{"id":185120,"date":"2025-01-22T06:28:21","date_gmt":"2025-01-22T06:28:21","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=185120"},"modified":"2025-01-22T06:28:24","modified_gmt":"2025-01-22T06:28:24","slug":"what-volume-of-18-0-m-sulfuric-acid-must-be-used-to-prepare-15-5-l-of-0-195-m-h2so4","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/22\/what-volume-of-18-0-m-sulfuric-acid-must-be-used-to-prepare-15-5-l-of-0-195-m-h2so4\/","title":{"rendered":"What volume of 18.0 M sulfuric acid must be used to prepare 15.5 L of 0.195 M H2SO4"},"content":{"rendered":"\n<p>What volume of 18.0 M sulfuric acid must be used to prepare 15.5 L of 0.195 M H<sub>2<\/sub>SO<sub>4<\/sub>?<\/p>\n\n\n\n<p>[A] 0.336 L<\/p>\n\n\n\n<p>[B] 92.3 mL<\/p>\n\n\n\n<p>[C] 168 mL<\/p>\n\n\n\n<p>[D] 226 mL<\/p>\n\n\n\n<p>[E] none of these<\/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 determine the volume of 18.0 M sulfuric acid (H\u2082SO\u2084) required to prepare 15.5 L of 0.195 M H\u2082SO\u2084, we use the <strong>dilution equation<\/strong>:<\/p>\n\n\n\n<p>[<br>M_1 V_1 = M_2 V_2<br>]<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( M_1 ) = initial concentration = 18.0 M<\/li>\n\n\n\n<li>( V_1 ) = volume of the concentrated acid (what we\u2019re solving for)<\/li>\n\n\n\n<li>( M_2 ) = final concentration = 0.195 M<\/li>\n\n\n\n<li>( V_2 ) = final volume = 15.5 L<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Rearrange the equation for ( V_1 ):<\/h3>\n\n\n\n<p>[<br>V_1 = \\frac{M_2 V_2}{M_1}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Plug in the values:<\/h3>\n\n\n\n<p>[<br>V_1 = \\frac{(0.195)(15.5)}{18.0}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Perform the calculations:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li>Multiply ( M_2 ) and ( V_2 ):<br>[<br>0.195 \\times 15.5 = 3.0225<br>]<\/li>\n\n\n\n<li>Divide by ( M_1 ):<br>[<br>\\frac{3.0225}{18.0} \\approx 0.168 \\, \\text{L}<br>]<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\">Step 4: Convert to mL (optional):<\/h3>\n\n\n\n<p>Since ( 1 \\, \\text{L} = 1000 \\, \\text{mL} ), we convert:<br>[<br>0.168 \\, \\text{L} \\times 1000 = 168 \\, \\text{mL}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Final Answer:<\/h3>\n\n\n\n<p>The volume of 18.0 M H\u2082SO\u2084 needed is <strong>168 mL<\/strong>, which corresponds to option <strong>[C]<\/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>This problem involves diluting a concentrated acid to achieve a lower concentration. The dilution equation ensures the number of moles of solute remains constant before and after dilution. The concentrated sulfuric acid is very strong, so only a small volume (168 mL) is required to prepare the 15.5 L solution. Always remember to add acid to water for safety.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>What volume of 18.0 M sulfuric acid must be used to prepare 15.5 L of 0.195 M H2SO4? [A] 0.336 L [B] 92.3 mL [C] 168 mL [D] 226 mL [E] none of these The Correct Answer and Explanation is : To determine the volume of 18.0 M sulfuric acid (H\u2082SO\u2084) required to prepare 15.5 [&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-185120","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185120","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=185120"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185120\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=185120"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=185120"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=185120"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}