{"id":66867,"date":"2026-10-13T10:00:47","date_gmt":"2026-10-13T07:00:47","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66867"},"modified":"2026-10-13T12:04:33","modified_gmt":"2026-10-13T09:04:33","slug":"solubility-product-ksp-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/solubility-product-ksp-calculator\/","title":{"rendered":"Solubility Product (Ksp) 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 Ksp from Molar Solubility<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66867\" data-favorite-title=\"Solubility Product\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/solubility-product-ksp-calculator\/\" data-favorite-excerpt=\"Calculate the solubility product (Ksp) of a sparingly soluble salt from its molar solubility. Enter the solubility, its unit, and the cation and anion coefficients from the formula AaBb.\" 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\/solubility-product-ksp-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66867\" data-post=\"66867\"><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\">Molar Solubility (s)<\/label><div class=\"term\">s<\/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=\"text\" name=\"molar_solubility_s\" id=\"field-1\" aria-describedby=\"calc-info-1\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 0.00021\" min=\"0\" value=\"0.00021\"\/><div class=\"grid grid-cols-1\"><select id=\"field-2\" name=\"unit\" aria-label=\"Unit\"><option value=\"molL\" selected>mol\/L<\/option><option value=\"mmolL\">mmol\/L<\/option><option value=\"gL\">g\/L<\/option><option value=\"mgL\">mg\/L<\/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-1\">Solubility of the salt in pure water at equilibrium. If you only know it in g\/L or mg\/L, pick that unit and enter the molar mass below.<\/small><\/div><div class=\"field has-term\" id=\"input-2\" hidden><label for=\"field-3\">Molar Mass of the Salt (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=\"molar_mass_of_the_salt_m\" id=\"field-3\" aria-describedby=\"calc-unit-3 calc-info-3\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 78.07\" min=\"0\" value=\"78.07\"\/><div class=\"unit\" id=\"calc-unit-3\">g\/mol<\/div><small id=\"calc-info-3\">Needed only when the solubility is given in g\/L or mg\/L, to convert it to mol\/L (e.g. CaF\u2082 = 78.07 g\/mol).<\/small><\/div><div class=\"field has-term\" id=\"input-3\"><label for=\"field-4\">Cation Coefficient (a)<\/label><div class=\"term\">a<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"cation_coefficient_a\" id=\"field-4\" aria-describedby=\"calc-info-4\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 1\" min=\"1\" max=\"12\" value=\"1\"\/><small id=\"calc-info-4\">Number of cations in one formula unit (e.g. 1 for Ca\u00b2\u207a in CaF\u2082, 2 for Ag\u207a in Ag\u2082CrO\u2084).<\/small><\/div><div class=\"field has-term\" id=\"input-4\"><label for=\"field-5\">Anion Coefficient (b)<\/label><div class=\"term\">b<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"anion_coefficient_b\" id=\"field-5\" aria-describedby=\"calc-info-5\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 2\" min=\"1\" max=\"12\" value=\"2\"\/><small id=\"calc-info-5\">Number of anions in one formula unit (e.g. 2 for F\u207b in CaF\u2082, 1 for CrO\u2084\u00b2\u207b in Ag\u2082CrO\u2084).<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66867\">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> Solubility Product Results<\/h3><div class=\"result-box\"><div class=\"field-result\" id=\"output-1\"><span class=\"field-title\"><span>Solubility Product<\/span><span class=\"result-term\">Ksp<\/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>Cation Concentration at Equilibrium<\/span><\/span><span class=\"field-value\" id=\"result-2\" data-unit=\"mol\/L\"><\/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>Anion Concentration at Equilibrium<\/span><\/span><span class=\"field-value\" id=\"result-3\" data-unit=\"mol\/L\"><\/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 class=\"field-result is-column\" id=\"output-5\"><span class=\"field-title\"><span>Common Ksp Values (25 \u00b0C)<\/span><\/span><span class=\"field-value\" id=\"result-5\"><\/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=\"66867\" 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>Solubility Product<\/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\\[ K_{sp} = [A]^a[B]^b = (a\\,s)^a\\,(b\\,s)^b = a^a \\cdot b^b \\cdot s^{\\,a+b} \\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(s\\) \u2014 molar solubility of the salt in pure water (mol\/L)<\/li>\n<li>\\(a\\) \u2014 number of cations released by one formula unit<\/li>\n<li>\\(b\\) \u2014 number of anions released by one formula unit<\/li>\n<li>\\([A]\\), \\([B]\\) \u2014 equilibrium ion concentrations (mol\/L)<\/li>\n<\/ul>\n<p>For a salt \\(A_aB_b\\) that dissolves as \\(A_aB_b(s) \\rightleftharpoons aA^{}+bB\\), each dissolved formula unit releases \\(a\\) cations and \\(b\\) anions, so \\([A] = a\\,s\\) and \\([B] = b\\,s\\). Substituting these into the equilibrium expression gives \\(K_{sp}\\) directly from the molar solubility.<\/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>Solubility Product \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> calcium fluoride, CaF\\(_2\\), has a molar solubility of \\(2.1\\times10^{-4}\\) mol\/L in pure water at 25 \\(^\\circ\\)C. Each formula unit releases one Ca\\(^{2+}\\) and two F\\(^{-}\\), so \\(a = 1\\) and \\(b = 2\\).<\/p>\n<p>\\[ [\\mathrm{Ca^{2+}}] = s = 2.1\\times10^{-4}\\ \\mathrm{mol\/L}, \\quad [\\mathrm{F^-}] = 2s = 4.2\\times10^{-4}\\ \\mathrm{mol\/L} \\]<\/p>\n<p>\\[ K_{sp} = [\\mathrm{Ca^{2+}}][\\mathrm{F^-}]^2 = (s)(2s)^2 = 4s^3 = 4\\,(2.1\\times10^{-4})^3 \\]<\/p>\n<p><strong>Result:<\/strong> \\(K_{sp} \\approx 3.7\\times10^{-11}\\), which matches the tabulated literature value of \\(3.9\\times10^{-11}\\) for CaF\\(_2\\) at 25 \\(^\\circ\\)C.<\/p>\n<p>\n\r\n<\/section>\n<h2>How to Use the Calculator<\/h2>\n<ol>\n<li>Enter the solubility of the salt in the <strong>Molar Solubility (s)<\/strong> field and choose its unit (mol\/L, mmol\/L, g\/L, or mg\/L) from the dropdown.<\/li>\n<li>If you selected g\/L or mg\/L, the <strong>Molar Mass of the Salt (M)<\/strong> field appears \u2014 enter the salt's molar mass in g\/mol so the value can be converted to mol\/L. If you're not sure, you can find it with the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/percent-composition-from-chemical-formula-calculator\/\">percent composition from chemical formula calculator<\/a>.<\/li>\n<li>Set the <strong>Cation Coefficient (a)<\/strong> to the number of cations in one formula unit (1 for Ca\\(^{2+}\\) in CaF\\(_2\\), 2 for Ag\\(^+\\) in Ag\\(_2\\)CrO\\(_4\\)).<\/li>\n<li>Set the <strong>Anion Coefficient (b)<\/strong> to the number of anions in one formula unit (2 for F\\(^{-\\) in CaF\\(_2\\), 1 for CrO\\(_4^{2-}\\)).<\/li>\n<li>Read the <strong>Solubility Product<\/strong>, the equilibrium cation and anion concentrations, the full calculation details, and a table of common literature \\(K_{sp}\\) values for comparison.<\/li>\n<\/ol>\n<h2>What Is the Solubility Product?<\/h2>\n<p>The solubility product, \\(K_{sp}\\), is the equilibrium constant for the dissolution of a sparingly soluble ionic solid in water. When a salt such as AgCl or CaF\\(_2\\) is added to water, it dissolves until the solution is saturated: the solid and its dissolved ions are then in dynamic equilibrium. Unlike soluble salts, these compounds dissolve only to a very small extent, and \\(K_{sp}\\) quantifies exactly how small that extent is.<\/p>\n<p>\\(K_{sp}\\) depends only on temperature (typically tabulated at 25 \\(^\\circ\\)C) and on the identity of the salt \u2014 not on how much solid is present, as long as some undissolved solid remains. A smaller \\(K_{sp}\\) means a less soluble salt. For example, AgBr (\\(K_{sp} = 5.4\\times10^{-13}\\)) is far less soluble than CaSO\\(_4\\) (\\(K_{sp} = 2.4\\times10^{-5}\\)).<\/p>\n<p>An important subtlety is the stoichiometry. You cannot compare \\(K_{sp}\\) values directly across salts with different ion ratios: for CaF\\(_2\\), \\(K_{sp} = 4s^3\\), while for AgCl, \\(K_{sp} = s^2\\). The relationship between \\(K_{sp}\\) and molar solubility always passes through the coefficients \\(a\\) and \\(b\\), which is why the calculator asks for them.<\/p>\n<p>\\(K_{sp}\\) is also the basis for predicting whether a precipitate will form when two solutions are mixed \u2014 compare the ion product with \\(K_{sp}\\) using the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/precipitation-prediction-calculator\/\">precipitation prediction calculator<\/a>. The same equilibrium governs the common-ion effect, qualitative analysis separations, and the behavior of scale-forming minerals measured by the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/water-hardness-calculator\/\">water hardness calculator<\/a>.<\/p>\n<h2>Assumptions, Limitations and Practical Tips<\/h2>\n<ul>\n<li><strong>Pure water, no other ion sources.<\/strong> The formula assumes the dissolving salt is the only source of both ions. If the solution already contains a common ion (e.g. F\\(^{-\\) from NaF), the solubility drops and the calculated \\(K_{sp}\\) from simple \\(s\\) no longer applies.<\/li>\n<li><strong>No side reactions.<\/strong> Ions that hydrolyze, complex, or react with water (carbonates, sulfides, salts of weak acids or bases) have apparent solubilities that differ from the simple \\(K_{sp}\\) model. Mg(OH)\\(_2\\), for instance, is affected by the pH-dependent OH\\(^{-\\) concentration.<\/li>\n<li><strong>Concentrations approximate activities.<\/strong> Strictly, \\(K_{sp}\\) is written in terms of ion activities. For dilute saturated solutions of sparingly soluble salts this approximation is excellent, which is why the calculator rejects solubilities above roughly 0.1 mol\/L.<\/li>\n<li><strong>Temperature matters.<\/strong> All results assume 25 \\(^\\circ\\)C. Solubility usually increases with temperature for endothermic dissolution, so \\(K_{sp}\\) changes accordingly \u2014 see the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/van-t-hoff-equation-calculator\/\">Van 't Hoff equation calculator<\/a> for the temperature dependence of equilibrium constants.<\/li>\n<li><strong>Check against literature values.<\/strong> Comparing your result with the reference table shown in the output is a quick sanity check; small deviations reflect rounding in the solubility data and ionic-strength effects.<\/li>\n<\/ul>\n<h2>Common Ksp Values at 25 \\(^\\circ\\)C<\/h2>\n<table>\n<thead>\n<tr>\n<th>Salt<\/th>\n<th>Dissolution equilibrium<\/th>\n<th>\\(K_{sp}\\)<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>AgCl<\/td>\n<td>\\(\\mathrm{AgCl \\rightleftharpoons Ag^+ + Cl^-}\\)<\/td>\n<td>\\(1.8\\times10^{-10}\\)<\/td>\n<\/tr>\n<tr>\n<td>AgBr<\/td>\n<td>\\(\\mathrm{AgBr \\rightleftharpoons Ag^+ + Br^-}\\)<\/td>\n<td>\\(5.4\\times10^{-13}\\)<\/td>\n<\/tr>\n<tr>\n<td>Ag\\(_2\\)CrO\\(_4\\)<\/td>\n<td>\\(\\mathrm{Ag_2CrO_4 \\rightleftharpoons 2Ag^+ + CrO_4^{2-}}\\)<\/td>\n<td>\\(1.1\\times10^{-12}\\)<\/td>\n<\/tr>\n<tr>\n<td>BaSO\\(_4\\)<\/td>\n<td>\\(\\mathrm{BaSO_4 \\rightleftharpoons Ba^{2+} + SO_4^{2-}}\\)<\/td>\n<td>\\(1.1\\times10^{-10}\\)<\/td>\n<\/tr>\n<tr>\n<td>CaCO\\(_3\\) (calcite)<\/td>\n<td>\\(\\mathrm{CaCO_3 \\rightleftharpoons Ca^{2+} + CO_3^{2-}}\\)<\/td>\n<td>\\(3.3\\times10^{-9}\\)<\/td>\n<\/tr>\n<tr>\n<td>CaF\\(_2\\)<\/td>\n<td>\\(\\mathrm{CaF_2 \\rightleftharpoons Ca^{2+} + 2F^-}\\)<\/td>\n<td>\\(3.9\\times10^{-11}\\)<\/td>\n<\/tr>\n<tr>\n<td>CaSO\\(_4\\)<\/td>\n<td>\\(\\mathrm{CaSO_4 \\rightleftharpoons Ca^{2+} + SO_4^{2-}}\\)<\/td>\n<td>\\(2.4\\times10^{-5}\\)<\/td>\n<\/tr>\n<tr>\n<td>Mg(OH)\\(_2\\)<\/td>\n<td>\\(\\mathrm{Mg(OH)_2 \\rightleftharpoons Mg^{2+} + 2OH^-}\\)<\/td>\n<td>\\(5.6\\times10^{-12}\\)<\/td>\n<\/tr>\n<tr>\n<td>PbI\\(_2\\)<\/td>\n<td>\\(\\mathrm{PbI_2 \\rightleftharpoons Pb^{2+} + 2I^-}\\)<\/td>\n<td>\\(7.1\\times10^{-9}\\)<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>These values are useful for verifying a calculation: entering the literature solubility of any of these salts with the correct coefficients should reproduce the tabulated \\(K_{sp}\\) to within rounding error.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the solubility product (Ksp) of a sparingly soluble salt from its molar solubility. Enter the solubility, its unit, and the cation and anion coefficients from the formula AaBb.<\/p>\n","protected":false},"author":3168,"featured_media":0,"comment_status":"open","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"footnotes":""},"categories":[54],"tags":[57],"class_list":["post-66867","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\/66867","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=66867"}],"version-history":[{"count":1,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66867\/revisions"}],"predecessor-version":[{"id":66868,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66867\/revisions\/66868"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66867"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66867"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66867"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}