The density of concentrated ammonia, which is 28.0% w\/w NH3, is 0.899 g\/mL. What volume of this reagent should be diluted to 1.0 \u00d7 103 mL to make a solution that is 0.036 M in NH3?<\/p>\n\n\n\n
The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n To find the volume of 28.0% (w\/w) concentrated ammonia needed to prepare 1000 mL (1.0 \u00d7 10\u00b3 mL) of a 0.036 M<\/strong> ammonia solution, we need to go step-by-step:<\/p>\n\n\n\n We’re given:<\/p>\n\n\n\n Let\u2019s find out how many moles of NH\u2083 are present in 1 liter (1000 mL) of the concentrated solution.<\/p>\n\n\n\n Mass of 1 mL of solution<\/strong> = 0.899 g Now, calculate the mass of NH\u2083 in this 899 g of solution:<\/p>\n\n\n\n [ Convert this to moles using the molar mass of NH\u2083 (17.03 g\/mol):<\/p>\n\n\n\n [ So, molarity of concentrated NH\u2083<\/strong> is:<\/p>\n\n\n\n [ [ Where:<\/p>\n\n\n\n [ [ This problem involves using percentage concentration, density, and molarity concepts to perform a dilution. First, we used the w\/w % and density to determine how many grams and moles of ammonia are present in 1 liter of the concentrated solution. This gave us the molarity of the concentrated reagent. Then, we used the dilution formula (M_1V_1 = M_2V_2) to find how much of the concentrated solution was required to prepare the target dilute solution. The final step involved simple algebra to solve for the unknown volume. This is a classic application of solution chemistry in lab preparations.<\/p>\n","protected":false},"excerpt":{"rendered":" The density of concentrated ammonia, which is 28.0% w\/w NH3, is 0.899 g\/mL. What volume of this reagent should be diluted to 1.0 \u00d7 103 mL to make a solution that is 0.036 M in NH3? The correct answer and explanation is : To find the volume of 28.0% (w\/w) concentrated ammonia needed to prepare […]<\/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-208002","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/208002","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=208002"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/208002\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=208002"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=208002"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=208002"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\nStep 1: Determine the molarity of the concentrated ammonia<\/strong><\/h3>\n\n\n\n
\n
Mass of 1000 mL<\/strong> = 0.899 g\/mL \u00d7 1000 mL = 899 g<\/strong><\/p>\n\n\n\n
\\text{Mass of NH\u2083} = 28\\% \\times 899\\ \\text{g} = 0.28 \\times 899 = 251.72\\ \\text{g NH\u2083}
]<\/p>\n\n\n\n
\\text{Moles of NH\u2083} = \\frac{251.72\\ \\text{g}}{17.03\\ \\text{g\/mol}} \\approx 14.78\\ \\text{mol}
]<\/p>\n\n\n\n
\\frac{14.78\\ \\text{mol}}{1\\ \\text{L}} = 14.78\\ \\text{M}
]<\/p>\n\n\n\n
\n\n\n\nStep 2: Use dilution formula to find required volume<\/strong><\/h3>\n\n\n\n
M_1 V_1 = M_2 V_2
]<\/p>\n\n\n\n\n
14.78 \\times V_1 = 0.036 \\times 1000
]<\/p>\n\n\n\n
V_1 = \\frac{36}{14.78} \\approx 2.43\\ \\text{mL}
]<\/p>\n\n\n\n
\n\n\n\n\u2705 Final Answer: 2.43 mL of concentrated ammonia solution<\/strong><\/h3>\n\n\n\n
\n\n\n\nExplanation<\/strong><\/h3>\n\n\n\n