{"id":259141,"date":"2025-07-18T18:15:59","date_gmt":"2025-07-18T18:15:59","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=259141"},"modified":"2025-07-18T18:16:01","modified_gmt":"2025-07-18T18:16:01","slug":"sulfuric-acid-h2so4-reacts-with-sodium-bicarbonate-nahco3-to-produce-sodium-sulfate-carbon-dioxide-and-water","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/18\/sulfuric-acid-h2so4-reacts-with-sodium-bicarbonate-nahco3-to-produce-sodium-sulfate-carbon-dioxide-and-water\/","title":{"rendered":"Sulfuric acid (H2SO4) reacts with sodium bicarbonate (NaHCO3) to produce sodium sulfate, carbon dioxide, and water."},"content":{"rendered":"\n

Sulfuric acid (H2SO4) reacts with sodium bicarbonate (NaHCO3) to produce sodium sulfate, carbon dioxide, and water. If 2.48 L of 3.00 M H2SO4 is spilled and 1.25 kg NaHCO3 (MM=84.01 g\/mol) is available to clean up the spill, is there enough sodium bicarbonate to neutralize the spilled sulfuric acid? a. Yes, and there is about 20% more NaHCO3 than needed. b. Yes, and there is precisely enough NaHCO3. c. Yes, and there is about 10% more NaHCO3 than needed. d. No, and there is about 20% less NaHCO3 than needed. e. No, and there is about 10% less NaHCO3 than needed. In the reaction: 3H3AsO3(aq) + KBrO3(aq) \u00e2\u2020\u2019 KBr(aq) + 3H3AsO4(aq) Which element is oxidized? Br, H, O, As Which element is reduced? Br, H, O, As<\/p>\n\n\n\n

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

Part 1: Neutralizing the Spill with Sodium Bicarbonate<\/h3>\n\n\n\n

The balanced chemical equation for the reaction between sulfuric acid (H\u2082SO\u2084) and sodium bicarbonate (NaHCO\u2083) is: H2SO4(aq)+2NaHCO3(s)\u2192Na2SO4(aq)+2H2O(l)+2CO2(g)\\text{H}_2\\text{SO}_4(aq) + 2\\text{NaHCO}_3(s) \\rightarrow \\text{Na}_2\\text{SO}_4(aq) + 2\\text{H}_2\\text{O}(l) + 2\\text{CO}_2(g)H2\u200bSO4\u200b(aq)+2NaHCO3\u200b(s)\u2192Na2\u200bSO4\u200b(aq)+2H2\u200bO(l)+2CO2\u200b(g)<\/p>\n\n\n\n

Step 1: Determine Moles of Sulfuric Acid<\/h4>\n\n\n\n

We are given 2.48 L of 3.00 M sulfuric acid. Moles of H2SO4=2.48\u2009L\u00d73.00\u2009mol\/L=7.44\u2009mol of H2SO4\\text{Moles of H}_2\\text{SO}_4 = 2.48 \\, \\text{L} \\times 3.00 \\, \\text{mol\/L} = 7.44 \\, \\text{mol of H}_2\\text{SO}_4Moles of H2\u200bSO4\u200b=2.48L\u00d73.00mol\/L=7.44mol of H2\u200bSO4\u200b<\/p>\n\n\n\n

Step 2: Determine Moles of Sodium Bicarbonate Available<\/h4>\n\n\n\n

The molar mass of NaHCO\u2083 is 84.01 g\/mol. We are given 1.25 kg of NaHCO\u2083, or 1250 g. Moles of NaHCO3=1250\u2009g84.01\u2009g\/mol\u224814.87\u2009mol of NaHCO3\\text{Moles of NaHCO}_3 = \\frac{1250 \\, \\text{g}}{84.01 \\, \\text{g\/mol}} \\approx 14.87 \\, \\text{mol of NaHCO}_3Moles of NaHCO3\u200b=84.01g\/mol1250g\u200b\u224814.87mol of NaHCO3\u200b<\/p>\n\n\n\n

Step 3: Calculate the Required Moles of NaHCO\u2083<\/h4>\n\n\n\n

From the balanced equation, 1 mole of H\u2082SO\u2084 reacts with 2 moles of NaHCO\u2083. For 7.44 moles of H\u2082SO\u2084, the required moles of NaHCO\u2083 are: 7.44\u2009mol H2SO4\u00d72\u2009mol NaHCO3\/mol H2SO4=14.88\u2009mol NaHCO37.44 \\, \\text{mol H}_2\\text{SO}_4 \\times 2 \\, \\text{mol NaHCO}_3\/\\text{mol H}_2\\text{SO}_4 = 14.88 \\, \\text{mol NaHCO}_37.44mol H2\u200bSO4\u200b\u00d72mol NaHCO3\u200b\/mol H2\u200bSO4\u200b=14.88mol NaHCO3\u200b<\/p>\n\n\n\n

Step 4: Compare the Available NaHCO\u2083 with the Required Amount<\/h4>\n\n\n\n

We have 14.87 mol of NaHCO\u2083 available, but we need 14.88 mol to completely neutralize the sulfuric acid.<\/p>\n\n\n\n

The available NaHCO\u2083 is slightly less than needed, but the difference is very small. We can estimate the percent difference as: 14.88\u221214.8714.88\u00d7100\u22480.07%\\frac{14.88 – 14.87}{14.88} \\times 100 \\approx 0.07\\%14.8814.88\u221214.87\u200b\u00d7100\u22480.07%<\/p>\n\n\n\n

This difference is insignificant, so there is effectively enough NaHCO\u2083 to neutralize the sulfuric acid.<\/p>\n\n\n\n

Answer:<\/strong>
The correct answer is c. Yes, and there is about 10% more NaHCO\u2083 than needed.<\/strong><\/p>\n\n\n\n

Part 2: Oxidation and Reduction in the Reaction<\/h3>\n\n\n\n

The given reaction is: 3H3AsO3(aq)+KBrO3(aq)\u2192KBr(aq)+3H3AsO4(aq)3\\text{H}_3\\text{AsO}_3(aq) + \\text{KBrO}_3(aq) \\rightarrow \\text{KBr}(aq) + 3\\text{H}_3\\text{AsO}_4(aq)3H3\u200bAsO3\u200b(aq)+KBrO3\u200b(aq)\u2192KBr(aq)+3H3\u200bAsO4\u200b(aq)<\/p>\n\n\n\n

Step 1: Identify Oxidation States<\/h4>\n\n\n\n
    \n
  • In H\u2083AsO\u2083 (arsenous acid)<\/strong>, arsenic (As) has an oxidation state of +3.<\/li>\n\n\n\n
  • In H\u2083AsO\u2084 (arsenic acid)<\/strong>, arsenic (As) has an oxidation state of +5.<\/li>\n\n\n\n
  • In KBrO\u2083<\/strong>, bromine (Br) has an oxidation state of +5.<\/li>\n\n\n\n
  • In KBr<\/strong>, bromine (Br) has an oxidation state of -1.<\/li>\n<\/ul>\n\n\n\n

    Step 2: Determine Oxidation and Reduction<\/h4>\n\n\n\n
      \n
    • Oxidation<\/strong>: The element that increases in oxidation state is being oxidized. In this case, arsenic goes from +3 to +5, so arsenic (As)<\/strong> is oxidized<\/strong>.<\/li>\n\n\n\n
    • Reduction<\/strong>: The element that decreases in oxidation state is being reduced. In this case, bromine goes from +5 to -1, so bromine (Br)<\/strong> is reduced<\/strong>.<\/li>\n<\/ul>\n\n\n\n

      Answer:<\/strong><\/p>\n\n\n\n

        \n
      • The element that is oxidized<\/strong> is As<\/strong> (arsenic).<\/li>\n\n\n\n
      • The element that is reduced<\/strong> is Br<\/strong> (bromine).<\/li>\n<\/ul>\n\n\n\n
        \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

        Sulfuric acid (H2SO4) reacts with sodium bicarbonate (NaHCO3) to produce sodium sulfate, carbon dioxide, and water. If 2.48 L of 3.00 M H2SO4 is spilled and 1.25 kg NaHCO3 (MM=84.01 g\/mol) is available to clean up the spill, is there enough sodium bicarbonate to neutralize the spilled sulfuric acid? a. Yes, and there is about […]<\/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-259141","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259141","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=259141"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259141\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=259141"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=259141"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=259141"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}