Write the net ionic equation for the reaction of citric acid and sodium hydroxide. NG 1 Info Mouse over the picture above to view the 4 components of a reactant or product that are needed to write chemical equations.<\/p>\n\n\n\n
Write the balanced net ionic equation for the reaction between citric acid and sodium hydroxide Mouse over the grey boxes for information on 2 NH4 coefficients, formulas, charges and states of matter. The coefficient and formula are required components – the components of a chemical equation. H + ——- Work Problem<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n [ 1. Understanding the Reactants:<\/strong> [ [ [ Since citric acid has three acidic protons, it reacts with three hydroxide ions (OH\u207b<\/strong>) from sodium hydroxide (NaOH<\/strong>) in a neutralization reaction.<\/p>\n\n\n\n 2. Understanding the Reaction with NaOH:<\/strong> [ Each hydroxide ion neutralizes a hydrogen ion from citric acid:<\/p>\n\n\n\n [ Since citric acid donates three protons, it requires three hydroxide ions for complete neutralization.<\/p>\n\n\n\n 3. Writing the Net Ionic Equation:<\/strong> [ This net ionic equation represents the neutralization of citric acid by sodium hydroxide, forming citrate ions and water.<\/p>\n\n\n\n 4. Summary:<\/strong> Write the net ionic equation for the reaction of citric acid and sodium hydroxide. NG 1 Info Mouse over the picture above to view the 4 components of a reactant or product that are needed to write chemical equations. Write the balanced net ionic equation for the reaction between citric acid and sodium hydroxide Mouse […]<\/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-191021","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191021","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=191021"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191021\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=191021"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=191021"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=191021"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Net Ionic Equation for the Reaction of Citric Acid and Sodium Hydroxide:<\/h3>\n\n\n\n
Balanced Net Ionic Equation:<\/strong><\/h4>\n\n\n\n
\\text{C}_6\\text{H}_5\\text{O}_7^{3-} + 3 \\text{OH}^- \\rightarrow \\text{C}_6\\text{H}_5\\text{O}_7^{3-} + 3 \\text{H}_2\\text{O}
]<\/p>\n\n\n\n
\n\n\n\nExplanation (300 words)<\/strong><\/h3>\n\n\n\n
Citric acid (C\u2086H\u2088O\u2087<\/strong>) is a weak, triprotic acid, meaning it can donate up to three hydrogen ions (H\u207a<\/strong>). It ionizes in water as follows:<\/p>\n\n\n\n
\\text{C}_6\\text{H}_8\\text{O}_7 \\rightleftharpoons \\text{C}_6\\text{H}_7\\text{O}_7^- + H^+
]<\/p>\n\n\n\n
\\text{C}_6\\text{H}_7\\text{O}_7^- \\rightleftharpoons \\text{C}_6\\text{H}_6\\text{O}_7^{2-} + H^+
]<\/p>\n\n\n\n
\\text{C}_6\\text{H}_6\\text{O}_7^{2-} \\rightleftharpoons \\text{C}_6\\text{H}_5\\text{O}_7^{3-} + H^+
]<\/p>\n\n\n\n
Sodium hydroxide is a strong base that completely dissociates in water:<\/p>\n\n\n\n
\\text{NaOH} \\rightarrow \\text{Na}^+ + \\text{OH}^-
]<\/p>\n\n\n\n
\\text{H}^+ + \\text{OH}^- \\rightarrow \\text{H}_2\\text{O}
]<\/p>\n\n\n\n
Since sodium ions (Na\u207a<\/strong>) are spectator ions and do not participate in the actual reaction, we remove them from the full equation, leaving only the reacting species:<\/p>\n\n\n\n
\\text{C}_6\\text{H}_8\\text{O}_7 + 3 \\text{OH}^- \\rightarrow \\text{C}_6\\text{H}_5\\text{O}_7^{3-} + 3 \\text{H}_2\\text{O}
]<\/p>\n\n\n\n
This reaction is a classic acid-base neutralization. The citric acid donates its hydrogen ions, while hydroxide ions neutralize them, forming water. The final product is the citrate ion (C\u2086H\u2085O\u2087\u00b3\u207b<\/strong>) and water molecules, indicating the complete neutralization of citric acid.<\/p>\n","protected":false},"excerpt":{"rendered":"