{"id":221957,"date":"2025-05-30T18:24:24","date_gmt":"2025-05-30T18:24:24","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=221957"},"modified":"2025-05-30T18:24:27","modified_gmt":"2025-05-30T18:24:27","slug":"ration-of-each-of-part-a-sodium-bromide-nabrs-a-strong-electrolyte-express-your-answer-as-a-chemical-equation-including-phases","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/30\/ration-of-each-of-part-a-sodium-bromide-nabrs-a-strong-electrolyte-express-your-answer-as-a-chemical-equation-including-phases\/","title":{"rendered":"Ration of each of Part A sodium bromide, NaBr(s), a strong electrolyte Express your answer as a chemical equation including phases"},"content":{"rendered":"\n

ration of each of Part A sodium bromide, NaBr(s), a strong electrolyte Express your answer as a chemical equation including phases. = AE ? NaBr(s) +H, O(1)+Na+ (aq) + Br- (aq) You have already submitted this answer. Enter a new answer No credit lost. Try again Submit Previous Answers Request Answer Part B lactic acid, HC,H,O,(s), a woak electrolyte Express your answer as a chemical equation including phases. Submit Request Answer – Part dextrose(D-glucose), C6H1206(s), a nonelectrolyte Express your answer as a chemical equation including phases. Submit Request Answer Provide Feedback<\/p>\n\n\n\n

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

Here are the correct chemical equations for the dissolution of each compound, followed by a detailed explanation.<\/p>\n\n\n\n

\n\n\n\n

Part A: Sodium bromide (NaBr), a strong electrolyte<\/strong><\/h3>\n\n\n\n

Chemical Equation:<\/strong> NaBr(s)\u2192Na+(aq)+Br\u2212(aq)\\text{NaBr(s)} \\rightarrow \\text{Na}^+(aq) + \\text{Br}^-(aq)<\/p>\n\n\n\n

Explanation:<\/strong>
Sodium bromide is an ionic compound<\/strong> composed of sodium ions (Na\u207a) and bromide ions (Br\u207b). It is classified as a strong electrolyte<\/strong>, which means it completely dissociates into its ions<\/strong> when dissolved in water. The process of dissociation doesn’t involve a reversible reaction; all the NaBr units separate into free-moving ions in the aqueous solution. This is why NaBr is good at conducting electricity in solution\u2014it provides a high concentration of ions. The water (H\u2082O) isn’t explicitly included in the reaction equation as a reactant because it’s the medium, not a reactant, but it facilitates the dissociation.<\/p>\n\n\n\n

\n\n\n\n

Part B: Lactic acid (HC\u2083H\u2085O\u2083), a weak electrolyte<\/strong><\/h3>\n\n\n\n

Chemical Equation:<\/strong> HC3H5O3(s)\u21ccH+(aq)+C3H5O3\u2212(aq)\\text{HC}_3\\text{H}_5\\text{O}_3(s) \\rightleftharpoons \\text{H}^+(aq) + \\text{C}_3\\text{H}_5\\text{O}_3^-(aq)<\/p>\n\n\n\n

Explanation:<\/strong>
Lactic acid is a weak electrolyte<\/strong>, meaning it only partially ionizes<\/strong> in aqueous solution. The equation shows a reversible reaction<\/strong> using a double arrow (\u21cc), indicating that an equilibrium is established between the undissociated lactic acid and its ions. Only a small fraction of lactic acid molecules donate protons (H\u207a) to form lactate ions (C\u2083H\u2085O\u2083\u207b), so the concentration of free ions in solution is relatively low. This incomplete ionization is why weak electrolytes conduct electricity poorly compared to strong electrolytes.<\/p>\n\n\n\n

\n\n\n\n

Part C: Dextrose (D-glucose, C\u2086H\u2081\u2082O\u2086), a nonelectrolyte<\/strong><\/h3>\n\n\n\n

Chemical Equation:<\/strong> C6H12O6(s)\u2192C6H12O6(aq)\\text{C}_6\\text{H}_{12}\\text{O}_6(s) \\rightarrow \\text{C}_6\\text{H}_{12}\\text{O}_6(aq)<\/p>\n\n\n\n

Explanation:<\/strong>
Dextrose (or glucose) is a nonelectrolyte<\/strong>, which means it dissolves in water without ionizing<\/strong>. The solid sugar simply dissolves as intact, neutral molecules, so it does not produce ions<\/strong> in solution. As a result, glucose solutions do not conduct electricity<\/strong>. In the chemical equation, the phase changes from solid (s) to aqueous (aq), indicating it has dissolved, but no chemical reaction has occurred\u2014only a physical process. The molecules remain unchanged, and water simply acts as a solvent.<\/p>\n\n\n\n

\n\n\n\n

Summary Table<\/h3>\n\n\n\n
Substance<\/th>Type of Electrolyte<\/th>Chemical Equation<\/th><\/tr><\/thead>
NaBr<\/strong><\/td>Strong electrolyte<\/td>NaBr(s) \u2192 Na\u207a(aq) + Br\u207b(aq)<\/td><\/tr>
HC\u2083H\u2085O\u2083<\/strong><\/td>Weak electrolyte<\/td>HC\u2083H\u2085O\u2083(s) \u21cc H\u207a(aq) + C\u2083H\u2085O\u2083\u207b(aq)<\/td><\/tr>
C\u2086H\u2081\u2082O\u2086<\/strong><\/td>Nonelectrolyte<\/td>C\u2086H\u2081\u2082O\u2086(s) \u2192 C\u2086H\u2081\u2082O\u2086(aq)<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

These equations demonstrate how the nature of the solute (ionic, molecular, strong\/weak acid\/base) determines the type of dissolution or ionization process in water.<\/p>\n\n\n\n

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

ration of each of Part A sodium bromide, NaBr(s), a strong electrolyte Express your answer as a chemical equation including phases. = AE ? NaBr(s) +H, O(1)+Na+ (aq) + Br- (aq) You have already submitted this answer. Enter a new answer No credit lost. Try again Submit Previous Answers Request Answer Part B lactic acid, […]<\/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-221957","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/221957","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=221957"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/221957\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=221957"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=221957"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=221957"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}