{"id":209006,"date":"2025-04-28T09:21:01","date_gmt":"2025-04-28T09:21:01","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=209006"},"modified":"2025-04-28T09:21:05","modified_gmt":"2025-04-28T09:21:05","slug":"15-ml-of-0-1m-naoh-was-used-to-titrate-30-ml-of-hi-solution-until-the-end-point-was-reached","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/04\/28\/15-ml-of-0-1m-naoh-was-used-to-titrate-30-ml-of-hi-solution-until-the-end-point-was-reached\/","title":{"rendered":"15 mL of 0.1M NaOH was used to titrate 30 ml of HI solution until the end point was reached"},"content":{"rendered":"\n

15 mL of 0.1M NaOH was used to titrate 30 ml of HI solution until the end point was reached. What is the concentration of the HI?<\/p>\n\n\n\n

A 0.10 M<\/p>\n\n\n\n

B 0.05 M
C 0.40 M
D 0.20 M<\/p>\n\n\n\n

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

To find the concentration of HI (hydroiodic acid) in this titration, we can use the concept of moles<\/strong> and stoichiometry<\/strong>. Here’s the step-by-step breakdown:<\/p>\n\n\n\n

Given:<\/h3>\n\n\n\n
    \n
  • Volume of NaOH<\/strong> = 15 mL = 0.015 L<\/li>\n\n\n\n
  • Concentration of NaOH<\/strong> = 0.1 M<\/li>\n\n\n\n
  • Volume of HI<\/strong> = 30 mL = 0.030 L<\/li>\n\n\n\n
  • Titration reaction<\/strong>: The balanced chemical equation for the titration of NaOH with HI is: [
    NaOH + HI \\rightarrow NaI + H_2O
    ]<\/li>\n<\/ul>\n\n\n\n

    This shows that NaOH reacts with HI in a 1:1 molar ratio. So, for every mole of NaOH, one mole of HI reacts.<\/p>\n\n\n\n

    Step 1: Calculate the moles of NaOH used<\/h3>\n\n\n\n

    The number of moles of NaOH can be calculated using the formula:<\/p>\n\n\n\n

    [
    \\text{moles of NaOH} = M \\times V
    ]<\/p>\n\n\n\n

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

      \n
    • ( M = 0.1 \\, \\text{M} ) (molarity of NaOH)<\/li>\n\n\n\n
    • ( V = 0.015 \\, \\text{L} ) (volume of NaOH in liters)<\/li>\n<\/ul>\n\n\n\n

      [
      \\text{moles of NaOH} = 0.1 \\, \\text{M} \\times 0.015 \\, \\text{L} = 0.0015 \\, \\text{moles of NaOH}
      ]<\/p>\n\n\n\n

      Step 2: Use the stoichiometry of the reaction<\/h3>\n\n\n\n

      From the balanced equation, we know that the mole ratio of NaOH to HI is 1:1. This means that the moles of HI that reacted are also 0.0015 moles.<\/p>\n\n\n\n

      Step 3: Calculate the concentration of HI<\/h3>\n\n\n\n

      Now, we can calculate the concentration of HI using the formula:<\/p>\n\n\n\n

      [
      \\text{molarity of HI} = \\frac{\\text{moles of HI}}{\\text{volume of HI in liters}}
      ]<\/p>\n\n\n\n

      [
      \\text{molarity of HI} = \\frac{0.0015 \\, \\text{moles}}{0.030 \\, \\text{L}} = 0.05 \\, \\text{M}
      ]<\/p>\n\n\n\n

      Conclusion:<\/h3>\n\n\n\n

      The concentration of HI is 0.05 M<\/strong>, so the correct answer is:<\/p>\n\n\n\n

      B) 0.05 M<\/strong>.<\/p>\n\n\n\n

      This calculation assumes complete neutralization, as indicated by the fact that the titration reached the endpoint, meaning all the HI has reacted with NaOH.<\/p>\n\n\n\n

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

        15 mL of 0.1M NaOH was used to titrate 30 ml of HI solution until the end point was reached. What is the concentration of the HI? A 0.10 M B 0.05 MC 0.40 MD 0.20 M The correct answer and explanation is : To find the concentration of HI (hydroiodic acid) in this titration, […]<\/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-209006","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/209006","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=209006"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/209006\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=209006"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=209006"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=209006"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}