{"id":248651,"date":"2025-07-08T14:41:13","date_gmt":"2025-07-08T14:41:13","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=248651"},"modified":"2025-07-08T14:41:15","modified_gmt":"2025-07-08T14:41:15","slug":"would-you-expect-the-equilibrium-to-lie-to-the-right-or-the-left","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/08\/would-you-expect-the-equilibrium-to-lie-to-the-right-or-the-left\/","title":{"rendered":"Would you expect the equilibrium to lie to the right or the left"},"content":{"rendered":"\n
HBrO2(aq) + BrO3-(aq) \u00e2\u2020\u201d BrO2-(aq) + HBrO3(aq) Would you expect the equilibrium to lie to the right or the left? Why? 2. HSO4-(aq) + H2PO4-(aq) \u00e2\u2020\u201d SO4-2(aq) + H3PO4(aq) a) What is the acid in this reaction (from a Br\u00c3\u00b8nsted-Lowry point of view)? b) If the equilibrium lies to the right, what does this mean concerning acid and base strengths?<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
Equilibrium Position:<\/strong> The equilibrium in this reaction is likely to lie to the left<\/strong>, as HBrO2<\/strong> is a stronger acid compared to HBrO3<\/strong>, and BrO3-<\/strong> is a stronger base compared to BrO2-<\/strong>.\n
\n
HBrO2<\/strong> can donate a proton to form BrO2-<\/strong>, while HBrO3<\/strong> is more likely to accept a proton to form HBrO2<\/strong>.<\/li>\n\n\n\n
Therefore, the system will favor the side with the stronger acid and weaker base. In this case, HBrO2<\/strong> is the stronger acid, and BrO3-<\/strong> is the stronger base, so the equilibrium tends to shift to the left, favoring the reactants.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n
(a) Acid (from a Br\u00f8nsted-Lowry Point of View):<\/strong>\n
\n
HSO4-<\/strong> is the acid in this reaction.<\/li>\n\n\n\n
According to the Br\u00f8nsted-Lowry theory, acids are proton donors. In this reaction, HSO4-<\/strong> donates a proton to form SO4\u00b2\u207b<\/strong>, while H2PO4-<\/strong> (hydrogen phosphate) acts as the base by accepting the proton to form H3PO4<\/strong> (phosphoric acid).<\/li>\n<\/ul>\n<\/li>\n\n\n\n
(b) Meaning if Equilibrium Lies to the Right:<\/strong>\n
\n
If the equilibrium lies to the right, this indicates that SO4\u00b2-<\/strong> and H3PO4<\/strong> are favored products. This means that HSO4-<\/strong> (bisulfate) is a stronger acid than H2PO4-<\/strong> (dihydrogen phosphate), and H3PO4<\/strong> is a weaker acid than H2PO4-<\/strong>.<\/li>\n\n\n\n
The proton transfer happens in such a way that the stronger acid (HSO4-<\/strong>) donates a proton to the weaker acid (H2PO4-<\/strong>), shifting the equilibrium toward the formation of SO4\u00b2-<\/strong> and H3PO4<\/strong>.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n
In summary, the equilibrium for both reactions is influenced by the relative strengths of the acids and bases involved. Stronger acids favor the dissociation, and weaker bases tend to accept protons, leading to a shift toward the products.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"
HBrO2(aq) + BrO3-(aq) \u00e2\u2020\u201d BrO2-(aq) + HBrO3(aq) Would you expect the equilibrium to lie to the right or the left? Why? 2. HSO4-(aq) + H2PO4-(aq) \u00e2\u2020\u201d SO4-2(aq) + H3PO4(aq) a) What is the acid in this reaction (from a Br\u00c3\u00b8nsted-Lowry point of view)? b) If the equilibrium lies to the right, what does this mean […]<\/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-248651","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/248651","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=248651"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/248651\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=248651"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=248651"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=248651"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
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