{"id":6081,"date":"2020-10-13T14:12:37","date_gmt":"2020-10-13T08:42:37","guid":{"rendered":"http:\/\/astan.lk\/al_virtualclassroom\/?p=6081"},"modified":"2020-10-13T14:12:33","modified_gmt":"2020-10-13T08:42:33","slug":"solubility-product","status":"publish","type":"post","link":"https:\/\/astan.lk\/al_virtualclassroom\/solubility-product\/","title":{"rendered":"Solubility product"},"content":{"rendered":"<p>\u2022 The solubility of NaCl in water is approximately 5 mol dm<sup>-3<\/sup>. In the solution there are interactions between Na<sup>+<\/sup> and Cl<sup>&#8211;<\/sup> ions. Though simple, they are not independent of one another.<\/p>\n<p>\u2022 In the case of a sparingly soluble electrolyte such as BaSO<sub>4<\/sub>, the ions exist independently in the solution and the following dynamic equilibrium exists between the solid and the ions in a saturated solution.<\/p>\n<p><img decoding=\"async\" src=\"http:\/\/www.chemguide.co.uk\/physical\/ksp\/baso4eqm.gif\" \/><\/p>\n<p>Applying the law of equilibrium<\/p>\n<p>[BaSO<sub>4<\/sub>(s)] is a constant. Therefore,<\/p>\n<p><img decoding=\"async\" src=\"http:\/\/www.chemguide.co.uk\/physical\/ksp\/ksp2baso4.gif\" \/><\/p>\n<p>\u2022 Ksp is a constant at constant temperature and is called &#8216;solubility product&#8217;. If the solubility of BaSO<sub>4<\/sub> is x mol dm<sup>-3<\/sup>, Ksp = x<sup>2<\/sup> mol<sup>2<\/sup> dm<sup>-6<\/sup>.<\/p>\n<p>\u2022 In general, solubility product is not applied for salts having high solubility.<\/p>\n<p>\u2022 If the ionic product is greater than the solubility product of a salt, it will precipitate.<br \/>\neg. If [Ba<sup>2+<\/sup>][SO<sub>4<\/sub><sup>2-<\/sup>] &gt; Ksp \u00a0 BaSO<sub>4<\/sub> will precipitate.<\/p>\n<p>&nbsp;<\/p>\n<p><strong>Example<\/strong><\/p>\n<p>The solubility of magnesium hydroxide at 298 K is 1.71 x 10<sup>-4<\/sup>mol dm<sup>-3<\/sup>. Calculate the solubility product.<\/p>\n<p>The equilibrium is:<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" src=\"http:\/\/www.chemguide.co.uk\/physical\/ksp\/padding.gif\" width=\"40\" height=\"15\" \/><img loading=\"lazy\" decoding=\"async\" src=\"http:\/\/www.chemguide.co.uk\/physical\/ksp\/kspcalc2a.gif\" width=\"278\" height=\"18\" \/><\/p>\n<p>For every mole of magnesium hydroxide that dissolves, you will get one mole of magnesium ions, but twice that number of hydroxide ions.<\/p>\n<p>So the concentration of the dissolved magnesium ions is the same as the dissolved magnesium hydroxide:<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" src=\"http:\/\/www.chemguide.co.uk\/physical\/ksp\/padding.gif\" width=\"40\" height=\"15\" \/><b>[Mg<sup>2+<\/sup>] = 1.71 x 10<sup>-4<\/sup> mol dm<sup>-3<\/sup><\/b><\/p>\n<p>The concentration of dissolved hydroxide ions is twice that:<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" src=\"http:\/\/www.chemguide.co.uk\/physical\/ksp\/padding.gif\" width=\"40\" height=\"15\" \/><b>[OH<sup>&#8211;<\/sup>] = 2 x 1.71 x 10<sup>-4<\/sup> = 3.42 x 10<sup>-4<\/sup> mol dm<sup>-3<\/sup><\/b><\/p>\n<p>Now put these numbers into the solubility product expression and do the sum.<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" src=\"http:\/\/www.chemguide.co.uk\/physical\/ksp\/padding.gif\" width=\"40\" height=\"15\" \/><img loading=\"lazy\" decoding=\"async\" src=\"http:\/\/www.chemguide.co.uk\/physical\/ksp\/kspcalc2b.gif\" width=\"263\" height=\"78\" \/><\/p>\n<p>&nbsp;<\/p>\n<h4>Common ion effect<\/h4>\n<p>\u2022 On addition of NaCl solution to a saturated solution of AgCl, concentration of Cl<sup>&#8211;<\/sup> ions increases. Since Ksp is a constant at constant temperature Ag<sup>+<\/sup> concentration in the medium should decrease. Therefore, AgCl is precipitated. In other words, the solubility of AgCl in a solution ofup&gt; ions is less compared to its solubility in pure water. This is called common ion effect. This principle is applicable for the Ag<sup>+<\/sup> ion as well.<\/p>\n<p>&nbsp;<\/p>\n","protected":false},"excerpt":{"rendered":"<p>\u2022 The solubility of NaCl in water is approximately 5 mol dm-3. In the solution there are interactions between Na+ and Cl&#8211; ions. Though simple, they are not independent of one another. \u2022 In the case of a sparingly soluble electrolyte such as BaSO4, the ions exist independently in the solution and the following dynamic [&hellip;]<\/p>\n","protected":false},"author":842,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"_monsterinsights_skip_tracking":false,"_monsterinsights_sitenote_active":false,"_monsterinsights_sitenote_note":"","_monsterinsights_sitenote_category":0,"footnotes":""},"categories":[14,1676],"tags":[],"class_list":["post-6081","post","type-post","status-publish","format-standard","hentry","category-chemistry","category-unit-13"],"acf":[],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v26.9 - https:\/\/yoast.com\/product\/yoast-seo-wordpress\/ -->\n<title>Solubility product - Learning &amp; Education Portal<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/astan.lk\/al_virtualclassroom\/solubility-product\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Solubility product - Learning &amp; Education Portal\" \/>\n<meta property=\"og:description\" content=\"\u2022 The solubility of NaCl in water is approximately 5 mol dm-3. 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