What is the molar mass of AgF. 51.9g\/mol 198.8g\/mol 126.87g\/mol 99.7g\/mol<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n To determine the molar mass of silver fluoride (AgF), we need to add the molar masses of its constituent elements: silver (Ag) and fluorine (F).<\/p>\n\n\n\n In summary, the correct molar mass of silver fluoride (AgF) is 126.87 g\/mol<\/strong>, derived from the atomic masses of silver and fluorine. This knowledge is fundamental in performing accurate calculations in both laboratory and industrial settings.<\/p>\n","protected":false},"excerpt":{"rendered":" What is the molar mass of AgF. 51.9g\/mol 198.8g\/mol 126.87g\/mol 99.7g\/mol The Correct Answer and Explanation is: To determine the molar mass of silver fluoride (AgF), we need to add the molar masses of its constituent elements: silver (Ag) and fluorine (F). In summary, the correct molar mass of silver fluoride (AgF) is 126.87 g\/mol, […]<\/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-156284","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/156284","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=156284"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/156284\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=156284"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=156284"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=156284"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}\n
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The formula for silver fluoride consists of one silver atom and one fluorine atom. Therefore, the molar mass of AgF is calculated as follows: [
\\text{Molar Mass of AgF} = \\text{Molar Mass of Ag} + \\text{Molar Mass of F}
]
[
\\text{Molar Mass of AgF} = 107.87 \\, \\text{g\/mol} + 19.00 \\, \\text{g\/mol} = 126.87 \\, \\text{g\/mol}
]<\/li>\n\n\n\n
Now, let’s review the provided options:<\/li>\n<\/ol>\n\n\n\n\n
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The molar mass is critical in various chemical calculations, particularly in stoichiometry, where it allows for the conversion between moles and grams of substances. It is used to determine how much of a reactant is needed in a chemical reaction or to predict the mass of products formed. In the case of silver fluoride, understanding its molar mass is essential for applications in chemistry, including its use in various synthesis reactions, dental applications, and as a reagent in analytical chemistry.<\/li>\n<\/ol>\n\n\n\n