{"id":227562,"date":"2025-06-06T08:03:50","date_gmt":"2025-06-06T08:03:50","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=227562"},"modified":"2025-06-06T08:03:52","modified_gmt":"2025-06-06T08:03:52","slug":"potassium-iodide-ki-has-a-molecular-mass-of-166-grams-mole","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/06\/potassium-iodide-ki-has-a-molecular-mass-of-166-grams-mole\/","title":{"rendered":"Potassium iodide (KI) has a molecular mass of 166 grams \/ (mole) ."},"content":{"rendered":"\n<p>Potassium iodide (KI) has a molecular mass of 166 grams \/ (mole) . What is the molarity of a KI solution with a concentration of 83 grams\/liter<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To find the <strong>molarity<\/strong> of a potassium iodide (KI) solution with a concentration of <strong>83 grams per liter<\/strong>, we use the following formula:Molarity&nbsp;(M)=mass&nbsp;of&nbsp;solute&nbsp;(g)molar&nbsp;mass&nbsp;(g\/mol)\u00d7volume&nbsp;of&nbsp;solution&nbsp;(L)\\text{Molarity (M)} = \\frac{\\text{mass of solute (g)}}{\\text{molar mass (g\/mol)} \\times \\text{volume of solution (L)}}Molarity&nbsp;(M)=molar&nbsp;mass&nbsp;(g\/mol)\u00d7volume&nbsp;of&nbsp;solution&nbsp;(L)mass&nbsp;of&nbsp;solute&nbsp;(g)\u200b<\/p>\n\n\n\n<p>Given:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Mass of KI = 83 g<\/li>\n\n\n\n<li>Molar mass of KI = 166 g\/mol<\/li>\n\n\n\n<li>Volume of solution = 1 L (since the concentration is per liter)<\/li>\n<\/ul>\n\n\n\n<p>Now, calculate the molarity:Molarity=83&nbsp;g166&nbsp;g\/mol\u00d71&nbsp;L=0.5&nbsp;mol\/L\\text{Molarity} = \\frac{83 \\text{ g}}{166 \\text{ g\/mol} \\times 1 \\text{ L}} = 0.5 \\text{ mol\/L}Molarity=166&nbsp;g\/mol\u00d71&nbsp;L83&nbsp;g\u200b=0.5&nbsp;mol\/L<\/p>\n\n\n\n<p><strong>Answer: The molarity of the KI solution is 0.5 M.<\/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<p>Molarity is one of the most common ways to express the concentration of a solution in chemistry. It is defined as the number of <strong>moles of solute per liter of solution<\/strong>. The formula is straightforward:M=nVM = \\frac{n}{V}M=Vn\u200b<\/p>\n\n\n\n<p>Where <em>n<\/em> is the number of moles of solute, and <em>V<\/em> is the volume of the solution in liters.<\/p>\n\n\n\n<p>To find the number of moles, we divide the <strong>mass of the solute<\/strong> by its <strong>molar mass<\/strong>. Potassium iodide (KI) has a molar mass of 166 g\/mol, meaning 1 mole of KI weighs 166 grams. If we have 83 grams of KI, we divide this by 166 g\/mol to find the number of moles:83166=0.5&nbsp;moles\\frac{83}{166} = 0.5 \\text{ moles}16683\u200b=0.5&nbsp;moles<\/p>\n\n\n\n<p>Since the solution has 83 grams of KI per 1 liter of solution, and we\u2019ve determined that 83 grams equals 0.5 moles, the molarity is:0.5&nbsp;moles&nbsp;per&nbsp;liter=0.5&nbsp;M0.5 \\text{ moles per liter} = 0.5 \\text{ M}0.5&nbsp;moles&nbsp;per&nbsp;liter=0.5&nbsp;M<\/p>\n\n\n\n<p>This tells us that every liter of this KI solution contains half a mole of KI. Understanding molarity is essential in chemical reactions and solution chemistry, as it helps chemists know how much of a substance is available for a reaction. Whether preparing buffers, titrations, or medications, accurately calculating molarity ensures predictable results.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner9-104.jpeg\" alt=\"\" class=\"wp-image-227563\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Potassium iodide (KI) has a molecular mass of 166 grams \/ (mole) . What is the molarity of a KI solution with a concentration of 83 grams\/liter The Correct Answer and Explanation is: To find the molarity of a potassium iodide (KI) solution with a concentration of 83 grams per liter, we use the following [&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-227562","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/227562","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=227562"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/227562\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=227562"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=227562"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=227562"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}