. A 5.0 g sample of calcium nitrate (Ca(NO3)2, M = 164 ) contaminated with silica (SiO\u2082, M = 60.1 ) is found to contain 1.0 g calcium. What is the mass percent purity of calcium nitrate in the sample?
a. 20%
b. 24%
c. 73%
d. 82%<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n The problem asks to find the mass percent purity of calcium nitrate (Ca(NO\u2083)\u2082) in a sample that contains both calcium nitrate and silica (SiO\u2082), where the total sample mass is 5.0 g, and the mass of calcium in the sample is 1.0 g.<\/p>\n\n\n\n From the chemical formula of calcium nitrate (Ca(NO\u2083)\u2082), we know that one mole of Ca(NO\u2083)\u2082 contains one mole of calcium (Ca). The molar mass of Ca(NO\u2083)\u2082 is 164 g\/mol, and the molar mass of calcium is 40.1 g\/mol.<\/p>\n\n\n\n Thus, the mass of calcium in one mole of Ca(NO\u2083)\u2082 is 40.1 g.<\/p>\n\n\n\n Using the molar mass of calcium nitrate and the molar mass of calcium, we can calculate the amount of calcium nitrate that contains 1.0 g of calcium.<\/p>\n\n\n\n [ [ [ Now, we can calculate the mass percent purity of calcium nitrate in the sample:<\/p>\n\n\n\n [ [ The mass percent purity of calcium nitrate in the sample is approximately 82%<\/strong>, so the correct answer is d. 82%<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":" . A 5.0 g sample of calcium nitrate (Ca(NO3)2, M = 164 ) contaminated with silica (SiO\u2082, M = 60.1 ) is found to contain 1.0 g calcium. What is the mass percent purity of calcium nitrate in the sample?a. 20%b. 24%c. 73%d. 82% The Correct Answer and Explanation is : The problem asks to […]<\/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-187034","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187034","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=187034"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187034\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187034"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187034"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187034"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 1: Determine the amount of calcium in calcium nitrate<\/h3>\n\n\n\n
Step 2: Calculate the amount of calcium nitrate corresponding to 1.0 g of calcium<\/h3>\n\n\n\n
\\text{mass of Ca(NO\u2083)\u2082} = \\frac{\\text{mass of Ca}}{\\text{mass of Ca in Ca(NO\u2083)\u2082}} \\times \\text{molar mass of Ca(NO\u2083)\u2082}
]<\/p>\n\n\n\n
\\text{mass of Ca(NO\u2083)\u2082} = \\frac{1.0 \\, \\text{g}}{40.1 \\, \\text{g\/mol}} \\times 164 \\, \\text{g\/mol}
]<\/p>\n\n\n\n
\\text{mass of Ca(NO\u2083)\u2082} = 4.09 \\, \\text{g}
]<\/p>\n\n\n\nStep 3: Calculate the mass percent purity of calcium nitrate<\/h3>\n\n\n\n
\\text{mass percent purity} = \\frac{\\text{mass of Ca(NO\u2083)\u2082}}{\\text{total sample mass}} \\times 100
]<\/p>\n\n\n\n
\\text{mass percent purity} = \\frac{4.09 \\, \\text{g}}{5.0 \\, \\text{g}} \\times 100 = 81.8\\%
]<\/p>\n\n\n\nConclusion<\/h3>\n\n\n\n