{"id":231369,"date":"2025-06-11T03:48:18","date_gmt":"2025-06-11T03:48:18","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=231369"},"modified":"2025-06-11T03:48:20","modified_gmt":"2025-06-11T03:48:20","slug":"water-150-ml-having-a-density-of-1-g-cm","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/11\/water-150-ml-having-a-density-of-1-g-cm\/","title":{"rendered":"water (150 mL) having a density of 1 g\/cm"},"content":{"rendered":"\n

water (150 mL) having a density of 1 g\/cm
. (a) Determine the volume percent of methanol (b) Determine the mass percent of water.m<\/p>\n\n\n\n

is mixed with water (150 mL) having a density of 1 g\/cm
. (a) Determine the volume percent of methanol (b) Determine the mass percent of water.<\/p>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

a) The volume percent of methanol is 14.29%.<\/strong>
(b) The mass percent of water is 88.34%.<\/strong><\/p>\n\n\n\n

\n\n\n\n

Explanation<\/strong><\/h3>\n\n\n\n

This problem requires the calculation of solution concentration in two different ways: volume percent and mass percent. These are common methods for expressing the amount of a solute (methanol) dissolved in a solvent (water).<\/p>\n\n\n\n

Part (a): Volume Percent of Methanol<\/strong><\/p>\n\n\n\n

The volume percent of a component in a mixture is the volume of that component divided by the total volume of the solution, multiplied by 100 to express it as a percentage. The formula is:<\/p>\n\n\n\n

Volume % = (Volume of Component \/ Total Volume of Solution) \u00d7 100%<\/p>\n\n\n\n

First, we must determine the total volume of the solution. Assuming the volumes are additive upon mixing, we sum the volumes of the individual components:<\/p>\n\n\n\n

Total Volume = Volume of Methanol + Volume of Water
Total Volume = 25 mL + 150 mL = 175 mL<\/p>\n\n\n\n

Next, we use this total volume to find the volume percent of methanol:<\/p>\n\n\n\n

Volume % Methanol = (25 mL \/ 175 mL) \u00d7 100% = 14.29%<\/p>\n\n\n\n

Part (b): Mass Percent of Water<\/strong><\/p>\n\n\n\n

The mass percent of a component is its mass divided by the total mass of the solution, multiplied by 100. The formula is:<\/p>\n\n\n\n

Mass % = (Mass of Component \/ Total Mass of Solution) \u00d7 100%<\/p>\n\n\n\n

The problem provides volumes and densities, so we must first calculate the mass of each component using the relationship: Mass = Density \u00d7 Volume. Note that 1 cm\u00b3 is equivalent to 1 mL, allowing for direct calculation.<\/p>\n\n\n\n

Mass of Methanol = 0.792 g\/cm\u00b3 \u00d7 25 mL = 19.8 g
Mass of Water = 1 g\/cm\u00b3 \u00d7 150 mL = 150 g<\/p>\n\n\n\n

Now, we calculate the total mass of the solution by summing the individual masses:<\/p>\n\n\n\n

Total Mass = Mass of Methanol + Mass of Water
Total Mass = 19.8 g + 150 g = 169.8 g<\/p>\n\n\n\n

Finally, we apply the mass percent formula for water:<\/p>\n\n\n\n

Mass % Water = (150 g \/ 169.8 g) \u00d7 100% = 88.34%<\/p>\n\n\n\n

This demonstrates how the same solution has different concentration values depending on whether it is expressed by volume or by mass, due to the different densities of the components.<\/p>\n\n\n\n

\"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

water (150 mL) having a density of 1 g\/cm. (a) Determine the volume percent of methanol (b) Determine the mass percent of water.m is mixed with water (150 mL) having a density of 1 g\/cm. (a) Determine the volume percent of methanol (b) Determine the mass percent of water. The Correct Answer and Explanation is: […]<\/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-231369","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231369","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=231369"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231369\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=231369"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=231369"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=231369"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}