{"id":206679,"date":"2025-04-08T06:28:05","date_gmt":"2025-04-08T06:28:05","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=206679"},"modified":"2025-04-08T06:28:08","modified_gmt":"2025-04-08T06:28:08","slug":"using-data-from-appendix-d-in-the-textbook","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/04\/08\/using-data-from-appendix-d-in-the-textbook\/","title":{"rendered":"Using data from Appendix D in the textbook"},"content":{"rendered":"\n<p>Using data from Appendix D in the textbook, calculate [OH\u2212] and pH for each of the following solutions.<\/p>\n\n\n\n<p>Calculate the [OH] and the pH.<\/p>\n\n\n\n<p>A mixture that is 5.2\u00d710\u22122 M in NaC2H3O2 and 5.7\u00d710\u22122 M in Ba(C2H3O2)2.<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Final Answer:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>[OH\u207b] = 9.60 \u00d7 10\u207b\u2076 M<\/strong><\/li>\n\n\n\n<li><strong>pH = 8.98<\/strong><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation (300+ words):<\/h3>\n\n\n\n<p>To calculate the hydroxide ion concentration ([OH\u207b]) and the pH of the given solution, we must understand the chemistry of the solutes involved:<\/p>\n\n\n\n<p>The solution contains:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Sodium acetate (NaC\u2082H\u2083O\u2082)<\/strong>, a salt of a weak acid (acetic acid), which dissociates to give <strong>acetate ions (C\u2082H\u2083O\u2082\u207b)<\/strong>.<\/li>\n\n\n\n<li><strong>Barium acetate [Ba(C\u2082H\u2083O\u2082)\u2082]<\/strong>, which dissociates to give <strong>two acetate ions per formula unit<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p>First, we calculate the <strong>total acetate ion concentration<\/strong> contributed by both salts:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sodium acetate provides 0.052 M acetate ions.<\/li>\n\n\n\n<li>Barium acetate (0.057 M) provides <strong>0.057 \u00d7 2 = 0.114 M<\/strong> acetate ions.<\/li>\n\n\n\n<li><strong>Total acetate ion concentration<\/strong> = 0.052 + 0.114 = <strong>0.166 M<\/strong><\/li>\n<\/ul>\n\n\n\n<p>The acetate ion is the <strong>conjugate base of acetic acid<\/strong> (CH\u2083COOH), a weak acid. It undergoes hydrolysis in water:<br>[<br>C\u2082H\u2083O\u2082\u207b + H\u2082O \u21cc HC\u2082H\u2083O\u2082 + OH\u207b<br>]<br>This reaction produces hydroxide ions, making the solution basic.<\/p>\n\n\n\n<p>We use the <strong>base dissociation constant<\/strong> (K_b) of the acetate ion to determine ([OH\u207b]). (K_b) can be derived from the relation:<br>[<br>K_b = \\frac{K_w}{K_a}<br>]<br>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>(K_w = 1.0 \u00d7 10^{-14}) (ion-product of water),<\/li>\n\n\n\n<li>(K_a = 1.8 \u00d7 10^{-5}) (for acetic acid from Appendix D).<\/li>\n<\/ul>\n\n\n\n<p>[<br>K_b = \\frac{1.0 \u00d7 10^{-14}}{1.8 \u00d7 10^{-5}} \u2248 5.56 \u00d7 10^{-10}<br>]<\/p>\n\n\n\n<p>Now apply the formula:<br>[<br>[OH\u207b] \u2248 \\sqrt{K_b \u00d7 [C\u2082H\u2083O\u2082\u207b]} = \\sqrt{5.56 \u00d7 10^{-10} \u00d7 0.166} \u2248 9.60 \u00d7 10^{-6} \\text{ M}<br>]<\/p>\n\n\n\n<p>Next, we find <strong>pOH<\/strong>:<br>[<br>pOH = -\\log_{10}[OH\u207b] \u2248 -\\log_{10}(9.60 \u00d7 10^{-6}) \u2248 5.02<br>]<\/p>\n\n\n\n<p>Then, calculate <strong>pH<\/strong>:<br>[<br>pH = 14 &#8211; pOH \u2248 14 &#8211; 5.02 = 8.98<br>]<\/p>\n\n\n\n<p>Thus, the solution is slightly basic due to the presence of the weak base (acetate ion).<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Image Representation:<\/h3>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/04\/image-41.png\" alt=\"\" class=\"wp-image-206680\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Using data from Appendix D in the textbook, calculate [OH\u2212] and pH for each of the following solutions. Calculate the [OH] and the pH. A mixture that is 5.2\u00d710\u22122 M in NaC2H3O2 and 5.7\u00d710\u22122 M in Ba(C2H3O2)2. The correct answer and explanation is : Final Answer: Explanation (300+ words): To calculate the hydroxide ion concentration [&hellip;]<\/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-206679","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/206679","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=206679"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/206679\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=206679"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=206679"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=206679"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}