{"id":217837,"date":"2025-05-22T14:37:58","date_gmt":"2025-05-22T14:37:58","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=217837"},"modified":"2025-05-22T14:38:00","modified_gmt":"2025-05-22T14:38:00","slug":"calculate-the-grams-or-milliliters-of-solute-needed-to-prepare-the-following-solutions","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/22\/calculate-the-grams-or-milliliters-of-solute-needed-to-prepare-the-following-solutions\/","title":{"rendered":"Calculate the grams or milliliters of solute needed to prepare the following solutions"},"content":{"rendered":"\n

Calculate the grams or milliliters of solute needed to prepare the following solutions.<\/strong><\/p>\n\n\n\n

(PART A)\u00c3\u201a\u00c2 <\/strong>60. gg of a 3.0 % (m\/m) KCl solution<\/strong>Express your answer using two significant figures. <\/strong>(Answer should be in grams<\/strong><\/p>\n\n\n\n

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

To solve this problem, we will use the formula for mass\/mass percent concentration (% m\/m)<\/strong>:<\/p>\n\n\n\n

$$
\\text{mass percent} = \\left( \\frac{\\text{mass of solute}}{\\text{mass of solution}} \\right) \\times 100
$$<\/p>\n\n\n\n

\n\n\n\n

Given:<\/h3>\n\n\n\n
    \n
  • Mass percent (% m\/m) = 3.0%<\/li>\n\n\n\n
  • Mass of solution = 60. g (note: “gg” seems to be a typo)<\/li>\n\n\n\n
  • Unknown: mass of solute (in grams)<\/li>\n<\/ul>\n\n\n\n
    \n\n\n\n

    Step 1: Rearranging the formula<\/h3>\n\n\n\n

    To find the mass of solute<\/strong>, rearrange the formula:<\/p>\n\n\n\n

    $$
    \\text{mass of solute} = \\left( \\frac{\\text{mass percent}}{100} \\right) \\times \\text{mass of solution}
    $$<\/p>\n\n\n\n

    \n\n\n\n

    Step 2: Plug in the values<\/h3>\n\n\n\n

    $$
    \\text{mass of solute} = \\left( \\frac{3.0}{100} \\right) \\times 60
    $$<\/p>\n\n\n\n

    $$
    \\text{mass of solute} = 0.03 \\times 60 = 1.8 \\, \\text{g}
    $$<\/p>\n\n\n\n

    \n\n\n\n

    \u2705 Final Answer: 1.8 g<\/strong><\/h3>\n\n\n\n
    \n\n\n\n

    \u270f\ufe0f Explanation (300 words)<\/h2>\n\n\n\n

    This problem involves preparing a potassium chloride (KCl) solution where the concentration is given in terms of mass\/mass percent (% m\/m). The mass\/mass percent tells us how many grams of solute are present in 100 grams of the entire solution<\/strong>. A 3.0% (m\/m) solution means that there are 3 grams of KCl in every 100 grams of solution.<\/p>\n\n\n\n

    In this case, we are told we need 60 grams of the entire solution<\/strong>, and we are asked to find how many grams of KCl (solute)<\/strong> are needed to make this.<\/p>\n\n\n\n

    To find that, we use the equation:<\/p>\n\n\n\n

    $$
    \\text{mass of solute} = \\left( \\frac{\\text{percent concentration}}{100} \\right) \\times \\text{mass of solution}
    $$<\/p>\n\n\n\n

    This formula works by taking the proportion of the solution that is KCl (3.0%, or 0.03 when expressed as a decimal), and multiplying it by the total solution mass (60 g). This gives:<\/p>\n\n\n\n

    $$
    0.03 \\times 60 = 1.8 \\, \\text{g of KCl}
    $$<\/p>\n\n\n\n

    This value represents the amount of potassium chloride you must weigh and dissolve in enough water to reach a total solution mass<\/strong> of 60 grams. It’s important not to add 60 grams of water, but rather to add enough water<\/strong> to bring the total mass (solute + solvent) up to 60 grams.<\/p>\n\n\n\n

    This concept is frequently applied in laboratory and clinical settings, where accurate concentrations are needed for chemical reactions, medication dosing, or IV fluid preparations.<\/p>\n\n\n\n

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

    Calculate the grams or milliliters of solute needed to prepare the following solutions. (PART A)\u00c3\u201a\u00c2 60. gg of a 3.0 % (m\/m) KCl solutionExpress your answer using two significant figures. (Answer should be in grams The Correct Answer and Explanation is: To solve this problem, we will use the formula for mass\/mass percent concentration (% m\/m): $$\\text{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-217837","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/217837","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=217837"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/217837\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=217837"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=217837"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=217837"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}