{"id":187591,"date":"2025-02-05T06:40:10","date_gmt":"2025-02-05T06:40:10","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=187591"},"modified":"2025-02-05T06:40:11","modified_gmt":"2025-02-05T06:40:11","slug":"rank-the-following-solutions-from-lowest-to-highest-ph","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/05\/rank-the-following-solutions-from-lowest-to-highest-ph\/","title":{"rendered":"Rank The Following Solutions From Lowest To Highest PH"},"content":{"rendered":"\n

Rank The Following Solutions From Lowest To Highest PH. A) 0.10 M HC4H7O2 (Ka = 1.5 \u00d7 10\u22125) B) 0.50 M HCN (Ka = 4.9 \u00d7 10\u221210)<\/p>\n\n\n\n

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

Ranking the Solutions from Lowest to Highest pH<\/strong><\/h3>\n\n\n\n

We are given two weak acid solutions with their respective concentrations and acid dissociation constants (( K_a )):<\/p>\n\n\n\n

    \n
  • A) 0.10 M HC\u2084H\u2087O\u2082<\/strong> (Ka = ( 1.5 \\times 10^{-5} ))<\/li>\n\n\n\n
  • B) 0.50 M HCN<\/strong> (Ka = ( 4.9 \\times 10^{-10} ))<\/li>\n<\/ul>\n\n\n\n

    To determine their pH values, we need to calculate the hydrogen ion concentration ([H^+]) for each solution using the weak acid dissociation formula:<\/p>\n\n\n\n

    [
    [H^+] = \\sqrt{K_a \\times C_a}
    ]<\/p>\n\n\n\n

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

      \n
    • ( K_a ) = acid dissociation constant<\/li>\n\n\n\n
    • ( C_a ) = initial concentration of the acid<\/li>\n<\/ul>\n\n\n\n

      Step 1: Calculate [H\u207a] for HC\u2084H\u2087O\u2082<\/strong><\/h4>\n\n\n\n

      [
      [H^+] = \\sqrt{(1.5 \\times 10^{-5}) \\times (0.10)}
      ]
      [
      [H^+] = \\sqrt{1.5 \\times 10^{-6}}
      ]
      [
      [H^+] \\approx 1.22 \\times 10^{-3} \\text{ M}
      ]
      [
      \\text{pH} = -\\log(1.22 \\times 10^{-3}) \\approx 2.91
      ]<\/p>\n\n\n\n

      Step 2: Calculate [H\u207a] for HCN<\/strong><\/h4>\n\n\n\n

      [
      [H^+] = \\sqrt{(4.9 \\times 10^{-10}) \\times (0.50)}
      ]
      [
      [H^+] = \\sqrt{2.45 \\times 10^{-10}}
      ]
      [
      [H^+] \\approx 1.57 \\times 10^{-5} \\text{ M}
      ]
      [
      \\text{pH} = -\\log(1.57 \\times 10^{-5}) \\approx 4.80
      ]<\/p>\n\n\n\n

      Final Ranking (Lowest to Highest pH)<\/strong><\/h3>\n\n\n\n
        \n
      1. 0.10 M HC\u2084H\u2087O\u2082 (pH \u2248 2.91)<\/strong><\/li>\n\n\n\n
      2. 0.50 M HCN (pH \u2248 4.80)<\/strong><\/li>\n<\/ol>\n\n\n\n

        Explanation<\/strong><\/h3>\n\n\n\n
          \n
        • The pH of a weak acid is determined by both its ( K_a ) value and its concentration.<\/li>\n\n\n\n
        • HC\u2084H\u2087O\u2082 has a larger ( K_a ) (( 1.5 \\times 10^{-5} )), meaning it ionizes more than HCN, leading to a lower pH.<\/li>\n\n\n\n
        • HCN has a much smaller ( K_a ) (( 4.9 \\times 10^{-10} )), meaning it ionizes very little, resulting in a higher pH.<\/li>\n\n\n\n
        • Since lower pH means more acidic, HC\u2084H\u2087O\u2082 is the more acidic solution<\/strong> compared to HCN.<\/li>\n<\/ul>\n\n\n\n

          Thus, HC\u2084H\u2087O\u2082 has the lowest pH, followed by HCN with a higher pH<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"

          Rank The Following Solutions From Lowest To Highest PH. A) 0.10 M HC4H7O2 (Ka = 1.5 \u00d7 10\u22125) B) 0.50 M HCN (Ka = 4.9 \u00d7 10\u221210) The Correct Answer and Explanation is : Ranking the Solutions from Lowest to Highest pH We are given two weak acid solutions with their respective concentrations and 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-187591","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187591","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=187591"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187591\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187591"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187591"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187591"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}