Calcium carbonate, CaCO3, has a solubility in water of 0.0180 g\/l at 25 C. Calculate the solubility product (Ksp) for CaCO3<\/p>\n\n\n\n
The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n To calculate the solubility product constant (Ksp)<\/strong> for calcium carbonate (CaCO\u2083)<\/strong>, follow these steps:<\/p>\n\n\n\n When calcium carbonate dissolves in water, it dissociates as:<\/p>\n\n\n\n [ From this equation, 1 mole of CaCO\u2083 produces 1 mole of Ca\u00b2\u207a and 1 mole of CO\u2083\u00b2\u207b<\/strong>.<\/p>\n\n\n\n The given solubility of CaCO\u2083 is 0.0180 g\/L<\/strong> at 25\u00b0C<\/strong>. To find the molar solubility, divide by its molar mass<\/strong>:<\/p>\n\n\n\n [ [ Since CaCO\u2083 dissociates in a 1:1 ratio<\/strong>, the equilibrium concentrations of ions are:<\/p>\n\n\n\n [ The solubility product expression for CaCO\u2083<\/strong> is:<\/p>\n\n\n\n [ Substituting the values:<\/p>\n\n\n\n [ [ [ The solubility product constant (Ksp<\/strong>) is a measure of the extent to which a sparingly soluble compound dissolves in water. In this case, CaCO\u2083<\/strong> dissociates into calcium ions (Ca\u00b2\u207a<\/strong>) and carbonate ions (CO\u2083\u00b2\u207b<\/strong>) in a 1:1 ratio<\/strong>.<\/p>\n\n\n\n We first determined the molar solubility<\/strong> of calcium carbonate by converting the given solubility in grams per liter to moles per liter using the molar mass. The calculated molar solubility<\/strong> was 1.80 \u00d7 10\u207b\u2074 M<\/strong>, which represents the concentration of both Ca\u00b2\u207a and CO\u2083\u00b2\u207b<\/strong> in solution.<\/p>\n\n\n\n Using the solubility product expression Ksp = [Ca\u00b2\u207a][CO\u2083\u00b2\u207b]<\/strong>, we substituted the molar solubility values into the equation. Since both ion concentrations are equal, we squared the molar solubility to obtain Ksp = 3.24 \u00d7 10\u207b\u2078<\/strong>.<\/p>\n\n\n\n This Ksp value<\/strong> is a fundamental property of CaCO\u2083<\/strong> and is useful for predicting precipitation reactions. For example, if the product of Ca\u00b2\u207a and CO\u2083\u00b2\u207b<\/strong> concentrations in a solution exceeds Ksp<\/strong>, precipitation will occur. Conversely, if the product is below Ksp<\/strong>, more CaCO\u2083<\/strong> can dissolve.<\/p>\n\n\n\n In practical applications, this principle is crucial in geology (limestone dissolution), water treatment (scale formation), and biology (bone formation and shell formation in marine organisms)<\/strong>. Additionally, changes in pH<\/strong> affect carbonate solubility since CO\u2083\u00b2\u207b<\/strong> reacts with H\u207a to form bicarbonate (HCO\u2083\u207b<\/strong>), increasing CaCO\u2083 solubility<\/strong> in acidic conditions.<\/p>\n\n\n\n Thus, the solubility product constant quantifies the limited solubility of CaCO\u2083<\/strong> and helps in predicting its behavior in different chemical and environmental conditions.<\/p>\n","protected":false},"excerpt":{"rendered":" Calcium carbonate, CaCO3, has a solubility in water of 0.0180 g\/l at 25 C. Calculate the solubility product (Ksp) for CaCO3 The correct answer and explanation is : To calculate the solubility product constant (Ksp) for calcium carbonate (CaCO\u2083), follow these steps: Step 1: Write the Dissociation Equation When calcium carbonate dissolves in water, it […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-201050","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/201050","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=201050"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/201050\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=201050"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=201050"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=201050"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 1: Write the Dissociation Equation<\/strong><\/h3>\n\n\n\n
CaCO_3 (s) \\rightleftharpoons Ca^{2+} (aq) + CO_3^{2-} (aq)
]<\/p>\n\n\n\nStep 2: Convert Solubility to Molarity<\/strong><\/h3>\n\n\n\n
\\text{Molar Mass of CaCO\u2083} = 40.08 + 12.01 + (3 \\times 16.00) = 100.09 \\, g\/mol
]<\/p>\n\n\n\n
\\text{Molar Solubility} = \\frac{0.0180 \\, g\/L}{100.09 \\, g\/mol} = 1.80 \\times 10^{-4} \\, M
]<\/p>\n\n\n\n
[Ca^{2+}] = 1.80 \\times 10^{-4} \\, M
]
[
[CO_3^{2-}] = 1.80 \\times 10^{-4} \\, M
]<\/p>\n\n\n\nStep 3: Calculate Ksp<\/strong><\/h3>\n\n\n\n
K_{sp} = [Ca^{2+}][CO_3^{2-}]
]<\/p>\n\n\n\n
K_{sp} = (1.80 \\times 10^{-4}) \\times (1.80 \\times 10^{-4})
]<\/p>\n\n\n\n
K_{sp} = 3.24 \\times 10^{-8}
]<\/p>\n\n\n\nFinal Answer:<\/strong><\/h3>\n\n\n\n
K_{sp} = 3.24 \\times 10^{-8}
]<\/p>\n\n\n\nExplanation (300 Words)<\/strong><\/h3>\n\n\n\n