{"id":182302,"date":"2025-01-13T15:59:12","date_gmt":"2025-01-13T15:59:12","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=182302"},"modified":"2025-01-13T16:08:28","modified_gmt":"2025-01-13T16:08:28","slug":"the-formula-for-the-conjugate-base-of-h2so3-is-the-formula-for-the-conjugate-acid-of-h2po4-is-compare-the-following-acid","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/13\/the-formula-for-the-conjugate-base-of-h2so3-is-the-formula-for-the-conjugate-acid-of-h2po4-is-compare-the-following-acid\/","title":{"rendered":"The formula for the conjugate base of H2SO3"},"content":{"rendered":"\n<p>1.) a. The formula for the conjugate base of H2SO3 is The formula for the conjugate acid of H2PO4- is Compare the following: Acid 1: hydrofluoric acid, HF Acid 2: hydrosulfuric acid, H2S Acid 3: carbonic acid, H2CO3 What is the formula for the weakest acid ? b. C. Compare the conjugate bases of these three acids. Acid 1: hypochlorous acid, HCIO Acid 2: phosphoric acid, H3PO4 Acid 3: hydrofluoric acid, HF What is the formula for the weakest conjugate base? d. e. f. Compare the conjugate bases of these three acids. Acid 1: hydrocyanic acid, HCN Acid 2: carbonic acid, H2CO3 Acid 3: hydrogen sulfite, HSO3- What is the formula for the strongest conjugate base? What is the hydronium ion concentration in an aqueous nitric acid solution with a pH of 3.730? [H3O+] = M What is the hydronium ion concentration in an aqueous nitric acid solution that has a pOH of 10.450? [H3O+] = M h. What is the pOH of an aqueous solution of 0.121 M hydrochloric acid?<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>Let&#8217;s break down the problems and address each one step by step.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">1a. Formula for the Conjugate Base of H2SO3<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>H2SO3 (sulfurous acid)<\/strong> dissociates as follows: H2SO3\u21ccH++HSO3\u2212H_2SO_3 \\rightleftharpoons H^+ + HSO_3^- The conjugate base of <strong>H2SO3<\/strong> is the species that remains after it donates a proton (H+), which is <strong>HSO3-<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">1b. Formula for the Conjugate Acid of H2PO4-<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>H2PO4-<\/strong> (dihydrogen phosphate ion) can accept a proton (H+) to form its conjugate acid: H2PO4\u2212+H+\u21ccH3PO4H_2PO_4^- + H^+ \\rightleftharpoons H_3PO_4 Therefore, the conjugate acid of <strong>H2PO4-<\/strong> is <strong>H3PO4<\/strong> (phosphoric acid).<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">2. Comparing the Weakest Acid<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Acid 1: HF (hydrofluoric acid)<\/strong>, <strong>Acid 2: H2S (hydrosulfuric acid)<\/strong>, and <strong>Acid 3: H2CO3 (carbonic acid)<\/strong>:\n<ul class=\"wp-block-list\">\n<li><strong>HF<\/strong> is a weak acid, with a pKa of 3.2.<\/li>\n\n\n\n<li><strong>H2S<\/strong> is also weak, with a pKa of 7.0 for the first dissociation.<\/li>\n\n\n\n<li><strong>H2CO3<\/strong> is weak, with a pKa of 6.4 for the first dissociation.<\/li>\n\n\n\n<li><strong>Weakest acid:<\/strong> <strong>H2S<\/strong> (because it has the highest pKa, indicating it&#8217;s less acidic).<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">3. Comparing Conjugate Bases of the Three Acids<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Acid 1: HOCl (hypochlorous acid)<\/strong>, <strong>Acid 2: H3PO4 (phosphoric acid)<\/strong>, and <strong>Acid 3: HF (hydrofluoric acid)<\/strong>:\n<ul class=\"wp-block-list\">\n<li>The conjugate base of <strong>HOCl<\/strong> is <strong>OCl-<\/strong> (hypochlorite).<\/li>\n\n\n\n<li>The conjugate base of <strong>H3PO4<\/strong> is <strong>H2PO4-<\/strong> (dihydrogen phosphate).<\/li>\n\n\n\n<li>The conjugate base of <strong>HF<\/strong> is <strong>F-<\/strong> (fluoride).<\/li>\n\n\n\n<li><strong>Weakest conjugate base:<\/strong> <strong>F-<\/strong> because it comes from the weakest acid, HF.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">4. Comparing the Conjugate Bases of These Three Acids<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Acid 1: HCN (hydrocyanic acid)<\/strong>, <strong>Acid 2: H2CO3 (carbonic acid)<\/strong>, and <strong>Acid 3: HSO3- (hydrogen sulfite)<\/strong>:\n<ul class=\"wp-block-list\">\n<li>The conjugate base of <strong>HCN<\/strong> is <strong>CN-<\/strong> (cyanide).<\/li>\n\n\n\n<li>The conjugate base of <strong>H2CO3<\/strong> is <strong>HCO3-<\/strong> (bicarbonate).<\/li>\n\n\n\n<li>The conjugate base of <strong>HSO3-<\/strong> is <strong>SO3^2-<\/strong> (sulfite).<\/li>\n\n\n\n<li><strong>Strongest conjugate base:<\/strong> <strong>SO3^2-<\/strong> because it is from the strongest acid (HSO3-).<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">5. Hydronium Ion Concentration with pH = 3.730<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The <strong>pH<\/strong> is related to the concentration of hydronium ions (H3O+): pH=\u2212log\u2061[H3O+]pH = -\\log[H_3O^+] To find <strong>[H3O+]<\/strong>, rearrange the equation: [H3O+]=10\u2212pH[H_3O^+] = 10^{-pH} Substituting the given pH value: [H3O+]=10\u22123.730\u22481.87\u00d710\u22124\u2009M[H_3O^+] = 10^{-3.730} \\approx 1.87 \\times 10^{-4} \\, \\text{M}<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">6. Hydronium Ion Concentration with pOH = 10.450<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>pH<\/strong> and <strong>pOH<\/strong> are related by the equation: pH+pOH=14pH + pOH = 14 Therefore, the pH is: pH=14\u221210.450=3.550pH = 14 &#8211; 10.450 = 3.550 Now, find <strong>[H3O+]<\/strong>: [H3O+]=10\u22123.550\u22482.82\u00d710\u22124\u2009M[H_3O^+] = 10^{-3.550} \\approx 2.82 \\times 10^{-4} \\, \\text{M}<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">7. pOH of 0.121 M Hydrochloric Acid<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Since <strong>HCl<\/strong> is a strong acid, it dissociates completely, so <strong>[H3O+]<\/strong> = 0.121 M.<\/li>\n\n\n\n<li>Use the relationship: pOH=14\u2212pHpOH = 14 &#8211; pH First, calculate <strong>pH<\/strong>: pH=\u2212log\u2061(0.121)\u22480.920pH = -\\log(0.121) \\approx 0.920 Now, calculate the pOH: pOH=14\u22120.920=13.080pOH = 14 &#8211; 0.920 = 13.080<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Conclusion<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li>Conjugate base of <strong>H2SO3<\/strong>: <strong>HSO3-<\/strong>.<\/li>\n\n\n\n<li>Conjugate acid of <strong>H2PO4-<\/strong>: <strong>H3PO4<\/strong>.<\/li>\n\n\n\n<li>Weakest acid: <strong>H2S<\/strong>.<\/li>\n\n\n\n<li>Weakest conjugate base: <strong>F-<\/strong>.<\/li>\n\n\n\n<li>Strongest conjugate base: <strong>SO3^2-<\/strong>.<\/li>\n\n\n\n<li><strong>[H3O+]<\/strong> for pH 3.730: <strong>1.87 \u00d7 10^-4 M<\/strong>.<\/li>\n\n\n\n<li><strong>[H3O+]<\/strong> for pOH 10.450: <strong>2.82 \u00d7 10^-4 M<\/strong>.<\/li>\n\n\n\n<li>pOH of 0.121 M HCl: <strong>13.080<\/strong>.<\/li>\n<\/ol>\n","protected":false},"excerpt":{"rendered":"<p>1.) a. The formula for the conjugate base of H2SO3 is The formula for the conjugate acid of H2PO4- is Compare the following: Acid 1: hydrofluoric acid, HF Acid 2: hydrosulfuric acid, H2S Acid 3: carbonic acid, H2CO3 What is the formula for the weakest acid ? b. C. Compare the conjugate bases of these [&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-182302","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182302","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=182302"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182302\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=182302"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=182302"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=182302"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}