{"id":194424,"date":"2025-02-24T05:57:05","date_gmt":"2025-02-24T05:57:05","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=194424"},"modified":"2025-02-24T05:57:07","modified_gmt":"2025-02-24T05:57:07","slug":"what-is-the-percent-ionization-of-a-monoprotic-weak-acid-solution-that-is-0-154-m","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/24\/what-is-the-percent-ionization-of-a-monoprotic-weak-acid-solution-that-is-0-154-m\/","title":{"rendered":"What is the percent ionization of a monoprotic weak acid solution that is 0.154 M"},"content":{"rendered":"\n

Chemistry What is the percent ionization of a monoprotic weak acid solution that is 0.154 M? The acid-dissociation (or ionization) constant, Ka, of this acid is 4.92\u00d710-10 percent ionization:<\/p>\n\n\n\n

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

The percent ionization of the monoprotic weak acid solution is 0.00565%<\/strong>.<\/p>\n\n\n\n

Explanation:<\/h3>\n\n\n\n

The percent ionization of a weak acid refers to the fraction of the acid molecules that ionize in solution. It is calculated using the formula:<\/p>\n\n\n\n

[
\\% \\text{Ionization} = \\left(\\frac{[\\text{H}^+]}{C} \\right) \\times 100
]<\/p>\n\n\n\n

where:<\/p>\n\n\n\n

    \n
  • ([\\text{H}^+]) is the concentration of hydrogen ions at equilibrium.<\/li>\n\n\n\n
  • (C) is the initial concentration of the acid.<\/li>\n<\/ul>\n\n\n\n

    For a weak acid, the equilibrium concentration of (\\text{H}^+) is approximated using:<\/p>\n\n\n\n

    [
    [\\text{H}^+] \\approx \\sqrt{K_a \\times C}
    ]<\/p>\n\n\n\n

    Substituting the given values:<\/p>\n\n\n\n

      \n
    • (K_a = 4.92 \\times 10^{-10})<\/li>\n\n\n\n
    • (C = 0.154)<\/li>\n<\/ul>\n\n\n\n

      [
      [\\text{H}^+] = \\sqrt{(4.92 \\times 10^{-10}) \\times (0.154)}
      ]<\/p>\n\n\n\n

      [
      [\\text{H}^+] \\approx 9.29 \\times 10^{-6} \\text{ M}
      ]<\/p>\n\n\n\n

      Now, calculating the percent ionization:<\/p>\n\n\n\n

      [
      \\% \\text{Ionization} = \\left(\\frac{9.29 \\times 10^{-6}}{0.154} \\right) \\times 100
      ]<\/p>\n\n\n\n

      [
      \\% \\text{Ionization} \\approx 0.00565\\%
      ]<\/p>\n\n\n\n

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

      Since the acid is weak, only a very small fraction of its molecules ionize in solution. The extremely low (K_a) value confirms that the acid is only minimally ionized, leading to a percent ionization of 0.00565%<\/strong>. This shows that in a relatively concentrated solution, weak acids ionize even less compared to more diluted solutions.<\/p>\n\n\n\n

      Here is a scientific illustration of a weak acid solution undergoing ionization, showing partial dissociation into H\u207a and A\u207b ions with equilibrium notations. Let me know if you need any modifications or further explanations!<\/p>\n\n\n\n

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

      Chemistry What is the percent ionization of a monoprotic weak acid solution that is 0.154 M? The acid-dissociation (or ionization) constant, Ka, of this acid is 4.92\u00d710-10 percent ionization: The Correct Answer and Explanation is : The percent ionization of the monoprotic weak acid solution is 0.00565%. Explanation: The percent ionization of a weak acid […]<\/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-194424","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194424","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=194424"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194424\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=194424"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=194424"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=194424"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}