{"id":234140,"date":"2025-06-13T19:03:01","date_gmt":"2025-06-13T19:03:01","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=234140"},"modified":"2025-06-13T19:03:03","modified_gmt":"2025-06-13T19:03:03","slug":"what-mass-of-sodium-hydrogen-sulphate-nahso4-is-required-to-prepare-200-ml-of-a-0-200-mol-l-solution","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/13\/what-mass-of-sodium-hydrogen-sulphate-nahso4-is-required-to-prepare-200-ml-of-a-0-200-mol-l-solution\/","title":{"rendered":"What mass of sodium hydrogen sulphate (NaHSO4) is required to prepare 200 mL of a 0.200 mol\/L solution"},"content":{"rendered":"\n

What mass of sodium hydrogen sulphate (NaHSO4) is required to prepare 200 mL of a 0.200 mol\/L solution? a) Calculate the moles of sodium hydrogen sulphate present. (n=CV) b) Calculate the mass of sodium hydrogen sulphate present. (m =nM<\/p>\n\n\n\n

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

Step a: Calculate the moles of sodium hydrogen sulfate present using the formula<\/strong><\/h3>\n\n\n\n

n = C \u00d7 V<\/strong><\/p>\n\n\n\n

Where:<\/p>\n\n\n\n

    \n
  • n<\/strong> = number of moles<\/li>\n\n\n\n
  • C<\/strong> = concentration (mol\/L)<\/li>\n\n\n\n
  • V<\/strong> = volume (in liters)<\/li>\n<\/ul>\n\n\n\n

    Given:<\/strong>
    C = 0.200 mol\/L
    V = 200 mL = 0.200 L<\/p>\n\n\n\n

    Substitute into the formula:<\/strong>
    n = 0.200 mol\/L \u00d7 0.200 L = 0.040 mol<\/strong><\/p>\n\n\n\n

    \n\n\n\n

    Step b: Calculate the mass of sodium hydrogen sulfate using the formula<\/strong><\/h3>\n\n\n\n

    m = n \u00d7 M<\/strong><\/p>\n\n\n\n

    Where:<\/p>\n\n\n\n

      \n
    • m<\/strong> = mass (g)<\/li>\n\n\n\n
    • n<\/strong> = number of moles<\/li>\n\n\n\n
    • M<\/strong> = molar mass of NaHSO\u2084<\/li>\n<\/ul>\n\n\n\n

      To calculate the molar mass of NaHSO\u2084:<\/p>\n\n\n\n

        \n
      • Na = 22.99 g\/mol<\/li>\n\n\n\n
      • H = 1.01 g\/mol<\/li>\n\n\n\n
      • S = 32.07 g\/mol<\/li>\n\n\n\n
      • O\u2084 = 16.00 \u00d7 4 = 64.00 g\/mol<\/li>\n<\/ul>\n\n\n\n

        M = 22.99 + 1.01 + 32.07 + 64.00 = 120.07 g\/mol<\/strong><\/p>\n\n\n\n

        Now calculate the mass:
        m = 0.040 mol \u00d7 120.07 g\/mol = 4.80 g<\/strong><\/p>\n\n\n\n

        \n\n\n\n

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

        4.80 grams<\/strong> of sodium hydrogen sulfate (NaHSO\u2084) is required.<\/p>\n\n\n\n

        \n\n\n\n

        \ud83d\udcd8 Explanation (like in textbooks):<\/strong><\/h3>\n\n\n\n

        To prepare a solution of a known concentration, it is essential to determine the exact amount of solute (in this case, NaHSO\u2084) needed. The molarity (mol\/L) expresses how many moles of solute are dissolved in one liter of solution. Since we are preparing only 200 mL (or 0.200 L), we multiply the desired concentration by this volume to find the moles of NaHSO\u2084 required. This gives 0.040 mol.<\/p>\n\n\n\n

        Next, to convert moles into grams\u2014a measurable quantity\u2014we multiply the number of moles by the molar mass of NaHSO\u2084. The molar mass is calculated by summing the atomic masses of each element in the compound. Multiplying 0.040 mol by 120.07 g\/mol gives the required mass as 4.80 grams<\/strong>. This process ensures precision in preparing chemical solutions for laboratory or industrial use.<\/p>\n\n\n\n

        \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

        What mass of sodium hydrogen sulphate (NaHSO4) is required to prepare 200 mL of a 0.200 mol\/L solution? a) Calculate the moles of sodium hydrogen sulphate present. (n=CV) b) Calculate the mass of sodium hydrogen sulphate present. (m =nM The Correct Answer and Explanation is: Step a: Calculate the moles of sodium hydrogen sulfate present […]<\/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-234140","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/234140","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=234140"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/234140\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=234140"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=234140"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=234140"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}