{"id":245556,"date":"2025-07-06T08:57:20","date_gmt":"2025-07-06T08:57:20","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=245556"},"modified":"2025-07-06T08:57:22","modified_gmt":"2025-07-06T08:57:22","slug":"a-buffer-is-prepared-by-mixing-hypochlorous-acid-hclo-and-sodium-hypochlorite","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/06\/a-buffer-is-prepared-by-mixing-hypochlorous-acid-hclo-and-sodium-hypochlorite\/","title":{"rendered":"A buffer is prepared by mixing hypochlorous acid (HClO) and sodium hypochlorite"},"content":{"rendered":"\n<p>A buffer is prepared by mixing hypochlorous acid (HClO) and sodium hypochlorite (NaClO). If a strong base, such as NaOH, is added to this buffer, which buffer component neutralizes the additional hydroxide ions (OH?)? ClO? HClO Write a balanced chemical equation for the reaction of the selected buffer component and the hydroxide ion (OH?). Do not include physical states. chemical equation<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>In the buffer solution prepared by mixing hypochlorous acid (HClO) and sodium hypochlorite (NaClO), the component that neutralizes additional hydroxide ions (OH-) when a strong base like NaOH is added is <strong>HClO (hypochlorous acid)<\/strong>.<\/p>\n\n\n\n<p><strong>Why HClO Neutralizes OH-:<\/strong><br>A buffer works by maintaining the pH of the solution when small amounts of acid or base are added. The key mechanism relies on the presence of a weak acid and its conjugate base in equilibrium. In this case, HClO is a weak acid and NaClO is its conjugate base. When NaOH is added, the hydroxide ions (OH-) from NaOH will be neutralized by HClO, the weak acid, because acids donate protons (H+), which will combine with OH- to form water.<\/p>\n\n\n\n<p><strong>Balanced Chemical Equation:<\/strong><br>The neutralization of hydroxide ions by HClO can be represented by the following balanced chemical equation:HClO+OH\u2212\u2192ClO\u2212+H2OHClO + OH- \\rightarrow ClO- + H2OHClO+OH\u2212\u2192ClO\u2212+H2O<\/p>\n\n\n\n<p>Here, HClO (hypochlorous acid) donates a proton (H+) to neutralize the hydroxide ion (OH-), forming the conjugate base, ClO- (hypochlorite ion), and water (H2O).<\/p>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>When NaOH is added to the buffer, it dissociates into Na+ and OH- ions. The hydroxide ions from NaOH will react with the weak acid, HClO, to form the conjugate base, ClO-, and water.<\/li>\n\n\n\n<li>This reaction helps to prevent a drastic increase in pH because the addition of hydroxide ions (OH-) would otherwise make the solution more basic. However, because HClO reacts with the OH-, the pH remains relatively stable.<\/li>\n\n\n\n<li>The buffer capacity is a result of the equilibrium between HClO and ClO- in solution, which can shift depending on the amounts of acid and base added.<\/li>\n<\/ul>\n\n\n\n<p>In summary, the weak acid component, HClO, is responsible for neutralizing excess OH- when a strong base is introduced into the buffer solution.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-659.jpeg\" alt=\"\" class=\"wp-image-245557\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>A buffer is prepared by mixing hypochlorous acid (HClO) and sodium hypochlorite (NaClO). If a strong base, such as NaOH, is added to this buffer, which buffer component neutralizes the additional hydroxide ions (OH?)? ClO? HClO Write a balanced chemical equation for the reaction of the selected buffer component and the hydroxide ion (OH?). Do [&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-245556","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/245556","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=245556"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/245556\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=245556"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=245556"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=245556"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}