The mass of NaNO3 (molar mass 85.00 g\/mol) present in 275mL of a 0.45M solution is equal to _____g.<\/p>\n\n\n\n
The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n To find the mass of sodium nitrate (NaNO\u2083) in a given volume of solution, we use the formula:<\/p>\n\n\n\n [ Now plug into the formula:<\/p>\n\n\n\n [ [ Rounded to three significant figures (based on the given data), the mass is:<\/strong><\/p>\n\n\n\n [ In chemistry, calculating the mass of a solute (the substance dissolved in a solution) is a fundamental skill, especially in preparing or analyzing solutions. In this example, we\u2019re working with sodium nitrate (NaNO\u2083), a common salt used in fertilizers and food preservation.<\/p>\n\n\n\n We\u2019re given the molarity<\/strong> (concentration) of the solution as 0.45 M, which means there are 0.45 moles of NaNO\u2083 dissolved in every liter of solution. We’re also given the volume<\/strong> of the solution as 275 mL, which must be converted to liters because molarity is expressed in moles per liter. So, 275 mL is equivalent to 0.275 liters.<\/p>\n\n\n\n Next, we apply the relationship:<\/p>\n\n\n\n [ So the moles of NaNO\u2083 present are:<\/p>\n\n\n\n [ To convert moles to grams, we multiply by the molar mass (85.00 g\/mol), giving:<\/p>\n\n\n\n [ Rounded to appropriate significant figures, the mass of NaNO\u2083 is 10.5 grams<\/strong>. This calculation is essential in laboratory settings, where accurate concentrations are required for reactions, titrations, or formulation of chemical solutions.<\/p>\n","protected":false},"excerpt":{"rendered":" The mass of NaNO3 (molar mass 85.00 g\/mol) present in 275mL of a 0.45M solution is equal to _____g. The correct answer and explanation is : To find the mass of sodium nitrate (NaNO\u2083) in a given volume of solution, we use the formula: [\\text{Mass (g)} = \\text{Molarity (mol\/L)} \\times \\text{Volume (L)} \\times \\text{Molar Mass […]<\/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-210173","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/210173","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=210173"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/210173\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=210173"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=210173"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=210173"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\\text{Mass (g)} = \\text{Molarity (mol\/L)} \\times \\text{Volume (L)} \\times \\text{Molar Mass (g\/mol)}
]<\/p>\n\n\n\nStep-by-step Calculation:<\/h3>\n\n\n\n
\n
\\text{Mass} = 0.45 \\, \\text{mol\/L} \\times 0.275 \\, \\text{L} \\times 85.00 \\, \\text{g\/mol}
]<\/p>\n\n\n\n
\\text{Mass} = 10.509375 \\, \\text{g}
]<\/p>\n\n\n\n
\\boxed{10.5 \\, \\text{g}}
]<\/p>\n\n\n\n
\n\n\n\nExplanation (Approx. 300 Words):<\/h3>\n\n\n\n
\\text{moles} = \\text{molarity} \\times \\text{volume}
]<\/p>\n\n\n\n
0.45 \\, \\text{mol\/L} \\times 0.275 \\, \\text{L} = 0.12375 \\, \\text{mol}
]<\/p>\n\n\n\n
0.12375 \\times 85.00 = 10.509375 \\, \\text{g}
]<\/p>\n\n\n\n