{"id":202137,"date":"2025-03-17T08:09:17","date_gmt":"2025-03-17T08:09:17","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=202137"},"modified":"2025-03-17T08:09:19","modified_gmt":"2025-03-17T08:09:19","slug":"enough-of-a-monoprotic-acid-is-dissolved-in-water-to-produce-a-0-0192-m-solution-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/17\/enough-of-a-monoprotic-acid-is-dissolved-in-water-to-produce-a-0-0192-m-solution-2\/","title":{"rendered":"Enough of a monoprotic acid is dissolved in water to produce a 0.0192 M solution"},"content":{"rendered":"\n

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.<\/p>\n\n\n\n

The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n

To calculate the acid dissociation constant (Ka<\/strong>) of the monoprotic acid, we follow these steps:<\/p>\n\n\n\n

Step 1: Define the Dissociation Reaction<\/strong><\/h3>\n\n\n\n

Let HA represent the monoprotic acid. It dissociates as:<\/p>\n\n\n\n

[
HA \\rightleftharpoons H^+ + A^-
]<\/p>\n\n\n\n

Given:<\/p>\n\n\n\n

    \n
  • Initial concentration of HA<\/strong> = 0.0192 M<\/li>\n\n\n\n
  • pH<\/strong> = 2.53<\/li>\n<\/ul>\n\n\n\n

    Step 2: Determine ([H^+])<\/strong><\/h3>\n\n\n\n

    The concentration of hydrogen ions ([H^+]) can be found using the pH formula:<\/p>\n\n\n\n

    [
    [H^+] = 10^{-\\text{pH}}
    ]<\/p>\n\n\n\n

    [
    [H^+] = 10^{-2.53} = 2.95 \\times 10^{-3} \\text{ M}
    ]<\/p>\n\n\n\n

    Step 3: Set Up the ICE Table<\/strong><\/h3>\n\n\n\n
    Species<\/th>Initial (M)<\/th>Change (M)<\/th>Equilibrium (M)<\/th><\/tr><\/thead>
    HA<\/td>0.0192<\/td>(- x)<\/td>0.0192 – x<\/td><\/tr>
    H\u207a<\/td>0<\/td>(+x)<\/td>(2.95 \\times 10^{-3})<\/td><\/tr>
    A\u207b<\/td>0<\/td>(+x)<\/td>(2.95 \\times 10^{-3})<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

    Since ([H^+] = x = 2.95 \\times 10^{-3}), the equilibrium concentration of HA is:<\/p>\n\n\n\n

    [
    [HA] = 0.0192 – 2.95 \\times 10^{-3} = 0.0163 \\text{ M}
    ]<\/p>\n\n\n\n

    Step 4: Calculate (K_a)<\/strong><\/h3>\n\n\n\n

    The acid dissociation constant is given by:<\/p>\n\n\n\n

    [
    K_a = \\frac{[H^+][A^-]}{[HA]}
    ]<\/p>\n\n\n\n

    [
    K_a = \\frac{(2.95 \\times 10^{-3}) (2.95 \\times 10^{-3})}{0.0163}
    ]<\/p>\n\n\n\n

    [
    K_a = \\frac{8.70 \\times 10^{-6}}{0.0163}
    ]<\/p>\n\n\n\n

    [
    K_a = 5.34 \\times 10^{-4}
    ]<\/p>\n\n\n\n

    Final Answer:<\/strong><\/h3>\n\n\n\n

    [
    K_a = 5.34 \\times 10^{-4}
    ]<\/p>\n\n\n\n

    Explanation (300 Words)<\/strong><\/h3>\n\n\n\n

    The acid dissociation constant ((K_a)) quantifies the strength of an acid in solution. A monoprotic acid ((HA)) dissociates into hydrogen ions ((H^+)) and conjugate base ((A^-)). Given a 0.0192 M acid solution with a pH of 2.53, we first find ([H^+]) using (10^{-\\text{pH}}), yielding (2.95 \\times 10^{-3}) M. Since ([H^+]) equals the dissociated amount of acid, we subtract this from the initial concentration to find the remaining ([HA]). The equilibrium concentrations allow us to apply the (K_a) formula: (\\frac{[H^+][A^-]}{[HA]}). Substituting values, we calculate (K_a = 5.34 \\times 10^{-4}), which is a moderate value, suggesting the acid is weak but partially dissociated 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 : To calculate the acid dissociation constant (Ka) of the monoprotic acid, we follow these steps: Step 1: Define the […]<\/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-202137","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/202137","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=202137"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/202137\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=202137"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=202137"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=202137"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}