{"id":185612,"date":"2025-01-22T18:31:27","date_gmt":"2025-01-22T18:31:27","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=185612"},"modified":"2025-01-22T18:31:28","modified_gmt":"2025-01-22T18:31:28","slug":"how-many-grams-of-lithium-nitrate-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/22\/how-many-grams-of-lithium-nitrate-2\/","title":{"rendered":"How many grams of lithium nitrate"},"content":{"rendered":"\n<p>How many grams of lithium nitrate, LiNO3 (68.9 g\/mol) are required to prepare 219.5 mL of a 0.357 M LiNO3 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 number of grams of lithium nitrate (LiNO\u2083) required to prepare 219.5 mL of a 0.357 M LiNO\u2083 solution, follow these steps:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Determine the number of moles required.<\/h3>\n\n\n\n<p>The molarity (M) of a solution is defined as the number of moles of solute per liter of solution. So, the number of moles of lithium nitrate required can be calculated by the formula:<\/p>\n\n\n\n<p>[<br>\\text{moles of LiNO\u2083} = Molarity \\times Volume \\, (\\text{in liters})<br>]<\/p>\n\n\n\n<p>Given:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Molarity (M) = 0.357 M<\/li>\n\n\n\n<li>Volume (V) = 219.5 mL = 0.2195 L (since 1 L = 1000 mL)<\/li>\n<\/ul>\n\n\n\n<p>[<br>\\text{moles of LiNO\u2083} = 0.357 \\, \\text{M} \\times 0.2195 \\, \\text{L} = 0.0784 \\, \\text{moles}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Convert moles of LiNO\u2083 to grams.<\/h3>\n\n\n\n<p>To find the mass of lithium nitrate required, use the molar mass of LiNO\u2083. The molar mass of LiNO\u2083 is given as 68.9 g\/mol.<\/p>\n\n\n\n<p>[<br>\\text{mass of LiNO\u2083} = \\text{moles of LiNO\u2083} \\times \\text{molar mass of LiNO\u2083}<br>]<\/p>\n\n\n\n<p>[<br>\\text{mass of LiNO\u2083} = 0.0784 \\, \\text{moles} \\times 68.9 \\, \\text{g\/mol} = 5.41 \\, \\text{g}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Final Answer:<\/h3>\n\n\n\n<p>To prepare 219.5 mL of a 0.357 M LiNO\u2083 solution, <strong>5.41 grams<\/strong> of lithium nitrate are required.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>Molarity (M) provides the relationship between the volume and the number of moles of solute in a solution. By converting the volume of the solution to liters and using the given molarity, we can find the number of moles of LiNO\u2083 needed. Then, by using the molar mass of LiNO\u2083 (68.9 g\/mol), we convert the moles into grams, which tells us the exact mass of lithium nitrate required to make the solution.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>How many grams of lithium nitrate, LiNO3 (68.9 g\/mol) are required to prepare 219.5 mL of a 0.357 M LiNO3 solution? The Correct Answer and Explanation is : To calculate the number of grams of lithium nitrate (LiNO\u2083) required to prepare 219.5 mL of a 0.357 M LiNO\u2083 solution, follow these steps: Step 1: Determine [&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-185612","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185612","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=185612"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185612\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=185612"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=185612"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=185612"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}