{"id":201257,"date":"2025-03-15T07:01:15","date_gmt":"2025-03-15T07:01:15","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=201257"},"modified":"2025-03-15T07:01:18","modified_gmt":"2025-03-15T07:01:18","slug":"50-0-g-of-methanol-ch3oh-molecular-mass-32-04-g-mol-is-dissolved-to-make-500-0-ml-of-solution","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/15\/50-0-g-of-methanol-ch3oh-molecular-mass-32-04-g-mol-is-dissolved-to-make-500-0-ml-of-solution\/","title":{"rendered":"50.0 g of methanol (CH3OH, molecular mass = 32.04 g\/mol) is dissolved to make 500.0 mL of solution"},"content":{"rendered":"\n

50.0 g of methanol (CH3OH, molecular mass = 32.04 g\/mol) is dissolved to make 500.0 mL of solution. What is the molarity, mol\/L, of the resulting solution?<\/p>\n\n\n\n

Would that be?<\/p>\n\n\n\n

32.04\/.50 = 64.08<\/p>\n\n\n\n

The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n

To calculate the molarity (M) of a solution, the formula is:<\/p>\n\n\n\n

[
\\text{Molarity (M)} = \\frac{\\text{moles of solute}}{\\text{volume of solution in liters}}
]<\/p>\n\n\n\n

Step-by-Step Calculation<\/h3>\n\n\n\n
    \n
  1. Determine the moles of methanol (CH\u2083OH):<\/strong>
    The number of moles is calculated by dividing the mass of the solute by its molar mass. Given:<\/li>\n<\/ol>\n\n\n\n
      \n
    • Mass of methanol = 50.0 g<\/li>\n\n\n\n
    • Molar mass of methanol (CH\u2083OH) = 32.04 g\/mol [
      \\text{Moles of methanol} = \\frac{\\text{Mass of methanol}}{\\text{Molar mass of methanol}} = \\frac{50.0 \\, \\text{g}}{32.04 \\, \\text{g\/mol}} = 1.561 \\, \\text{mol}
      ]<\/li>\n<\/ul>\n\n\n\n
        \n
      1. Convert the volume of the solution to liters:<\/strong>
        The volume of the solution is given as 500.0 mL. To use it in the molarity formula, we need to convert it to liters: [
        \\text{Volume in liters} = \\frac{500.0 \\, \\text{mL}}{1000} = 0.5000 \\, \\text{L}
        ]<\/li>\n\n\n\n
      2. Calculate the molarity:<\/strong>
        Now that we have the number of moles of solute and the volume of the solution in liters, we can substitute these values into the molarity formula: [
        M = \\frac{\\text{moles of solute}}{\\text{volume of solution in liters}} = \\frac{1.561 \\, \\text{mol}}{0.5000 \\, \\text{L}} = 3.122 \\, \\text{M}
        ]<\/li>\n<\/ol>\n\n\n\n

        Thus, the molarity of the methanol solution is 3.12 M<\/strong>.<\/p>\n\n\n\n

        Explanation of the Steps:<\/h3>\n\n\n\n

        To understand this, let\u2019s break it down:<\/p>\n\n\n\n

          \n
        • Moles of Solute<\/strong>: The number of moles of methanol is found by dividing the mass of the methanol (50.0 g) by its molar mass (32.04 g\/mol). This step gives us how many individual molecules of methanol are present in the solution.<\/li>\n\n\n\n
        • Volume of Solution<\/strong>: The volume is given as 500.0 mL, which is converted into liters (since molarity uses liters).<\/li>\n\n\n\n
        • Molarity Calculation<\/strong>: Molarity represents the concentration of a solution, specifically the number of moles of solute per liter of solution. By dividing the number of moles by the volume of the solution, we find the molarity.<\/li>\n<\/ul>\n\n\n\n

          Thus, the correct answer is 3.12 M<\/strong>, not 64.08. Your formula of 32.04\/.50 = 64.08<\/strong> is incorrect because it doesn’t take into account the number of moles or the correct application of the molarity formula.<\/p>\n","protected":false},"excerpt":{"rendered":"

          50.0 g of methanol (CH3OH, molecular mass = 32.04 g\/mol) is dissolved to make 500.0 mL of solution. What is the molarity, mol\/L, of the resulting solution? Would that be? 32.04\/.50 = 64.08 The correct answer and explanation is : To calculate the molarity (M) of a solution, the formula is: [\\text{Molarity (M)} = \\frac{\\text{moles […]<\/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-201257","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/201257","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=201257"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/201257\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=201257"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=201257"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=201257"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}