Find the molar mass of alum (KAl(SO\u2084)\u2082 \u00b7 12H\u2082O).<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n The molar mass of alum, potassium aluminum sulfate dodecahydrate, KAl(SO\u2084)\u2082 \u00b7 12H\u2082O, can be calculated by summing the atomic masses of all the atoms in its formula.<\/p>\n\n\n\n Now, adding everything together:<\/p>\n\n\n\n Total molar mass of KAl(SO\u2084)\u2082 \u00b7 12H\u2082O = 39.10 + 26.98 + 64.14 + 128.00 + 216.19 = 474.41 g\/mol<\/strong><\/p>\n\n\n\n Alum, KAl(SO\u2084)\u2082 \u00b7 12H\u2082O, is a double sulfate salt containing potassium (K), aluminum (Al), and two sulfate (SO\u2084\u00b2\u207b) ions along with 12 water molecules (H\u2082O) of hydration. Each component contributes to the overall mass of the compound. Potassium and aluminum are the metals that combine with the sulfate ions to form the main framework of the alum crystal. Sulfate ions (SO\u2084\u00b2\u207b) contribute both sulfur and oxygen atoms. The water molecules (12 H\u2082O) are part of the structure, hydrating the ions and helping maintain the crystalline form.<\/p>\n\n\n\n The molar mass is important because it allows chemists to calculate the number of moles of the substance in a given mass, which is crucial for stoichiometric calculations in reactions involving alum, such as in water purification, dyeing, or as an astringent in various applications.<\/p>\n","protected":false},"excerpt":{"rendered":" Find the molar mass of alum (KAl(SO\u2084)\u2082 \u00b7 12H\u2082O). The Correct Answer and Explanation is : The molar mass of alum, potassium aluminum sulfate dodecahydrate, KAl(SO\u2084)\u2082 \u00b7 12H\u2082O, can be calculated by summing the atomic masses of all the atoms in its formula. Step-by-step Calculation: Now, adding everything together: Total molar mass of KAl(SO\u2084)\u2082 \u00b7 […]<\/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-147922","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/147922","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=147922"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/147922\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=147922"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=147922"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=147922"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step-by-step Calculation:<\/h3>\n\n\n\n
\n
Atomic mass of K = 39.10 g\/mol<\/li>\n\n\n\n
Atomic mass of Al = 26.98 g\/mol<\/li>\n\n\n\n
Atomic mass of S = 32.07 g\/mol
Total mass of sulfur = 2 \u00d7 32.07 = 64.14 g\/mol<\/li>\n\n\n\n
Atomic mass of O = 16.00 g\/mol
Total mass of oxygen in SO\u2084\u00b2\u207b = 8 \u00d7 16.00 = 128.00 g\/mol<\/li>\n\n\n\n
Molecular mass of water = 2 \u00d7 1.008 (H) + 16.00 (O) = 18.016 g\/mol
Total mass of 12 H\u2082O = 12 \u00d7 18.016 = 216.19 g\/mol<\/li>\n<\/ol>\n\n\n\n\n
Explanation:<\/h3>\n\n\n\n