![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/04\/image-44.png\")
<\/figure>\n\n\n\nHowever, here is the correct answer<\/strong> and a 300-word explanation<\/strong> for the question:<\/p>\n\n\n\n Ka \u2248 5.36 \u00d7 10\u207b\u2074<\/strong><\/p>\n\n\n\n To find the acid dissociation constant (Ka)<\/strong> for a monoprotic acid<\/strong>, we follow these steps:<\/p>\n\n\n\n The pH<\/strong> of the solution is given as 2.53<\/strong>. Since pH is the negative logarithm of the hydrogen ion concentration, we use: The monoprotic acid dissociates as follows: Let\u2019s assume the initial concentration of HA is 0.0192 M<\/strong>, and none of it has dissociated yet.<\/p>\n\n\n\n At equilibrium:<\/p>\n\n\n\n [ The acid dissociation constant (Ka<\/strong>) reflects how strongly the acid ionizes in water. A Ka \u2248 5.36 \u00d7 10\u207b\u2074<\/strong> suggests this is a weak acid<\/strong>, which only partially ionizes in solution.<\/p>\n","protected":false},"excerpt":{"rendered":" Enough of a monoprotic acid is dissolved in water to produce a 0.0192 M solution. The pH of the resulting solution is 2.53. Calculate the Ka for the acid. The correct answer and explanation is : However, here is the correct answer and a 300-word explanation for the question: Correct Answer: Ka \u2248 5.36 \u00d7 […]<\/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-206691","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/206691","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=206691"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/206691\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=206691"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=206691"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=206691"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Correct Answer:<\/strong><\/h3>\n\n\n\n
\n\n\n\nDetailed Explanation:<\/strong><\/h3>\n\n\n\n
1. Use the pH to find [H\u207a]:<\/strong><\/h4>\n\n\n\n
[
[H^+] = 10^{-pH} = 10^{-2.53} \\approx 2.95 \\times 10^{-3} \\, \\text{M}
]<\/p>\n\n\n\n2. Set up the equilibrium expression:<\/strong><\/h4>\n\n\n\n
[
HA \\rightleftharpoons H^+ + A^-
]<\/p>\n\n\n\n\n
3. Apply the Ka formula:<\/strong><\/h4>\n\n\n\n
Ka = \\frac{[H^+][A^-]}{[HA]} = \\frac{(2.95 \\times 10^{-3})^2}{0.0192 – 2.95 \\times 10^{-3}} \\approx \\frac{8.70 \\times 10^{-6}}{0.0162} \\approx 5.36 \\times 10^{-4}
]<\/p>\n\n\n\n
\n\n\n\nConclusion:<\/strong><\/h3>\n\n\n\n