{"id":192934,"date":"2025-02-18T12:49:51","date_gmt":"2025-02-18T12:49:51","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=192934"},"modified":"2025-02-18T12:50:16","modified_gmt":"2025-02-18T12:50:16","slug":"given-that-kb-for-ammonia-is-1-8-x10-5-and-that-for","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/18\/given-that-kb-for-ammonia-is-1-8-x10-5-and-that-for\/","title":{"rendered":"Given that Kb for ammonia is 1.8 x10-5 and that formhydroxylamine is 1.1 x 10-8, which is the stronger base"},"content":{"rendered":"\n<p>(a) Given that Kb for ammonia is 1.8 x10-5 and that formhydroxylamine is 1.1 x 10-8, which is the stronger base?<br>(b) Which is the stronger acid, the ammonium ion or the<br>hydroxylammonium ion? (c) Calculate Ka values for NH4+<br>and H3NOH+.<\/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<p>Let&#8217;s break down each part of the problem.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">(a) Which is the stronger base, ammonia (NH\u2083) or hydroxylamine (NH\u2082OH)?<\/h3>\n\n\n\n<p>To determine which is the stronger base, we need to compare the values of their base dissociation constants (Kb). The Kb represents the strength of a base, with a higher Kb indicating a stronger base.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Kb for ammonia (NH\u2083) = 1.8 \u00d7 10\u207b\u2075<\/strong><\/li>\n\n\n\n<li><strong>Kb for hydroxylamine (NH\u2082OH) = 1.1 \u00d7 10\u207b\u2078<\/strong><\/li>\n<\/ul>\n\n\n\n<p>Since 1.8 \u00d7 10\u207b\u2075 is much larger than 1.1 \u00d7 10\u207b\u2078, ammonia is the stronger base. This means ammonia more readily accepts a proton (H\u207a) from water compared to hydroxylamine.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">(b) Which is the stronger acid, the ammonium ion (NH\u2084\u207a) or the hydroxylammonium ion (H\u2083NOH\u207a)?<\/h3>\n\n\n\n<p>To compare the strengths of these acids, we need to look at the values of their acid dissociation constants (Ka). A higher Ka indicates a stronger acid.<\/p>\n\n\n\n<p>We know that <strong>Ka = Kw \/ Kb<\/strong> (where Kw is the ionization constant for water, 1.0 \u00d7 10\u207b\u00b9\u2074 at 25\u00b0C). Therefore, we can calculate the Ka for each ion by using the Kb values from the previous part.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Kb for NH\u2083 = 1.8 \u00d7 10\u207b\u2075<\/strong>, so Ka for NH\u2084\u207a is:<br>[<br>\\text{Ka for NH\u2084\u207a} = \\frac{1.0 \\times 10^{-14}}{1.8 \\times 10^{-5}} = 5.56 \\times 10^{-10}<br>]<\/li>\n\n\n\n<li><strong>Kb for NH\u2082OH = 1.1 \u00d7 10\u207b\u2078<\/strong>, so Ka for H\u2083NOH\u207a is:<br>[<br>\\text{Ka for H\u2083NOH\u207a} = \\frac{1.0 \\times 10^{-14}}{1.1 \\times 10^{-8}} = 9.09 \\times 10^{-7}<br>]<\/li>\n<\/ul>\n\n\n\n<p>Since 9.09 \u00d7 10\u207b\u2077 is much larger than 5.56 \u00d7 10\u207b\u00b9\u2070, the <strong>hydroxylammonium ion (H\u2083NOH\u207a)<\/strong> is the stronger acid.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">(c) Calculating Ka values for NH\u2084\u207a and H\u2083NOH\u207a<\/h3>\n\n\n\n<p>As seen in part (b), we used the relationship between Kb and Ka to calculate the Ka values:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Ka for NH\u2084\u207a = 5.56 \u00d7 10\u207b\u00b9\u2070<\/strong><\/li>\n\n\n\n<li><strong>Ka for H\u2083NOH\u207a = 9.09 \u00d7 10\u207b\u2077<\/strong><\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Kb (Base Dissociation Constant)<\/strong> represents the extent to which a base accepts a proton in solution. The larger the Kb, the stronger the base.<\/li>\n\n\n\n<li><strong>Ka (Acid Dissociation Constant)<\/strong> represents the extent to which an acid donates a proton. The larger the Ka, the stronger the acid.<\/li>\n<\/ul>\n\n\n\n<p>By comparing the Kb values, we can deduce that ammonia is the stronger base because it has a higher Kb. Conversely, by comparing Ka values, we conclude that the hydroxylammonium ion is the stronger acid due to its larger Ka. The calculations for Ka using the Kb values of the conjugate bases follow directly from the formula Ka = Kw \/ Kb, where Kw is a known constant (1.0 \u00d7 10\u207b\u00b9\u2074 at 25\u00b0C).<\/p>\n","protected":false},"excerpt":{"rendered":"<p>(a) Given that Kb for ammonia is 1.8 x10-5 and that formhydroxylamine is 1.1 x 10-8, which is the stronger base?(b) Which is the stronger acid, the ammonium ion or thehydroxylammonium ion? (c) Calculate Ka values for NH4+and H3NOH+. The Correct Answer and Explanation is : Let&#8217;s break down each part of the problem. (a) [&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-192934","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/192934","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=192934"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/192934\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=192934"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=192934"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=192934"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}