{"id":193999,"date":"2025-02-22T06:42:55","date_gmt":"2025-02-22T06:42:55","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=193999"},"modified":"2025-02-22T06:42:58","modified_gmt":"2025-02-22T06:42:58","slug":"write-the-formula-for-the-conjugate-acid-of-each-of-the-following-bases","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/22\/write-the-formula-for-the-conjugate-acid-of-each-of-the-following-bases\/","title":{"rendered":"Write the formula for the conjugate acid of each of the following bases"},"content":{"rendered":"\n

You may want to reference (Page) section 16.3 while completing this problem.
Write the formula for the conjugate acid of each of the following bases<\/p>\n\n\n\n

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

Answers:<\/h3>\n\n\n\n
    \n
  1. Conjugate Acid of NH\u2083 (Ammonia):<\/strong>
    [
    \\text{NH}_4^+ (\\text{Ammonium Ion})
    ]<\/li>\n\n\n\n
  2. Conjugate Acid of OH\u207b (Hydroxide Ion):<\/strong>
    [
    \\text{H}_2\\text{O} (\\text{Water})
    ]<\/li>\n\n\n\n
  3. Conjugate Acid of CO\u2083\u00b2\u207b (Carbonate Ion):<\/strong>
    [
    \\text{HCO}_3^- (\\text{Bicarbonate Ion})
    ]<\/li>\n\n\n\n
  4. Conjugate Acid of HPO\u2084\u00b2\u207b (Hydrogen Phosphate Ion):<\/strong>
    [
    \\text{H}_2\\text{PO}_4^- (\\text{Dihydrogen Phosphate Ion})
    ]<\/li>\n<\/ol>\n\n\n\n
    \n\n\n\n

    Explanation:<\/h3>\n\n\n\n

    In acid-base chemistry, the conjugate acid<\/strong> of a base is formed by adding a proton (( H^+ )) to the base. This is based on the Br\u00f8nsted-Lowry acid-base theory<\/strong>, which defines acids as proton donors and bases as proton acceptors.<\/p>\n\n\n\n

    1. NH\u2083 (Ammonia) \u2192 NH\u2084\u207a (Ammonium Ion)<\/strong><\/h4>\n\n\n\n

    Ammonia (( \\text{NH}_3 )) is a weak base that can accept a proton to form ammonium ion (( \\text{NH}_4^+ )). This process occurs in water and is common in biological and chemical systems:
    [
    \\text{NH}_3 + H^+ \\rightarrow \\text{NH}_4^+
    ]<\/p>\n\n\n\n

    2. OH\u207b (Hydroxide Ion) \u2192 H\u2082O (Water)<\/strong><\/h4>\n\n\n\n

    Hydroxide ion (( \\text{OH}^- )) is a strong base that readily accepts a proton to form neutral water:
    [
    \\text{OH}^- + H^+ \\rightarrow \\text{H}_2\\text{O}
    ]
    This is one of the most fundamental acid-base reactions, forming the basis of pH and neutralization reactions.<\/p>\n\n\n\n

    3. CO\u2083\u00b2\u207b (Carbonate Ion) \u2192 HCO\u2083\u207b (Bicarbonate Ion)<\/strong><\/h4>\n\n\n\n

    Carbonate (( \\text{CO}_3^{2-} )) is a polyatomic anion that can accept a proton to form the bicarbonate ion<\/strong>:
    [
    \\text{CO}_3^{2-} + H^+ \\rightarrow \\text{HCO}_3^-
    ]
    Bicarbonate is an important buffer in biological and environmental chemistry.<\/p>\n\n\n\n

    4. HPO\u2084\u00b2\u207b (Hydrogen Phosphate Ion) \u2192 H\u2082PO\u2084\u207b (Dihydrogen Phosphate Ion)<\/strong><\/h4>\n\n\n\n

    Hydrogen phosphate (( \\text{HPO}_4^{2-} )) can accept a proton to form dihydrogen phosphate:
    [
    \\text{HPO}_4^{2-} + H^+ \\rightarrow \\text{H}_2\\text{PO}_4^-
    ]
    This reaction plays a key role in the phosphate buffer system, important for maintaining pH in biological fluids.<\/p>\n\n\n\n

    \n\n\n\n

    These conjugate acids are essential in chemical equilibrium, buffer solutions, and biological systems, ensuring pH stability.<\/p>\n\n\n\n

    Here is the scientific illustration of acid-base conjugate pairs, visually representing the transformation of bases into their conjugate acids. Let me know if you need any modifications!<\/p>\n\n\n\n

    \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

    You may want to reference (Page) section 16.3 while completing this problem.Write the formula for the conjugate acid of each of the following bases The Correct Answer and Explanation is : Answers: Explanation: In acid-base chemistry, the conjugate acid of a base is formed by adding a proton (( H^+ )) to the base. This […]<\/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-193999","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/193999","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=193999"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/193999\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=193999"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=193999"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=193999"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}