{"id":207872,"date":"2025-04-25T13:42:18","date_gmt":"2025-04-25T13:42:18","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=207872"},"modified":"2025-04-25T13:42:20","modified_gmt":"2025-04-25T13:42:20","slug":"what-is-the-molarity-of-10-5-kg-of-na2so4%c2%b710h2o-in-18-60-l-of-solution","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/04\/25\/what-is-the-molarity-of-10-5-kg-of-na2so4%c2%b710h2o-in-18-60-l-of-solution\/","title":{"rendered":"what is the molarity of 10.5 kg of Na2SO4\u00b710H2O in 18.60 L of solution"},"content":{"rendered":"\n<p>what is the molarity of 10.5 kg of Na2SO4\u00b710H2O in 18.60 L of solution<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>To calculate the molarity of a solution, we need to know the amount of solute in moles and the volume of the solution in liters. In this case, the solute is sodium sulfate decahydrate (Na\u2082SO\u2084\u00b710H\u2082O), and we are given its mass (10.5 kg) and the volume of the solution (18.60 L).<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Find the molar mass of Na\u2082SO\u2084\u00b710H\u2082O<\/h3>\n\n\n\n<p>The formula Na\u2082SO\u2084\u00b710H\u2082O represents sodium sulfate (Na\u2082SO\u2084) combined with 10 water molecules. To find its molar mass, we sum the atomic masses of all elements in the formula:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sodium (Na): 22.99 g\/mol (there are 2 Na atoms)<\/li>\n\n\n\n<li>Sulfur (S): 32.07 g\/mol (1 S atom)<\/li>\n\n\n\n<li>Oxygen (O): 16.00 g\/mol (4 O atoms in Na\u2082SO\u2084 and 10 O atoms in H\u2082O)<\/li>\n\n\n\n<li>Hydrogen (H): 1.008 g\/mol (20 H atoms in 10H\u2082O)<\/li>\n<\/ul>\n\n\n\n<p>Now calculate the molar mass:<\/p>\n\n\n\n<p>[<br>\\text{Molar mass of Na\u2082SO\u2084\u00b710H\u2082O} = (2 \\times 22.99) + 32.07 + (4 \\times 16.00) + (20 \\times 1.008)<br>]<br>[<br>= 45.98 + 32.07 + 64.00 + 20.16 = 162.21 \\, \\text{g\/mol}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Convert the mass of Na\u2082SO\u2084\u00b710H\u2082O to moles<\/h3>\n\n\n\n<p>We are given 10.5 kg of Na\u2082SO\u2084\u00b710H\u2082O. First, convert the mass to grams:<\/p>\n\n\n\n<p>[<br>10.5 \\, \\text{kg} = 10,500 \\, \\text{g}<br>]<\/p>\n\n\n\n<p>Now, use the molar mass to find the number of moles:<\/p>\n\n\n\n<p>[<br>\\text{Moles of Na\u2082SO\u2084\u00b710H\u2082O} = \\frac{\\text{Mass}}{\\text{Molar mass}} = \\frac{10,500 \\, \\text{g}}{162.21 \\, \\text{g\/mol}} = 64.74 \\, \\text{mol}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Calculate the molarity<\/h3>\n\n\n\n<p>Molarity (M) is calculated as the number of moles of solute per liter of solution:<\/p>\n\n\n\n<p>[<br>\\text{Molarity} = \\frac{\\text{Moles of solute}}{\\text{Volume of solution in liters}} = \\frac{64.74 \\, \\text{mol}}{18.60 \\, \\text{L}} = 3.48 \\, \\text{M}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Conclusion:<\/h3>\n\n\n\n<p>The molarity of the Na\u2082SO\u2084\u00b710H\u2082O solution is <strong>3.48 M<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>what is the molarity of 10.5 kg of Na2SO4\u00b710H2O in 18.60 L of solution The correct answer and explanation is : To calculate the molarity of a solution, we need to know the amount of solute in moles and the volume of the solution in liters. In this case, the solute is sodium sulfate decahydrate [&hellip;]<\/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-207872","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/207872","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=207872"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/207872\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=207872"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=207872"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=207872"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}