{"id":198044,"date":"2025-03-08T08:50:11","date_gmt":"2025-03-08T08:50:11","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=198044"},"modified":"2025-03-08T08:50:13","modified_gmt":"2025-03-08T08:50:13","slug":"how-to-make-6m-hcl-20ml-by-hsing-37wt-hcld1-2g-ml-aq-solution","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/08\/how-to-make-6m-hcl-20ml-by-hsing-37wt-hcld1-2g-ml-aq-solution\/","title":{"rendered":"How to make 6M HCl 20ml by hsing 37wt% HCl(d=1.2g\/ml) aq solution"},"content":{"rendered":"\n<p>How to make 6M HCl 20ml by hsing 37wt% HCl(d=1.2g\/ml) aq solution? (The molecular weight of HCl is 36.46g\/mol and consider significant figure) <\/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>To prepare 20 mL of a 6 M hydrochloric acid (HCl) solution from a 37% (w\/w) HCl aqueous solution with a density of 1.2 g\/mL, follow these steps:<\/p>\n\n\n\n<p><strong>1. Calculate the required amount of pure HCl:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Desired concentration: 6 M<\/li>\n\n\n\n<li>Desired volume: 20 mL (0.020 L)<\/li>\n<\/ul>\n\n\n\n<p>Using the formula:<\/p>\n\n\n\n<p>[ \\text{moles of HCl} = \\text{Molarity} \\times \\text{Volume} ]<\/p>\n\n\n\n<p>[ \\text{moles of HCl} = 6\\, \\text{mol\/L} \\times 0.020\\, \\text{L} = 0.12\\, \\text{mol} ]<\/p>\n\n\n\n<p>Now, calculate the mass of HCl needed:<\/p>\n\n\n\n<p>[ \\text{mass of HCl} = \\text{moles} \\times \\text{molecular weight} ]<\/p>\n\n\n\n<p>[ \\text{mass of HCl} = 0.12\\, \\text{mol} \\times 36.46\\, \\text{g\/mol} = 4.375\\, \\text{g} ]<\/p>\n\n\n\n<p><strong>2. Determine the volume of the 37% HCl solution required:<\/strong><\/p>\n\n\n\n<p>First, calculate the mass of HCl per milliliter of the 37% solution:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Density of 37% HCl solution: 1.2 g\/mL<\/li>\n\n\n\n<li>Mass percent of HCl: 37%<\/li>\n<\/ul>\n\n\n\n<p>Mass of HCl per mL:<\/p>\n\n\n\n<p>[ \\text{mass of HCl per mL} = 1.2\\, \\text{g\/mL} \\times 0.37 = 0.444\\, \\text{g\/mL} ]<\/p>\n\n\n\n<p>Now, calculate the volume needed to obtain 4.375 g of HCl:<\/p>\n\n\n\n<p>[ \\text{volume required} = \\frac{\\text{mass required}}{\\text{mass per mL}} ]<\/p>\n\n\n\n<p>[ \\text{volume required} = \\frac{4.375\\, \\text{g}}{0.444\\, \\text{g\/mL}} \\approx 9.85\\, \\text{mL} ]<\/p>\n\n\n\n<p><strong>3. Prepare the solution:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Measure approximately 9.85 mL of the 37% HCl solution using a graduated cylinder.<\/li>\n\n\n\n<li>Transfer this volume to a 20 mL volumetric flask.<\/li>\n\n\n\n<li>Carefully add distilled water to the flask until the total volume reaches the 20 mL mark.<\/li>\n\n\n\n<li>Mix thoroughly to ensure a homogeneous solution.<\/li>\n<\/ul>\n\n\n\n<p><strong>Safety Precautions:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Always add acid to water, not the reverse, to prevent exothermic splashing.<\/li>\n\n\n\n<li>Wear appropriate personal protective equipment (PPE), including gloves, safety goggles, and a lab coat.<\/li>\n\n\n\n<li>Perform the dilution in a well-ventilated area, preferably under a fume hood, to avoid inhaling fumes.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>How to make 6M HCl 20ml by hsing 37wt% HCl(d=1.2g\/ml) aq solution? (The molecular weight of HCl is 36.46g\/mol and consider significant figure) The correct answer and explanation is : To prepare 20 mL of a 6 M hydrochloric acid (HCl) solution from a 37% (w\/w) HCl aqueous solution with a density of 1.2 g\/mL, [&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-198044","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198044","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=198044"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198044\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=198044"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=198044"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=198044"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}