{"id":198499,"date":"2025-03-10T06:06:20","date_gmt":"2025-03-10T06:06:20","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=198499"},"modified":"2025-03-10T06:06:22","modified_gmt":"2025-03-10T06:06:22","slug":"what-mass-of-potassium-hydroxide-koh-molar-mass-56-1-g-moll-is-needed-to-make-250-0-ml-of-a-0-125m-koh-solution","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/10\/what-mass-of-potassium-hydroxide-koh-molar-mass-56-1-g-moll-is-needed-to-make-250-0-ml-of-a-0-125m-koh-solution\/","title":{"rendered":"What mass of potassium hydroxide (KOH, molar mass = 56.1 g moll) is needed to make 250.0 mL of a 0.125M KOH solution"},"content":{"rendered":"\n<p>What mass of potassium hydroxide (KOH, molar mass = 56.1 g moll) is needed to make 250.0 mL of a 0.125M KOH solution? 0.0313g 1.75g 3.13g 3.51g<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>The correct answer is <strong>1.75 g<\/strong> of KOH.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>To determine the mass of potassium hydroxide (KOH) needed to prepare 250.0 mL of a <strong>0.125 M<\/strong> solution, we follow these steps:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Understand Molarity Formula:<\/strong> Molarity (M) is defined as: M=moles\u00a0of\u00a0soluteliters\u00a0of\u00a0solutionM = \\frac{\\text{moles of solute}}{\\text{liters of solution}} Rearranging the formula to solve for moles of KOH: moles\u00a0of\u00a0KOH=M\u00d7liters\u00a0of\u00a0solution\\text{moles of KOH} = M \\times \\text{liters of solution}<\/li>\n\n\n\n<li><strong>Convert Volume to Liters:<\/strong> The given volume is 250.0 mL, which is converted to liters: 250.0\u00a0mL\u00d71\u00a0L1000\u00a0mL=0.2500\u00a0L250.0 \\text{ mL} \\times \\frac{1 \\text{ L}}{1000 \\text{ mL}} = 0.2500 \\text{ L}<\/li>\n\n\n\n<li><strong>Calculate Moles of KOH:<\/strong> Using the molarity equation: moles\u00a0of\u00a0KOH=0.125\u00a0M\u00d70.2500\u00a0L=0.03125\u00a0moles\\text{moles of KOH} = 0.125 \\text{ M} \\times 0.2500 \\text{ L} = 0.03125 \\text{ moles}<\/li>\n\n\n\n<li><strong>Convert Moles to Grams:<\/strong> The molar mass of KOH is <strong>56.1 g\/mol<\/strong>, so we calculate: mass\u00a0of\u00a0KOH=0.03125\u00a0moles\u00d756.1\u00a0g\/mol=1.75\u00a0g\\text{mass of KOH} = 0.03125 \\text{ moles} \\times 56.1 \\text{ g\/mol} = 1.75 \\text{ g}<\/li>\n<\/ol>\n\n\n\n<p>Thus, <strong>1.75 g<\/strong> of KOH is needed.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/03\/image-705.png\" alt=\"\" class=\"wp-image-198500\"\/><\/figure>\n\n\n\n<p>The image above visually presents the step-by-step calculation for determining the mass of KOH needed to prepare 250.0 mL of a 0.125 M solution. The correct answer is <strong>1.75 g<\/strong> of KOH.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>What mass of potassium hydroxide (KOH, molar mass = 56.1 g moll) is needed to make 250.0 mL of a 0.125M KOH solution? 0.0313g 1.75g 3.13g 3.51g The correct answer and explanation is : The correct answer is 1.75 g of KOH. Explanation: To determine the mass of potassium hydroxide (KOH) needed to prepare 250.0 [&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-198499","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198499","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=198499"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198499\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=198499"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=198499"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=198499"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}