{"id":191256,"date":"2025-02-14T10:58:32","date_gmt":"2025-02-14T10:58:32","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=191256"},"modified":"2025-02-14T10:58:35","modified_gmt":"2025-02-14T10:58:35","slug":"on-the-polyprotic-weak-acid-strong-base-titration-curve-below-label-the-following-points","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/14\/on-the-polyprotic-weak-acid-strong-base-titration-curve-below-label-the-following-points\/","title":{"rendered":"On the polyprotic weak acid\/strong base titration curve below, label the following points"},"content":{"rendered":"\n

On the polyprotic weak acid\/strong base titration curve below, label the following points.
The point where the pH corresponds to a solution of H\u2082A in water.
b) The point where the pH corresponds to a solution of HA” in water.
) The point where the pH corresponds to a solution of A\u00b3 in water. c
d) The point where pH = pKa
e) The point where pH = pK_a2.<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n

    \n
  1. The point where the pH corresponds to a solution of H\u2082A in water<\/strong>: This corresponds to the initial point in the titration before any base is added. At this point, the solution contains only the weak acid (H\u2082A), which can donate protons (H\u207a) to the solution. You will typically observe a relatively low pH because H\u2082A partially dissociates in water.<\/li>\n\n\n\n
  2. The point where the pH corresponds to a solution of HA\u207b in water<\/strong>: This occurs after the first dissociation of H\u2082A has happened but before the second dissociation. The solution now contains the conjugate base of the weak acid, HA\u207b. HA\u207b is a weaker base compared to A\u00b2\u207b, but it can still accept protons. The pH at this point will be higher than the initial pH of the H\u2082A solution because HA\u207b raises the pH by absorbing H\u207a ions.<\/li>\n\n\n\n
  3. The point where the pH corresponds to a solution of A\u00b2\u207b in water<\/strong>: This point comes after the second dissociation of the acid. The solution now contains A\u00b2\u207b, the fully deprotonated form of the acid. A\u00b2\u207b is a stronger base than HA\u207b and will absorb protons from the water, significantly raising the pH.<\/li>\n\n\n\n
  4. The point where pH = pKa\u2081<\/strong>: This occurs at the first equivalence point, where the concentration of H\u2082A is equal to HA\u207b. At this point, the pH of the solution is roughly equal to the pKa\u2081 (the first dissociation constant) because the weak acid has been partially converted to its conjugate base, and the system is at a buffering point.<\/li>\n\n\n\n
  5. The point where pH = pKa\u2082<\/strong>: This corresponds to the second equivalence point, where the concentration of HA\u207b is equal to A\u00b2\u207b. At this point, the pH is approximately equal to the pKa\u2082, the second dissociation constant, as the weak acid has been fully converted to its conjugate base, and the system is buffering again, but this time at a higher pH.<\/li>\n<\/ol>\n\n\n\n

    Let me know if you need any further clarification!<\/p>\n","protected":false},"excerpt":{"rendered":"

    On the polyprotic weak acid\/strong base titration curve below, label the following points.The point where the pH corresponds to a solution of H\u2082A in water.b) The point where the pH corresponds to a solution of HA” in water.) The point where the pH corresponds to a solution of A\u00b3 in water. cd) The point where […]<\/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-191256","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191256","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=191256"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191256\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=191256"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=191256"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=191256"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}