>\n<li>Set the <strong>Anion Exponent (n)<\/strong> \u2014 the number of anions in the formula unit (e.g. 2 for PbCl\u2082).<\/li>\n<li>Enter the <strong>Solubility Product (Ksp)<\/strong> of the salt at 25 \u00b0C. Scientific notation such as <code>1.8e-5<\/code> is accepted.<\/li>\n<li>Read the results: the <strong>Ion Product<\/strong>, the <strong>Saturation Ratio<\/strong> \\(Q_{sp}\/K_{sp}\\), the <strong>Prediction<\/strong>, and the <strong>Calculation Details<\/strong> showing the full comparison.<\/li>\n<\/ol>\n<h2>What Is the Ion Product and Why Compare It with Ksp?<\/h2>\n<p>The solubility product \\(K_{sp}\\) is the equilibrium constant for a slightly soluble salt dissolving in water. For a salt \\(M_mA_n\\), it equals the product of the equilibrium ion concentrations, each raised to its stoichiometric power. At 25 \u00b0C, AgCl has \\(K_{sp} = 1.8 \\times 10^{-5}\\), which corresponds to a molar solubility of about \\(1.3 \\times 10^{-5}\\) mol\/L in pure water.<\/p>\n<p>When two soluble solutions are mixed, the ions may or may not exceed this equilibrium limit. The ion product \\(Q_{sp}\\) is computed from the concentrations actually present. It works like a reaction quotient: comparing it with \\(K_{sp}\\) reveals which way the dissolution equilibrium must shift.<\/p>\n<p>The interpretation follows three simple rules:<\/p>\n<ul>\n<li><strong>\\(Q_{sp} &lt; K_{sp}\\)<\/strong> \u2014 unsaturated: no precipitate forms, and any added solid would keep dissolving.<\/li>\n<li><strong>\\(Q_{sp} = K_{sp}\\)<\/strong> \u2014 exactly saturated: the system is at equilibrium, with no net change.<\/li>\n<li><strong>\\(Q_{sp} &gt; K_{sp}\\)<\/strong> \u2014 supersaturated: a precipitate forms, removing ions from solution until \\(Q_{sp}\\) falls back to \\(K_{sp}\\).<\/li>\n<\/ul>\n<p>The saturation ratio \\(Q_{sp}\/K_{sp}\\) adds a sense of scale. A ratio of 5.56 means the ion product is more than five times the equilibrium value, so precipitation is essentially certain and substantial. A ratio of 1.02 predicts precipitation too, but only a tiny amount of solid will form before equilibrium is reached.<\/p>\n<h2>Assumptions, Limitations and Practical Tips<\/h2>\n<p><strong>Use post-mixing concentrations.<\/strong> The most common mistake is entering the concentrations of the original solutions. When you mix \\(V_1\\) and \\(V_2\\) of two solutions, each concentration is diluted by the total volume: \\(C_{\\text{mixed}} = C_{\\text{initial}} \\cdot V_1\/(V_1 + V_2)\\). In the example above, mixing equal volumes halves each 0.020 M solution to 0.010 M. Our <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/molarity-calculator\/\">Molarity Calculator<\/a> can help you convert between concentration units first.<\/p>\n<p><strong>Ksp values are temperature-dependent.<\/strong> Tabulated values are normally quoted at 25 \u00b0C. At other temperatures the solubility product changes, and the prediction may shift \u2014 most salts become more soluble as temperature rises.<\/p>\n<p><strong>Concentrations approximate activities.<\/strong> In dilute solutions molar concentrations and thermodynamic activities are nearly equal, but in ionic media above roughly 0.1 mol\/L the effective \\(K_{sp}\\) appears larger because of ionic interactions. For such solutions, check the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/ionic-strength-calculator\/\">Ionic Strength Calculator<\/a> to see whether activity corrections matter for your case.<\/p>\n<p><strong>Side reactions are ignored.<\/strong> The calculator assumes both ions remain free in solution. Complex formation (e.g. Ag\u207a binding to NH\u2083), acid\u2013base reactions of the anion (e.g. CO\u2083\u00b2\u207b partially converting to HCO\u2083\u207b), or redox processes can change the free ion concentrations and alter the outcome. For acid\u2013base effects on weak-acid anions, the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/ph-calculator\/\">pH Calculator<\/a> is a useful companion.<\/p>\n<p><strong>Kinetics are not predicted.<\/strong> The calculator tells you whether precipitation is thermodynamically favored, not how fast it happens. Some supersaturated solutions (especially with sparingly soluble carbonates and sulfates) can persist for minutes or longer before visible crystals appear.<\/p>\n<p>To explore the reverse question \u2014 how much of a salt dissolves before the solution saturates \u2014 the same \\(K_{sp}\\) comparison applies, and the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/equilibrium-constant-calculator\/\">Equilibrium Constant Calculator<\/a> covers the broader family of equilibrium problems.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Enter the cation and anion concentrations, their stoichiometric exponents, and the solubility product Ksp to find out whether a precipitate forms when two solutions are mixed. The calculator compares the ion product Qsp with Ksp and predicts precipitation instantly.<\/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":[57],"class_list":["post-66502","post","type-post","status-publish","format-standard","hentry","category-chemistry","tag-reactions"],"acf":[],"_links":{"self":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66502","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=66502"}],"version-history":[{"count":1,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66502\/revisions"}],"predecessor-version":[{"id":66503,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66502\/revisions\/66503"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66502"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66502"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66502"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}