{"id":206413,"date":"2025-03-29T07:56:14","date_gmt":"2025-03-29T07:56:14","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=206413"},"modified":"2025-03-29T07:56:16","modified_gmt":"2025-03-29T07:56:16","slug":"how-many-grams-of-naoh-mw-40-0-are-there-in-150-0-ml-of-a-0-175-m-naoh-solution","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/29\/how-many-grams-of-naoh-mw-40-0-are-there-in-150-0-ml-of-a-0-175-m-naoh-solution\/","title":{"rendered":"How many grams of NaOH (MW = 40.0) are there in 150.0 mL of a 0.175 M NaOH solution"},"content":{"rendered":"\n

How many grams of NaOH (MW = 40.0) are there in 150.0 mL of a 0.175 M NaOH solution?<\/p>\n\n\n\n

0.00219
0.0263
114
14.0
1.05<\/p>\n\n\n\n

The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n

Solution:<\/strong><\/h3>\n\n\n\n

To find the mass of NaOH in the solution, we use the formula:<\/p>\n\n\n\n

[
\\text{Mass} = \\text{Molarity} \\times \\text{Volume} \\times \\text{Molar Mass}
]<\/p>\n\n\n\n

Step 1: Identify the given values<\/strong><\/h4>\n\n\n\n
    \n
  • Molarity (M)<\/strong> = 0.175 M (moles per liter)<\/li>\n\n\n\n
  • Volume (V)<\/strong> = 150.0 mL = 0.150 L<\/strong> (convert mL to L)<\/li>\n\n\n\n
  • Molar Mass of NaOH (MW)<\/strong> = 40.0 g\/mol<\/li>\n<\/ul>\n\n\n\n

    Step 2: Calculate the number of moles of NaOH<\/strong><\/h4>\n\n\n\n

    [
    \\text{Moles of NaOH} = \\text{Molarity} \\times \\text{Volume}
    ]
    [
    = 0.175 \\times 0.150
    ]
    [
    = 0.02625 \\text{ moles}
    ]<\/p>\n\n\n\n

    Step 3: Convert moles to grams<\/strong><\/h4>\n\n\n\n

    [
    \\text{Mass} = \\text{Moles} \\times \\text{Molar Mass}
    ]
    [
    = 0.02625 \\times 40.0
    ]
    [
    = 1.05 \\text{ grams}
    ]<\/p>\n\n\n\n

    Final Answer:<\/strong><\/h3>\n\n\n\n

    1.05 g<\/strong> (Correct option: 1.05<\/strong>)<\/p>\n\n\n\n

    \n\n\n\n

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

    This problem involves a simple molarity to mass conversion<\/strong>. The key steps are:<\/p>\n\n\n\n

      \n
    1. Convert mL to L<\/strong> (since molarity is in moles per liter<\/strong>).<\/li>\n\n\n\n
    2. Use Molarity \u00d7 Volume<\/strong> to find moles of solute<\/strong>.<\/li>\n\n\n\n
    3. Multiply by the molar mass<\/strong> to find the mass in grams<\/strong>.<\/li>\n<\/ol>\n\n\n\n

      The most common mistake is forgetting to convert mL to L, which would result in an incorrect answer. Another mistake is misusing the molar mass in calculations.<\/p>\n\n\n\n

      Thus, 1.05 g of NaOH is present in 150.0 mL of 0.175 M NaOH solution<\/strong>.<\/p>\n\n\n\n

      \n\n\n\n
      \"\"<\/figure>\n\n\n\n

      Here is an image generated with DALL\u00b7E to represent the NaOH solution problem. It features a chemistry beaker with 150.0 mL of clear NaOH solution, a molecular structure of NaOH above it, and a balance scale showing 1.05 grams of NaOH being weighed. The background includes a periodic table and a lab setting.<\/p>\n","protected":false},"excerpt":{"rendered":"

      How many grams of NaOH (MW = 40.0) are there in 150.0 mL of a 0.175 M NaOH solution? 0.002190.026311414.01.05 The correct answer and explanation is : Solution: To find the mass of NaOH in the solution, we use the formula: [\\text{Mass} = \\text{Molarity} \\times \\text{Volume} \\times \\text{Molar Mass}] Step 1: Identify the given values […]<\/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-206413","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/206413","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=206413"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/206413\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=206413"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=206413"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=206413"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}