{"id":205533,"date":"2025-03-25T05:09:36","date_gmt":"2025-03-25T05:09:36","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=205533"},"modified":"2025-03-25T05:09:39","modified_gmt":"2025-03-25T05:09:39","slug":"a-solution-contains-6-00-by-mass-or-mass-mass-nabr-sodium-bromide-molar-mass-102-89-g-mol","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/25\/a-solution-contains-6-00-by-mass-or-mass-mass-nabr-sodium-bromide-molar-mass-102-89-g-mol\/","title":{"rendered":"A solution contains 6.00% (by mass) or (mass\/mass) NaBr (sodium bromide) (molar mass = 102.89 g\/mol)"},"content":{"rendered":"\n<p>A solution contains 6.00% (by mass) or (mass\/mass) NaBr (sodium bromide) (molar mass = 102.89 g\/mol). The density of the solution is 1.046 g\/cm. What is the molarity of the NaBr solution?<\/p>\n\n\n\n<p>a. 0.610<br>b. 0.305<br>c. 0.583<br>d. 0.280<br>e. 0.105<\/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 determine the molarity of the NaBr solution, we follow these steps:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Step 1: Define Given Information<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Mass percent of NaBr<\/strong> = 6.00% (which means 6.00 g NaBr in 100 g of solution)<\/li>\n\n\n\n<li><strong>Density of solution<\/strong> = 1.046 g\/cm\u00b3<\/li>\n\n\n\n<li><strong>Molar mass of NaBr<\/strong> = 102.89 g\/mol<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Step 2: Convert Mass of Solution to Volume<\/strong><\/h3>\n\n\n\n<p>We assume 100 g of solution. Using density:<\/p>\n\n\n\n<p>[<br>\\text{Volume} = \\frac{\\text{Mass}}{\\text{Density}} = \\frac{100 \\text{ g}}{1.046 \\text{ g\/cm}^3}<br>]<\/p>\n\n\n\n<p>[<br>= 95.60 \\text{ cm}^3 = 95.60 \\text{ mL} = 0.09560 \\text{ L}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Step 3: Calculate Moles of NaBr<\/strong><\/h3>\n\n\n\n<p>Since 6.00 g of NaBr is present in 100 g of solution:<\/p>\n\n\n\n<p>[<br>\\text{Moles of NaBr} = \\frac{6.00 \\text{ g}}{102.89 \\text{ g\/mol}}<br>]<\/p>\n\n\n\n<p>[<br>= 0.0583 \\text{ moles}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Step 4: Calculate Molarity<\/strong><\/h3>\n\n\n\n<p>Molarity (M) is defined as:<\/p>\n\n\n\n<p>[<br>M = \\frac{\\text{moles of solute}}{\\text{liters of solution}}<br>]<\/p>\n\n\n\n<p>[<br>M = \\frac{0.0583}{0.09560}<br>]<\/p>\n\n\n\n<p>[<br>= 0.610 \\text{ M}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Final Answer:<\/strong><\/h3>\n\n\n\n<p>[<br>\\mathbf{0.610 \\text{ M} \\Rightarrow \\text{Option (a)}}<br>]<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Explanation<\/strong><\/h3>\n\n\n\n<p>Molarity is the number of moles of solute per liter of solution. We calculated the moles of NaBr from the given mass and molar mass. Then, using density, we found the volume of the solution. Finally, dividing moles by volume gave the correct molarity.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/03\/image-1336.png\" alt=\"\" class=\"wp-image-205534\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>A solution contains 6.00% (by mass) or (mass\/mass) NaBr (sodium bromide) (molar mass = 102.89 g\/mol). The density of the solution is 1.046 g\/cm. What is the molarity of the NaBr solution? a. 0.610b. 0.305c. 0.583d. 0.280e. 0.105 The correct answer and explanation is : To determine the molarity of the NaBr solution, we follow [&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-205533","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/205533","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=205533"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/205533\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=205533"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=205533"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=205533"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}