Balanced Complete Ionic Equation:<\/strong> 3Na+(aq)+PO43\u2212(aq)+3Cu2+(aq)+6Cl\u2212(aq)\u2192Cu3(PO4)2(s)+6Na+(aq)+6Cl\u2212(aq)3\\text{Na}^+(aq) + \\text{PO}_4^{3-}(aq) + 3\\text{Cu}^{2+}(aq) + 6\\text{Cl}^-(aq) \\rightarrow \\text{Cu}_3(\\text{PO}_4)_2(s) + 6\\text{Na}^+(aq) + 6\\text{Cl}^-(aq)3Na+(aq)+PO43\u2212\u200b(aq)+3Cu2+(aq)+6Cl\u2212(aq)\u2192Cu3\u200b(PO4\u200b)2\u200b(s)+6Na+(aq)+6Cl\u2212(aq)<\/p>\n\n\n\n Textbook-Style Explanation<\/strong><\/p>\n\n\n\n When sodium phosphate (Na3PO4\\text{Na}_3\\text{PO}_4Na3\u200bPO4\u200b) and copper(II) chloride (CuCl2\\text{CuCl}_2CuCl2\u200b) are mixed in aqueous solution, a double displacement reaction occurs. This reaction involves the exchange of ions between two soluble ionic compounds, leading to the formation of a precipitate, copper(II) phosphate (Cu3(PO4)2\\text{Cu}_3(\\text{PO}_4)_2Cu3\u200b(PO4\u200b)2\u200b), and sodium chloride (NaCl\\text{NaCl}NaCl), which remains dissolved in water.<\/p>\n\n\n\n First, we write the balanced molecular equation: 2Na3PO4(aq)+3CuCl2(aq)\u2192Cu3(PO4)2(s)+6NaCl(aq)2\\text{Na}_3\\text{PO}_4(aq) + 3\\text{CuCl}_2(aq) \\rightarrow \\text{Cu}_3(\\text{PO}_4)_2(s) + 6\\text{NaCl}(aq)2Na3\u200bPO4\u200b(aq)+3CuCl2\u200b(aq)\u2192Cu3\u200b(PO4\u200b)2\u200b(s)+6NaCl(aq)<\/p>\n\n\n\n This shows that 2 moles of sodium phosphate react with 3 moles of copper(II) chloride to produce 1 mole of solid copper(II) phosphate and 6 moles of sodium chloride in solution.<\/p>\n\n\n\n Next, we express the reaction as a complete ionic equation by dissociating all strong electrolytes into their constituent ions: 6Na+(aq)+2PO43\u2212(aq)+3Cu2+(aq)+6Cl\u2212(aq)\u2192Cu3(PO4)2(s)+6Na+(aq)+6Cl\u2212(aq)6\\text{Na}^+(aq) + 2\\text{PO}_4^{3-}(aq) + 3\\text{Cu}^{2+}(aq) + 6\\text{Cl}^-(aq) \\rightarrow \\text{Cu}_3(\\text{PO}_4)_2(s) + 6\\text{Na}^+(aq) + 6\\text{Cl}^-(aq)6Na+(aq)+2PO43\u2212\u200b(aq)+3Cu2+(aq)+6Cl\u2212(aq)\u2192Cu3\u200b(PO4\u200b)2\u200b(s)+6Na+(aq)+6Cl\u2212(aq)<\/p>\n\n\n\n Here, Na3PO4\\text{Na}_3\\text{PO}_4Na3\u200bPO4\u200b and CuCl2\\text{CuCl}_2CuCl2\u200b fully dissociate in water. Copper(II) phosphate, however, is insoluble and precipitates out as a solid. Sodium ions and chloride ions remain in solution as spectator ions.<\/p>\n\n\n\n Finally, if we remove the spectator ions (species that appear unchanged on both sides), we get the net ionic equation: 3Cu2+(aq)+2PO43\u2212(aq)\u2192Cu3(PO4)2(s)3\\text{Cu}^{2+}(aq) + 2\\text{PO}_4^{3-}(aq) \\rightarrow \\text{Cu}_3(\\text{PO}_4)_2(s)3Cu2+(aq)+2PO43\u2212\u200b(aq)\u2192Cu3\u200b(PO4\u200b)2\u200b(s)<\/p>\n\n\n\n This net ionic equation clearly shows the formation of solid copper(II) phosphate from its constituent ions in solution.<\/p>\n\n\n\n Write a balanced complete ionic equation for Na3PO4(aq) + CuCl2(aq) = Cu3(PO4)2(s) + 6NaCl(aq). Express your answer as a chemical equation. Identify all of the phases in your answer The Correct Answer and Explanation is: Balanced Complete Ionic Equation: 3Na+(aq)+PO43\u2212(aq)+3Cu2+(aq)+6Cl\u2212(aq)\u2192Cu3(PO4)2(s)+6Na+(aq)+6Cl\u2212(aq)3\\text{Na}^+(aq) + \\text{PO}_4^{3-}(aq) + 3\\text{Cu}^{2+}(aq) + 6\\text{Cl}^-(aq) \\rightarrow \\text{Cu}_3(\\text{PO}_4)_2(s) + 6\\text{Na}^+(aq) + 6\\text{Cl}^-(aq)3Na+(aq)+PO43\u2212\u200b(aq)+3Cu2+(aq)+6Cl\u2212(aq)\u2192Cu3\u200b(PO4\u200b)2\u200b(s)+6Na+(aq)+6Cl\u2212(aq) Textbook-Style Explanation When […]<\/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-231883","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231883","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=231883"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231883\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=231883"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=231883"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=231883"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
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