{"id":21076,"date":"2025-06-14T22:28:47","date_gmt":"2025-06-14T22:28:47","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=21076"},"modified":"2025-06-14T22:28:54","modified_gmt":"2025-06-14T22:28:54","slug":"how-many-grams-of-sucrose-are-needed-to-make-a-375-millimolar-concentration-in-250milliliters","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/how-many-grams-of-sucrose-are-needed-to-make-a-375-millimolar-concentration-in-250milliliters\/","title":{"rendered":"How many grams of sucrose are needed to make a 375 millimolar concentration in 250milliliters"},"content":{"rendered":"\n<p>How many grams of sucrose are needed to make a 375 millimolar concentration in 250milliliters<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-vivid-cyan-blue-color\"><strong>The correct answer and explanation is:<\/strong><\/mark><\/p>\n\n\n\n<p>To find the <strong>grams of sucrose<\/strong> needed to make a <strong>375 millimolar (mM)<\/strong> solution in <strong>250 milliliters (mL)<\/strong>, we use the <strong>molarity formula<\/strong>: Molarity&nbsp;(M)=moles&nbsp;of&nbsp;soluteliters&nbsp;of&nbsp;solution\\text{Molarity (M)} = \\frac{\\text{moles of solute}}{\\text{liters of solution}}<\/p>\n\n\n\n<p>Since we\u2019re given millimolar (mM), we\u2019ll convert it to molar (M): 375\u2009mM=0.375\u2009M375 \\, \\text{mM} = 0.375 \\, \\text{M}<\/p>\n\n\n\n<p>We\u2019re also given volume in mL, so convert to liters: 250\u2009mL=0.250\u2009L250 \\, \\text{mL} = 0.250 \\, \\text{L}<\/p>\n\n\n\n<p>Now calculate <strong>moles of sucrose<\/strong>: Moles=Molarity\u00d7Volume=0.375\u2009mol\/L\u00d70.250\u2009L=0.09375\u2009mol\\text{Moles} = Molarity \\times Volume = 0.375 \\, \\text{mol\/L} \\times 0.250 \\, \\text{L} = 0.09375 \\, \\text{mol}<\/p>\n\n\n\n<p>Next, convert moles to grams using the molar mass of <strong>sucrose (C\u2081\u2082H\u2082\u2082O\u2081\u2081)<\/strong>, which is approximately <strong>342.3 g\/mol<\/strong>: Mass&nbsp;(g)=Moles\u00d7Molar&nbsp;Mass=0.09375\u00d7342.3=32.093\u2009g\\text{Mass (g)} = \\text{Moles} \\times \\text{Molar Mass} = 0.09375 \\times 342.3 = 32.093 \\, \\text{g}<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">\u2705 Final Answer:<\/h3>\n\n\n\n<p><strong>32.09 grams of sucrose<\/strong> are needed to make a 375 mM solution in 250 mL of water.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">\ud83d\udd0d Explanation (300 words):<\/h3>\n\n\n\n<p>Creating a solution of a specific molarity involves using the formula: Molarity=Moles&nbsp;of&nbsp;soluteLiters&nbsp;of&nbsp;solution\\text{Molarity} = \\frac{\\text{Moles of solute}}{\\text{Liters of solution}}<\/p>\n\n\n\n<p>Molarity (M) tells us how many moles of solute are present in one liter of solution. In this case, we\u2019re making a <strong>375 mM<\/strong> (millimolar) solution, which is equal to <strong>0.375 M<\/strong>. We&#8217;re preparing <strong>250 mL<\/strong> of this solution, which is <strong>0.250 liters<\/strong>. To determine the number of moles needed, multiply molarity by volume: Moles=0.375\u00d70.250=0.09375&nbsp;mol\\text{Moles} = 0.375 \\times 0.250 = 0.09375 \\text{ mol}<\/p>\n\n\n\n<p>Sucrose\u2019s molar mass (its weight per mole) is <strong>342.3 g\/mol<\/strong>. This value is found by adding the atomic weights of its atoms:<br>12 Carbon (12\u00d712.01), 22 Hydrogen (22\u00d71.008), and 11 Oxygen (11\u00d716.00).<\/p>\n\n\n\n<p>Now, convert moles to grams: Grams=Moles\u00d7Molar&nbsp;Mass=0.09375\u00d7342.3=32.09&nbsp;g\\text{Grams} = \\text{Moles} \\times \\text{Molar Mass} = 0.09375 \\times 342.3 = 32.09 \\text{ g}<\/p>\n\n\n\n<p>Thus, to make the solution, you would <strong>weigh out 32.09 grams of sucrose<\/strong>, then dissolve it in water and make up the volume to <strong>250 mL<\/strong>. This is a common technique in labs for preparing standard solutions used in biology, chemistry, and medical fields.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>How many grams of sucrose are needed to make a 375 millimolar concentration in 250milliliters The correct answer and explanation is: To find the grams of sucrose needed to make a 375 millimolar (mM) solution in 250 milliliters (mL), we use the molarity formula: Molarity&nbsp;(M)=moles&nbsp;of&nbsp;soluteliters&nbsp;of&nbsp;solution\\text{Molarity (M)} = \\frac{\\text{moles of solute}}{\\text{liters of solution}} Since we\u2019re given [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-21076","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/21076","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=21076"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/21076\/revisions"}],"predecessor-version":[{"id":21078,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/21076\/revisions\/21078"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=21076"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=21076"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=21076"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}