{"id":218513,"date":"2025-05-23T21:55:10","date_gmt":"2025-05-23T21:55:10","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=218513"},"modified":"2025-05-23T21:55:13","modified_gmt":"2025-05-23T21:55:13","slug":"the-ionic-compound-nabr-is-soluble-in-water","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/23\/the-ionic-compound-nabr-is-soluble-in-water\/","title":{"rendered":"The ionic compound NaBr is soluble in water"},"content":{"rendered":"\n<p>Transcribed image text: The ionic compound NaBr is soluble in water. Calculate the osmotic pressure (in atm) generated when 7.70 grams of sodium bromide are dissolved in 94.1 mL of an aqueous solution at 298 K. The van&#8217;t Hoff factor for NaBr in this solution is 1.94. atm<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To calculate the <strong>osmotic pressure<\/strong> (\u03c0) of a solution, we use the <strong>van\u2019t Hoff equation<\/strong>: \u03c0=iMRT\\pi = iMRT<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>\u03c0\\pi = osmotic pressure (in atm)<\/li>\n\n\n\n<li>ii = van\u2019t Hoff factor (number of particles the solute breaks into)<\/li>\n\n\n\n<li>MM = molarity of the solution (mol\/L)<\/li>\n\n\n\n<li>RR = ideal gas constant = 0.08206 L\u00b7atm\/mol\u00b7K<\/li>\n\n\n\n<li>TT = temperature in Kelvin (K)<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Step 1: Calculate moles of NaBr<\/strong><\/h3>\n\n\n\n<p>Molar mass of NaBr = 22.99 (Na) + 79.90 (Br) = <strong>102.89 g\/mol<\/strong> Moles&nbsp;of&nbsp;NaBr=7.70&nbsp;g102.89&nbsp;g\/mol=0.07487&nbsp;mol\\text{Moles of NaBr} = \\frac{7.70 \\text{ g}}{102.89 \\text{ g\/mol}} = 0.07487 \\text{ mol}<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Step 2: Convert volume to liters<\/strong><\/h3>\n\n\n\n<p>94.1&nbsp;mL=0.0941&nbsp;L94.1 \\text{ mL} = 0.0941 \\text{ L}<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Step 3: Calculate molarity<\/strong><\/h3>\n\n\n\n<p>M=0.07487&nbsp;mol0.0941&nbsp;L=0.7956&nbsp;mol\/LM = \\frac{0.07487 \\text{ mol}}{0.0941 \\text{ L}} = 0.7956 \\text{ mol\/L}<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Step 4: Plug values into van\u2019t Hoff equation<\/strong><\/h3>\n\n\n\n<p>\u03c0=(1.94)(0.7956&nbsp;mol\/L)(0.08206&nbsp;L\\cdotpatm\/mol\\cdotpK)(298&nbsp;K)\\pi = (1.94)(0.7956 \\text{ mol\/L})(0.08206 \\text{ L\u00b7atm\/mol\u00b7K})(298 \\text{ K}) \u03c0=1.94\u00d70.7956\u00d70.08206\u00d7298=37.71&nbsp;atm\\pi = 1.94 \\times 0.7956 \\times 0.08206 \\times 298 = 37.71 \\text{ atm}<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">\u2705 <strong>Final Answer:<\/strong><\/h3>\n\n\n\n<p><strong>Osmotic pressure = 37.7 atm<\/strong><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Explanation (\u2248300 words)<\/strong><\/h3>\n\n\n\n<p>Osmotic pressure is the pressure required to stop the flow of solvent through a semipermeable membrane from pure solvent into a solution. This property depends on the <strong>concentration of solute particles<\/strong>, not their identity\u2014making it a <strong>colligative property<\/strong>.<\/p>\n\n\n\n<p>Sodium bromide (NaBr) is an <strong>ionic compound<\/strong> that dissociates in water into two ions: <strong>Na\u207a<\/strong> and <strong>Br\u207b<\/strong>. Ideally, one formula unit of NaBr yields two particles, so the ideal van\u2019t Hoff factor would be 2. However, due to ion pairing in real solutions, the actual van\u2019t Hoff factor is often slightly less. In this problem, it\u2019s given as <strong>1.94<\/strong>, indicating partial ion association.<\/p>\n\n\n\n<p>We first calculated the number of moles of NaBr using its molar mass and the given mass (7.70 g). Next, we converted the volume of the solution from milliliters to liters to determine molarity (mol\/L). Molarity tells us how many moles of solute are present in each liter of solution.<\/p>\n\n\n\n<p>Then we applied the van\u2019t Hoff equation: \u03c0=iMRT\\pi = iMRT<\/p>\n\n\n\n<p>Here, the constants R=0.08206&nbsp;L\\cdotpatm\/mol\\cdotpKR = 0.08206 \\text{ L\u00b7atm\/mol\u00b7K} and temperature T=298&nbsp;KT = 298 \\text{ K} were used. Multiplying all values together gave the final osmotic pressure of <strong>37.7 atm<\/strong>, a relatively high pressure due to the strong dissociation of NaBr and the concentrated nature of the solution.<\/p>\n\n\n\n<p>This calculation is crucial in biological and chemical systems where osmotic pressure affects processes like nutrient absorption, water balance in cells, and drug delivery.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/05\/image-265.png\" alt=\"\" class=\"wp-image-218514\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Transcribed image text: The ionic compound NaBr is soluble in water. Calculate the osmotic pressure (in atm) generated when 7.70 grams of sodium bromide are dissolved in 94.1 mL of an aqueous solution at 298 K. The van&#8217;t Hoff factor for NaBr in this solution is 1.94. atm The Correct Answer and Explanation is: To [&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-218513","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/218513","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=218513"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/218513\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=218513"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=218513"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=218513"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}