{"id":239664,"date":"2025-07-03T04:09:56","date_gmt":"2025-07-03T04:09:56","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=239664"},"modified":"2025-07-03T04:09:58","modified_gmt":"2025-07-03T04:09:58","slug":"calculate-the-ph-of-solution-containing-0-06-m-nh4cl-ka-5-7-x-10-10-and-0-11-m-nh3","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/03\/calculate-the-ph-of-solution-containing-0-06-m-nh4cl-ka-5-7-x-10-10-and-0-11-m-nh3\/","title":{"rendered":"Calculate the pH of solution containing 0.06 M NH4Cl (Ka = 5.7 x 10-10) and 0.11 M NH3"},"content":{"rendered":"\n

Calculate the pH of solution containing 0.06 M NH4Cl (Ka = 5.7 x 10-10) and 0.11 M NH3.<\/p>\n\n\n\n

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

To calculate the pH of a solution containing NH\u2084Cl (ammonium chloride) and NH\u2083 (ammonia), we can use the Henderson-Hasselbalch equation<\/strong> for buffer systems: pH=pKa+log\u2061([Base][Acid])\\text{pH} = \\text{pKa} + \\log \\left( \\frac{[\\text{Base}]}{[\\text{Acid}]} \\right)<\/p>\n\n\n\n

Step-by-step solution:<\/h3>\n\n\n\n
    \n
  1. Identify the Acid and Base:<\/strong>\n
      \n
    • NH\u2084Cl is the acid<\/strong>, as it dissociates into NH\u2084\u207a (ammonium ion) in water. NH\u2084\u207a acts as a weak acid.<\/li>\n\n\n\n
    • NH\u2083 is the base<\/strong>, as it accepts a proton (H\u207a) to form NH\u2084\u207a.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
    • Calculate pKa:<\/strong>\n
        \n
      • The given Ka for NH\u2084\u207a is 5.7\u00d710\u2212105.7 \\times 10^{-10}. The pKa can be found using the formula: pKa=\u2212log\u2061(Ka)\\text{pKa} = -\\log(\\text{Ka}) pKa=\u2212log\u2061(5.7\u00d710\u221210)\u22489.24\\text{pKa} = -\\log(5.7 \\times 10^{-10}) \\approx 9.24<\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • Apply the Henderson-Hasselbalch equation:<\/strong>
        • The concentration of the base (NH\u2083) is 0.11 M, and the concentration of the acid (NH\u2084\u207a from NH\u2084Cl) is 0.06 M.<\/li><\/ul>pH=9.24+log\u2061(0.110.06)\\text{pH} = 9.24 + \\log \\left( \\frac{0.11}{0.06} \\right)\n
            \n
          • Calculate the ratio: 0.110.06=1.833\\frac{0.11}{0.06} = 1.833<\/li>\n\n\n\n
          • Now find the logarithm: log\u2061(1.833)\u22480.263\\log(1.833) \\approx 0.263<\/li>\n\n\n\n
          • So, the pH is: pH=9.24+0.263=9.50\\text{pH} = 9.24 + 0.263 = 9.50<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n

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

            The pH of the solution is approximately 9.50<\/strong>.<\/p>\n\n\n\n

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

            This solution acts as a buffer system, where the weak acid (NH\u2084\u207a) and its conjugate base (NH\u2083) resist large changes in pH. The Henderson-Hasselbalch equation<\/strong> is used to find the pH based on the concentrations of the acid and the base. Since NH\u2084Cl is a weak acid and NH\u2083 is a weak base, their concentrations determine the solution’s ability to maintain a stable pH. The pKa value reflects the strength of NH\u2084\u207a as an acid, and the ratio of the base (NH\u2083) to the acid (NH\u2084\u207a) gives the pH.<\/p>\n","protected":false},"excerpt":{"rendered":"

            Calculate the pH of solution containing 0.06 M NH4Cl (Ka = 5.7 x 10-10) and 0.11 M NH3. The correct answer and explanation is: To calculate the pH of a solution containing NH\u2084Cl (ammonium chloride) and NH\u2083 (ammonia), we can use the Henderson-Hasselbalch equation for buffer systems: pH=pKa+log\u2061([Base][Acid])\\text{pH} = \\text{pKa} + \\log \\left( \\frac{[\\text{Base}]}{[\\text{Acid}]} \\right) […]<\/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-239664","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/239664","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=239664"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/239664\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=239664"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=239664"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=239664"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}