{"id":191550,"date":"2025-02-15T08:13:24","date_gmt":"2025-02-15T08:13:24","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=191550"},"modified":"2025-02-15T08:13:27","modified_gmt":"2025-02-15T08:13:27","slug":"write-the-formula-for-copper-ii-phosphate","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/15\/write-the-formula-for-copper-ii-phosphate\/","title":{"rendered":"Write the formula for copper (II) phosphate"},"content":{"rendered":"\n<p>a. Write the formula for copper (II) phosphate<\/p>\n\n\n\n<p>b. Calculate the molecular weight for copper (II) phosphate<\/p>\n\n\n\n<p>c. Calculate the number of moles of copper (II) phosphate in 129.4 g of copper (II) phosphate.<\/p>\n\n\n\n<p>d. Calculate the total number of atoms of phosphorus in 129.4 g of copper (II) phosphate.<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">a. Formula for Copper (II) Phosphate<\/h3>\n\n\n\n<p>The formula for copper (II) phosphate is <strong>Cu\u2083(PO\u2084)\u2082<\/strong>. This is based on copper&#8217;s +2 oxidation state (Cu\u00b2\u207a) and phosphate&#8217;s -3 charge (PO\u2084\u00b3\u207b). To balance the charges, you need 3 copper ions for every 2 phosphate ions, resulting in the formula Cu\u2083(PO\u2084)\u2082.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">b. Molecular Weight of Copper (II) Phosphate<\/h3>\n\n\n\n<p>To calculate the molecular weight of copper (II) phosphate (Cu\u2083(PO\u2084)\u2082), we sum the atomic weights of each element in the formula:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Atomic weight of Copper (Cu) = 63.55 g\/mol<\/li>\n\n\n\n<li>Atomic weight of Phosphorus (P) = 30.97 g\/mol<\/li>\n\n\n\n<li>Atomic weight of Oxygen (O) = 16.00 g\/mol<\/li>\n<\/ul>\n\n\n\n<p>The molecular weight is calculated as:<\/p>\n\n\n\n<p>[<br>\\text{Molar Mass} = 3 \\times 63.55 \\, \\text{g\/mol} + 2 \\times (30.97 \\, \\text{g\/mol} + 4 \\times 16.00 \\, \\text{g\/mol})<br>]<\/p>\n\n\n\n<p>[<br>\\text{Molar Mass} = 3 \\times 63.55 + 2 \\times (30.97 + 64.00)<br>]<\/p>\n\n\n\n<p>[<br>\\text{Molar Mass} = 190.65 + 2 \\times 94.97<br>]<\/p>\n\n\n\n<p>[<br>\\text{Molar Mass} = 190.65 + 189.94 = 380.59 \\, \\text{g\/mol}<br>]<\/p>\n\n\n\n<p>Thus, the molecular weight of Cu\u2083(PO\u2084)\u2082 is <strong>380.59 g\/mol<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">c. Number of Moles of Copper (II) Phosphate in 129.4 g<\/h3>\n\n\n\n<p>To calculate the number of moles of Cu\u2083(PO\u2084)\u2082 in 129.4 g, use the formula:<\/p>\n\n\n\n<p>[<br>\\text{Moles} = \\frac{\\text{Mass}}{\\text{Molar Mass}}<br>]<\/p>\n\n\n\n<p>[<br>\\text{Moles} = \\frac{129.4 \\, \\text{g}}{380.59 \\, \\text{g\/mol}} = 0.340 \\, \\text{mol}<br>]<\/p>\n\n\n\n<p>So, the number of moles of copper (II) phosphate in 129.4 g is <strong>0.340 mol<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">d. Total Number of Atoms of Phosphorus<\/h3>\n\n\n\n<p>To calculate the total number of atoms of phosphorus in 129.4 g of copper (II) phosphate:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li>First, we find the number of moles of phosphorus atoms in 0.340 moles of Cu\u2083(PO\u2084)\u2082. Since each formula unit of Cu\u2083(PO\u2084)\u2082 contains 2 phosphorus atoms, the moles of phosphorus atoms will be:<\/li>\n<\/ol>\n\n\n\n<p>[<br>\\text{Moles of P} = 0.340 \\, \\text{mol} \\times 2 = 0.680 \\, \\text{mol of P}<br>]<\/p>\n\n\n\n<ol start=\"2\" class=\"wp-block-list\">\n<li>Now, we use Avogadro&#8217;s number (6.022 \u00d7 10\u00b2\u00b3 atoms\/mol) to find the total number of phosphorus atoms:<\/li>\n<\/ol>\n\n\n\n<p>[<br>\\text{Atoms of P} = 0.680 \\, \\text{mol of P} \\times 6.022 \\times 10^{23} \\, \\text{atoms\/mol}<br>]<\/p>\n\n\n\n<p>[<br>\\text{Atoms of P} = 4.09 \\times 10^{23} \\, \\text{atoms of P}<br>]<\/p>\n\n\n\n<p>So, the total number of phosphorus atoms in 129.4 g of copper (II) phosphate is <strong>4.09 \u00d7 10\u00b2\u00b3 atoms<\/strong>.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Formula of Copper (II) Phosphate (Cu\u2083(PO\u2084)\u2082)<\/strong>: The compound copper (II) phosphate consists of copper ions in the +2 oxidation state (Cu\u00b2\u207a) and phosphate ions (PO\u2084\u00b3\u207b). To balance the charges, 3 copper ions pair with 2 phosphate ions, yielding Cu\u2083(PO\u2084)\u2082.<\/li>\n\n\n\n<li><strong>Molecular Weight<\/strong>: The molecular weight is the sum of the atomic masses of all the elements in the compound. Copper, phosphorus, and oxygen contribute to the molecular weight of Cu\u2083(PO\u2084)\u2082, and the calculation yields 380.59 g\/mol.<\/li>\n\n\n\n<li><strong>Moles of Copper (II) Phosphate<\/strong>: The number of moles of Cu\u2083(PO\u2084)\u2082 in a given mass is calculated by dividing the mass by the molecular weight. For 129.4 g of Cu\u2083(PO\u2084)\u2082, the number of moles is 0.340 mol.<\/li>\n\n\n\n<li><strong>Atoms of Phosphorus<\/strong>: Since each formula unit of Cu\u2083(PO\u2084)\u2082 contains 2 phosphorus atoms, the total number of moles of phosphorus atoms is double the moles of the compound. Then, multiplying by Avogadro&#8217;s number gives the total number of phosphorus atoms as 4.09 \u00d7 10\u00b2\u00b3.<\/li>\n<\/ol>\n\n\n\n<p>I will now generate a visual representation of these calculations.<\/p>\n\n\n\n<p>Here is a visual representation of the steps involved in calculating the copper (II) phosphate properties, including the formula, molecular weight, moles, and atoms of phosphorus. Each step is associated with the corresponding calculation or value derived.<\/p>\n\n\n\n<figure class=\"wp-block-image size-large\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/02\/image-588-1024x635.png\" alt=\"\" class=\"wp-image-191551\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>a. Write the formula for copper (II) phosphate b. Calculate the molecular weight for copper (II) phosphate c. Calculate the number of moles of copper (II) phosphate in 129.4 g of copper (II) phosphate. d. Calculate the total number of atoms of phosphorus in 129.4 g of copper (II) phosphate. The Correct Answer and Explanation [&hellip;]<\/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-191550","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191550","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=191550"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191550\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=191550"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=191550"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=191550"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}