{"id":154888,"date":"2024-10-15T15:26:34","date_gmt":"2024-10-15T15:26:34","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=154888"},"modified":"2024-10-15T15:26:36","modified_gmt":"2024-10-15T15:26:36","slug":"what-m-is-the-molar-mass-of-the-compound-silver-chloride","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/10\/15\/what-m-is-the-molar-mass-of-the-compound-silver-chloride\/","title":{"rendered":"What m is the molar mass of the compound silver chloride"},"content":{"rendered":"\n<p>What m is the molar mass of the compound silver chloride?<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>The molar mass of silver chloride (AgCl) is approximately <strong>143.32 g\/mol<\/strong>. This value is calculated by adding the molar masses of its constituent elements, silver (Ag) and chlorine (Cl).<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Calculation of Molar Mass:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Molar Mass of Silver (Ag)<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The atomic mass of silver is approximately <strong>107.87 g\/mol<\/strong>. This value is derived from the periodic table and reflects the weighted average of the isotopes of silver found in nature.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Molar Mass of Chlorine (Cl)<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The atomic mass of chlorine is about <strong>35.45 g\/mol<\/strong>. Chlorine exists primarily as two isotopes: Cl-35 and Cl-37, with Cl-35 being the more abundant isotope. The molar mass accounts for this isotopic distribution.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Adding the Molar Masses<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>To find the molar mass of silver chloride, we sum the molar masses of silver and chlorine:<br>[<br>\\text{Molar Mass of AgCl} = \\text{Molar Mass of Ag} + \\text{Molar Mass of Cl}<br>]<br>[<br>\\text{Molar Mass of AgCl} = 107.87 \\, \\text{g\/mol} + 35.45 \\, \\text{g\/mol} = 143.32 \\, \\text{g\/mol}<br>]<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Importance of Molar Mass:<\/h3>\n\n\n\n<p>The molar mass is crucial in chemistry for several reasons:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Stoichiometry<\/strong>: It allows chemists to convert between grams and moles when performing calculations in chemical reactions. Knowing the molar mass of silver chloride enables accurate preparation of solutions and mixtures in laboratories.<\/li>\n\n\n\n<li><strong>Quantitative Analysis<\/strong>: In quantitative analysis, determining the concentration of silver ions in a solution involves using molar mass to convert between the mass of silver chloride and the number of moles present.<\/li>\n\n\n\n<li><strong>Reactions and Precipitation<\/strong>: Silver chloride is used in various applications, including photography and as a precursor in the synthesis of other silver compounds. Understanding its molar mass helps predict how it will react in different chemical scenarios.<\/li>\n<\/ul>\n\n\n\n<p>In summary, the molar mass of silver chloride (143.32 g\/mol) is calculated by summing the atomic masses of silver and chlorine, which plays a critical role in various chemical applications and calculations.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>What m is the molar mass of the compound silver chloride? The Correct Answer and Explanation is: The molar mass of silver chloride (AgCl) is approximately 143.32 g\/mol. This value is calculated by adding the molar masses of its constituent elements, silver (Ag) and chlorine (Cl). Calculation of Molar Mass: Importance of Molar Mass: The [&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-154888","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/154888","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=154888"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/154888\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=154888"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=154888"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=154888"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}