{"id":185207,"date":"2025-01-22T08:17:13","date_gmt":"2025-01-22T08:17:13","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=185207"},"modified":"2025-01-22T08:17:15","modified_gmt":"2025-01-22T08:17:15","slug":"hydrobromic-acid-molar-mass-80-9-g-mol-is-commercially-available-in-a-34","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/22\/hydrobromic-acid-molar-mass-80-9-g-mol-is-commercially-available-in-a-34\/","title":{"rendered":"Hydrobromic Acid (Molar Mass = 80.9 G\/Mol) Is Commercially Available In A 34"},"content":{"rendered":"\n
    \n
  1. Hydrobromic Acid (Molar Mass = 80.9 G\/Mol) Is Commercially Available In A 34.0 Mass Percent Solution Which Has A Density Of 1.31 G\/Cm\u00b2. What Is The Molarity Of The Commercially Available Hydrobromic Acid?<\/li>\n<\/ol>\n\n\n\n

    The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n

    To determine the molarity of the commercially available hydrobromic acid (HBr), we use the formula: Molarity (M)=moles of solutevolume of solution in liters\\text{Molarity (M)} = \\frac{\\text{moles of solute}}{\\text{volume of solution in liters}}<\/p>\n\n\n\n

    Step 1: Calculate the mass of HBr in 1 liter of solution<\/h3>\n\n\n\n

    The density of the solution is 1.31 g\/cm\u00b3, equivalent to 1.31 g\/mL.
    Since 1 liter = 1000 mL: Mass of solution in 1 liter=1.31\u2009g\/mL\u00d71000\u2009mL=1310\u2009g\\text{Mass of solution in 1 liter} = 1.31 \\, \\text{g\/mL} \\times 1000 \\, \\text{mL} = 1310 \\, \\text{g}<\/p>\n\n\n\n

    The solution is 34.0% HBr by mass, meaning 34.0 g of HBr are present in 100 g of solution. Mass of HBr in 1 liter of solution=34.0100\u00d71310=445.4\u2009g\\text{Mass of HBr in 1 liter of solution} = \\frac{34.0}{100} \\times 1310 = 445.4 \\, \\text{g}<\/p>\n\n\n\n

    Step 2: Convert the mass of HBr to moles<\/h3>\n\n\n\n

    The molar mass of HBr is 80.9 g\/mol. Moles of HBr=Mass of HBrMolar mass=445.480.9=5.51\u2009moles\\text{Moles of HBr} = \\frac{\\text{Mass of HBr}}{\\text{Molar mass}} = \\frac{445.4}{80.9} = 5.51 \\, \\text{moles}<\/p>\n\n\n\n

    Step 3: Calculate molarity<\/h3>\n\n\n\n

    The volume of solution is 1 liter. Thus: Molarity (M)=Moles of HBrVolume of solution in liters=5.511=5.51\u2009M\\text{Molarity (M)} = \\frac{\\text{Moles of HBr}}{\\text{Volume of solution in liters}} = \\frac{5.51}{1} = 5.51 \\, \\text{M}<\/p>\n\n\n\n

    Final Answer:<\/h3>\n\n\n\n

    The molarity of the commercially available hydrobromic acid is 5.51 M<\/strong>.<\/p>\n\n\n\n

    \n\n\n\n

    Explanation:<\/h3>\n\n\n\n
      \n
    1. Density and Percent Composition<\/strong>: The density allows us to calculate the mass of the solution per unit volume, while the percent composition gives the proportion of HBr in the solution.<\/li>\n\n\n\n
    2. Moles of Solute<\/strong>: Using the molar mass, we convert the mass of HBr to moles.<\/li>\n\n\n\n
    3. Molarity<\/strong>: Dividing the moles of HBr by the volume of the solution gives the molarity. This step links the amount of solute to its concentration in the solution.<\/li>\n<\/ol>\n","protected":false},"excerpt":{"rendered":"

      The Correct Answer and Explanation is : To determine the molarity of the commercially available hydrobromic acid (HBr), we use the formula: Molarity (M)=moles of solutevolume of solution in liters\\text{Molarity (M)} = \\frac{\\text{moles of solute}}{\\text{volume of solution in liters}} Step 1: Calculate the mass of HBr in 1 liter of solution The density of the solution is 1.31 g\/cm\u00b3, equivalent to 1.31 […]<\/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-185207","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185207","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=185207"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185207\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=185207"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=185207"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=185207"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}