{"id":235934,"date":"2025-06-15T21:28:53","date_gmt":"2025-06-15T21:28:53","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=235934"},"modified":"2025-06-15T21:28:55","modified_gmt":"2025-06-15T21:28:55","slug":"aqueous-solution-by-mass-of-urea-has-boiling-point","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/15\/aqueous-solution-by-mass-of-urea-has-boiling-point\/","title":{"rendered":"Aqueous solution (by mass) of urea has boiling point"},"content":{"rendered":"\n<p class=\"wp-block-paragraph\"><br>Aqueous solution (by mass) of urea has boiling point<br>. The boiling point of<br>glucose in watar :- &#8216;?oint noint of water is<br>) (1)<br>(2)<br>(3)<br>(4)<\/p>\n\n\n\n<figure class=\"wp-block-image size-large\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/image-543-1024x565.png\" alt=\"\" class=\"wp-image-235935\"\/><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\"><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-0-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">The correct answer is <strong>373.47 K<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p class=\"wp-block-paragraph\">The boiling point elevation of a solution depends on the number of dissolved particles, which is determined by the van\u2019t Hoff factor (ii) and the molal concentration of the solute. The equation used to calculate the boiling point elevation is:<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">\u0394Tb=iKbm\\Delta T_b = i K_b m<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>\u0394Tb\\Delta T_b is the boiling point elevation,<\/li>\n\n\n\n<li>ii is the van\u2019t Hoff factor (the number of particles into which the solute dissociates),<\/li>\n\n\n\n<li>KbK_b is the ebullioscopic constant of the solvent (for water, Kb=0.512K_b = 0.512 K\u00b7kg\/mol),<\/li>\n\n\n\n<li>mm is the molality of the solution.<\/li>\n<\/ul>\n\n\n\n<p class=\"wp-block-paragraph\">Urea is a non-electrolyte and does not dissociate in solution, so its van\u2019t Hoff factor is 1. The boiling point of the 10% aqueous urea solution is given as <strong>374.11 K<\/strong>, meaning it experienced boiling point elevation.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Similarly, glucose is also a non-electrolyte and does not dissociate in water. A 10% glucose solution has a similar number of dissolved molecules, but since glucose has a higher molar mass (180 g\/mol) than urea (60 g\/mol), its molality is lower for the same mass percent.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Since boiling point elevation is directly proportional to molality, a 10% glucose solution will experience a slightly lower increase in boiling point compared to urea. This results in a boiling point of <strong>373.47 K<\/strong>, which is the correct answer.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">The difference in boiling points arises due to the fact that urea has a lower molar mass, resulting in more dissolved moles for the same mass percent and greater colligative effects. This explains why urea\u2019s solution has a higher boiling point elevation than glucose\u2019s solution, even though both are non-electrolytes.<\/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-banner10-133.jpeg\" alt=\"\" class=\"wp-image-235936\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Aqueous solution (by mass) of urea has boiling point. The boiling point ofglucose in watar :- &#8216;?oint noint of water is) (1)(2)(3)(4) The Correct Answer and Explanation is: The correct answer is 373.47 K. Explanation: The boiling point elevation of a solution depends on the number of dissolved particles, which is determined by the van\u2019t [&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-235934","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/235934","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=235934"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/235934\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=235934"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=235934"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=235934"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}