{"id":236899,"date":"2025-06-16T15:58:40","date_gmt":"2025-06-16T15:58:40","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=236899"},"modified":"2025-06-16T15:58:42","modified_gmt":"2025-06-16T15:58:42","slug":"balanced-equations-for-the-reaction-of-aqueous-nitric-acid-and-aqueous-ammonia-balanced-equation-representing-aqueous-nitric-acid-and-aqueous-ammonia-reacting-4hno3aq-nh3aq-a%e2%80%a0","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/16\/balanced-equations-for-the-reaction-of-aqueous-nitric-acid-and-aqueous-ammonia-balanced-equation-representing-aqueous-nitric-acid-and-aqueous-ammonia-reacting-4hno3aq-nh3aq-a%e2%80%a0\/","title":{"rendered":"Balanced Equations for the Reaction of Aqueous Nitric Acid and Aqueous Ammonia Balanced equation representing aqueous nitric acid and aqueous ammonia reacting: 4HNO3(aq) + NH3(aq) \u00e2\u2020\u2019 NH4NO3(aq)."},"content":{"rendered":"\n

Title: Balanced Equations for the Reaction of Aqueous Nitric Acid and Aqueous Ammonia Balanced equation representing aqueous nitric acid and aqueous ammonia reacting: 4HNO3(aq) + NH3(aq) \u00e2\u2020\u2019 NH4NO3(aq). Identify all of the phases in your answer. Balanced net ionic equation representing aqueous nitric acid and aqueous ammonia reacting: H+(aq) + OH-(aq) \u00e2\u2020\u2019 H2O(l). Identify all of the phases in your answer.<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

The Correct Answer and Explanation is:<\/strong>1<\/a><\/sup><\/p>\n\n\n\n\n\n

Balanced Equations for the Reaction of Aqueous Nitric Acid and Aqueous Ammonia<\/h3>\n\n\n\n

Balanced molecular equation<\/strong> HNO3(aq) + NH3(aq) \u2192 NH4NO3(aq)<\/p>\n\n\n\n

Phases:<\/p>\n\n\n\n

    \n
  • HNO3 is aqueous (aq)<\/li>\n\n\n\n
  • NH3 is aqueous (aq)<\/li>\n\n\n\n
  • NH4NO3 is aqueous (aq)<\/li>\n<\/ul>\n\n\n\n

    Balanced net ionic equation<\/strong> H+(aq) + NH3(aq) \u2192 NH4+(aq)<\/p>\n\n\n\n

    Phases:<\/p>\n\n\n\n

      \n
    • H+ is aqueous (aq)<\/li>\n\n\n\n
    • NH3 is aqueous (aq)<\/li>\n\n\n\n
    • NH4+ is aqueous (aq)<\/li>\n<\/ul>\n\n\n\n

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

      The reaction between aqueous nitric acid and aqueous ammonia is an acid-base neutralization. Nitric acid (HNO3) is a strong acid that dissociates completely in water, producing hydrogen ions (H+) and nitrate ions (NO3-). Ammonia (NH3), on the other hand, is a weak base that does not fully dissociate but readily accepts a proton (H+) to form ammonium (NH4+).<\/p>\n\n\n\n

      The balanced molecular equation shows that nitric acid donates a proton to ammonia, leading to the formation of ammonium nitrate (NH4NO3). Since all reactants and products remain dissolved in water, they are labeled as aqueous.<\/p>\n\n\n\n

      To derive the net ionic equation, we focus on the species directly involved in the proton transfer. The nitrate ion (NO3-) does not participate in the reaction and is considered a spectator ion. The essential process is the transfer of a hydrogen ion from the acid to ammonia, forming the ammonium ion (NH4+). This simplifies the reaction to H+ + NH3 \u2192 NH4+.<\/p>\n\n\n\n

      This reaction is significant in various chemical and industrial processes. Ammonium nitrate is widely used as a fertilizer and has applications in explosives. Additionally, acid-base interactions like this play an important role in buffering solutions and maintaining pH stability in biological and environmental systems.<\/p>\n\n\n\n

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

      Title: Balanced Equations for the Reaction of Aqueous Nitric Acid and Aqueous Ammonia Balanced equation representing aqueous nitric acid and aqueous ammonia reacting: 4HNO3(aq) + NH3(aq) \u00e2\u2020\u2019 NH4NO3(aq). Identify all of the phases in your answer. Balanced net ionic equation representing aqueous nitric acid and aqueous ammonia reacting: H+(aq) + OH-(aq) \u00e2\u2020\u2019 H2O(l). Identify all […]<\/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-236899","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/236899","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=236899"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/236899\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=236899"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=236899"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=236899"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}