{"id":189736,"date":"2025-02-10T08:10:52","date_gmt":"2025-02-10T08:10:52","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=189736"},"modified":"2025-02-10T08:10:54","modified_gmt":"2025-02-10T08:10:54","slug":"calculate-the-osmotic-pressure-of-5-glucose-solution","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/10\/calculate-the-osmotic-pressure-of-5-glucose-solution\/","title":{"rendered":"calculate the osmotic pressure of 5% glucose solution"},"content":{"rendered":"\n<p>calculate the osmotic pressure of 5% glucose solution,where the molecular weight of glucose is 180 gm,at 18 c ??<\/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 calculate the osmotic pressure of a 5% glucose solution at 18\u00b0C, we will use the formula for osmotic pressure:<\/p>\n\n\n\n<p>[<br>\\Pi = \\frac{nRT}{V}<br>]<\/p>\n\n\n\n<p>where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>(\\Pi) is the osmotic pressure in atmospheres (atm),<\/li>\n\n\n\n<li>(n) is the number of moles of solute,<\/li>\n\n\n\n<li>(R) is the ideal gas constant (0.0821 L\u00b7atm\/mol\u00b7K),<\/li>\n\n\n\n<li>(T) is the absolute temperature in Kelvin (K),<\/li>\n\n\n\n<li>(V) is the volume of the solution in liters.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step-by-Step Calculation:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Convert the mass percentage of glucose to moles:<\/strong> A 5% glucose solution means there are 5 grams of glucose per 100 mL of solution. Since we are dealing with 100 mL, it\u2019s equivalent to 0.1 L. To calculate the number of moles of glucose: [<br>\\text{Moles of glucose} = \\frac{\\text{Mass of glucose}}{\\text{Molecular weight of glucose}}<br>] Given:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Mass of glucose = 5 grams,<\/li>\n\n\n\n<li>Molecular weight of glucose = 180 g\/mol. [<br>\\text{Moles of glucose} = \\frac{5 \\text{ g}}{180 \\text{ g\/mol}} = 0.02778 \\text{ moles}<br>]<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Convert the temperature to Kelvin:<\/strong> The temperature is given as 18\u00b0C. To convert this to Kelvin: [<br>T = 18\u00b0C + 273.15 = 291.15 \\text{ K}<br>]<\/li>\n\n\n\n<li><strong>Calculate the osmotic pressure:<\/strong> Now, we can substitute all the values into the osmotic pressure formula: [<br>\\Pi = \\frac{(0.02778 \\text{ mol})(0.0821 \\text{ L\u00b7atm\/mol\u00b7K})(291.15 \\text{ K})}{0.1 \\text{ L}}<br>] [<br>\\Pi = \\frac{(0.02778)(0.0821)(291.15)}{0.1}<br>] [<br>\\Pi \\approx 0.0673 \\text{ atm}<br>]<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>The osmotic pressure of a solution is a colligative property, meaning it depends on the number of solute particles in the solution, not the identity of the solute. The formula (\\Pi = \\frac{nRT}{V}) tells us how much pressure is exerted by the solute particles when they move across a semipermeable membrane. The greater the number of solute particles, the higher the osmotic pressure.<\/p>\n\n\n\n<p>In this case, we calculated the osmotic pressure of a 5% glucose solution at 18\u00b0C and found it to be approximately <strong>0.0673 atm<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>calculate the osmotic pressure of 5% glucose solution,where the molecular weight of glucose is 180 gm,at 18 c ?? The Correct Answer and Explanation is : To calculate the osmotic pressure of a 5% glucose solution at 18\u00b0C, we will use the formula for osmotic pressure: [\\Pi = \\frac{nRT}{V}] where: Step-by-Step Calculation: Explanation: The osmotic [&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-189736","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/189736","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=189736"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/189736\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=189736"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=189736"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=189736"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}