To calculate the mole percent of sodium hydroxide (NaOH) in a 36.9% by mass aqueous NaOH solution with a density of 1.03 g\/mL, follow these steps:<\/p>\n\n\n\n
1. Determine the mass of NaOH in the solution<\/strong><\/h3>\n\n\n\nThe solution is 36.9% by mass NaOH, meaning 36.9 grams of NaOH are present in 100 grams of the solution. Therefore, in 100 grams of solution, we have:<\/p>\n\n\n\n
\n- Mass of NaOH = 36.9 g<\/li>\n<\/ul>\n\n\n\n
2. Determine the mass of water in the solution<\/strong><\/h3>\n\n\n\nThe remaining mass of the solution is water. Since the total mass is 100 grams, the mass of water is:<\/p>\n\n\n\n
\n- Mass of water = 100 g – 36.9 g = 63.1 g<\/li>\n<\/ul>\n\n\n\n
3. Calculate the number of moles of NaOH<\/strong><\/h3>\n\n\n\nTo find the number of moles of NaOH, use its molar mass. The molar mass of NaOH is:<\/p>\n\n\n\n
\n- NaOH: 22.99 (Na) + 15.999 (O) + 1.008 (H) = 39.997 g\/mol<\/li>\n<\/ul>\n\n\n\n
Now, calculate the moles of NaOH:Moles of NaOH=Mass of NaOHMolar Mass of NaOH=36.9\u2009g39.997\u2009g\/mol=0.922\u2009mol\\text{Moles of NaOH} = \\frac{\\text{Mass of NaOH}}{\\text{Molar Mass of NaOH}} = \\frac{36.9 \\, \\text{g}}{39.997 \\, \\text{g\/mol}} = 0.922 \\, \\text{mol}Moles of NaOH=Molar Mass of NaOHMass of NaOH\u200b=39.997g\/mol36.9g\u200b=0.922mol<\/p>\n\n\n\n
4. Calculate the moles of water (H\u2082O)<\/strong><\/h3>\n\n\n\nThe molar mass of water (H\u2082O) is:<\/p>\n\n\n\n
\n- H\u2082O: 2 \u00d7 1.008 (H) + 15.999 (O) = 18.015 g\/mol<\/li>\n<\/ul>\n\n\n\n
Now, calculate the moles of water:Moles of water=Mass of waterMolar Mass of water=63.1\u2009g18.015\u2009g\/mol=3.5\u2009mol\\text{Moles of water} = \\frac{\\text{Mass of water}}{\\text{Molar Mass of water}} = \\frac{63.1 \\, \\text{g}}{18.015 \\, \\text{g\/mol}} = 3.5 \\, \\text{mol}Moles of water=Molar Mass of waterMass of water\u200b=18.015g\/mol63.1g\u200b=3.5mol<\/p>\n\n\n\n
5. Calculate the total moles of the solution<\/strong><\/h3>\n\n\n\nThe total number of moles in the solution is the sum of the moles of NaOH and the moles of water:Total moles=0.922\u2009mol NaOH+3.5\u2009mol water=4.422\u2009mol\\text{Total moles} = 0.922 \\, \\text{mol NaOH} + 3.5 \\, \\text{mol water} = 4.422 \\, \\text{mol}Total moles=0.922mol NaOH+3.5mol water=4.422mol<\/p>\n\n\n\n
6. Calculate the mole percent of NaOH<\/strong><\/h3>\n\n\n\nThe mole percent of NaOH is given by the ratio of the moles of NaOH to the total moles of the solution, multiplied by 100:Mole percent of NaOH=(Moles of NaOHTotal moles)\u00d7100=(0.9224.422)\u00d7100=20.85%\\text{Mole percent of NaOH} = \\left( \\frac{\\text{Moles of NaOH}}{\\text{Total moles}} \\right) \\times 100 = \\left( \\frac{0.922}{4.422} \\right) \\times 100 = 20.85\\%Mole percent of NaOH=(Total molesMoles of NaOH\u200b)\u00d7100=(4.4220.922\u200b)\u00d7100=20.85%<\/p>\n\n\n\n
Final Answer:<\/h3>\n\n\n\n
The mole percent of NaOH in the solution is 20.85%<\/strong>.<\/p>\n\n\n\n![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner6-1572.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"An aqueous solution is 36.9% by mass sodium hydroxide and has a density of 1.03 g mL What is the mole percent of NaOH? The Correct Answer and Explanation is: To calculate the mole percent of sodium hydroxide (NaOH) in a 36.9% by mass aqueous NaOH solution with a density of 1.03 g\/mL, follow these […]<\/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-266277","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266277","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=266277"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266277\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=266277"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=266277"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=266277"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
2. Determine the mass of water in the solution<\/strong><\/h3>\n\n\n\nThe remaining mass of the solution is water. Since the total mass is 100 grams, the mass of water is:<\/p>\n\n\n\n
\n- Mass of water = 100 g – 36.9 g = 63.1 g<\/li>\n<\/ul>\n\n\n\n
3. Calculate the number of moles of NaOH<\/strong><\/h3>\n\n\n\nTo find the number of moles of NaOH, use its molar mass. The molar mass of NaOH is:<\/p>\n\n\n\n
\n- NaOH: 22.99 (Na) + 15.999 (O) + 1.008 (H) = 39.997 g\/mol<\/li>\n<\/ul>\n\n\n\n
Now, calculate the moles of NaOH:Moles of NaOH=Mass of NaOHMolar Mass of NaOH=36.9\u2009g39.997\u2009g\/mol=0.922\u2009mol\\text{Moles of NaOH} = \\frac{\\text{Mass of NaOH}}{\\text{Molar Mass of NaOH}} = \\frac{36.9 \\, \\text{g}}{39.997 \\, \\text{g\/mol}} = 0.922 \\, \\text{mol}Moles of NaOH=Molar Mass of NaOHMass of NaOH\u200b=39.997g\/mol36.9g\u200b=0.922mol<\/p>\n\n\n\n
4. Calculate the moles of water (H\u2082O)<\/strong><\/h3>\n\n\n\nThe molar mass of water (H\u2082O) is:<\/p>\n\n\n\n
\n- H\u2082O: 2 \u00d7 1.008 (H) + 15.999 (O) = 18.015 g\/mol<\/li>\n<\/ul>\n\n\n\n
Now, calculate the moles of water:Moles of water=Mass of waterMolar Mass of water=63.1\u2009g18.015\u2009g\/mol=3.5\u2009mol\\text{Moles of water} = \\frac{\\text{Mass of water}}{\\text{Molar Mass of water}} = \\frac{63.1 \\, \\text{g}}{18.015 \\, \\text{g\/mol}} = 3.5 \\, \\text{mol}Moles of water=Molar Mass of waterMass of water\u200b=18.015g\/mol63.1g\u200b=3.5mol<\/p>\n\n\n\n
5. Calculate the total moles of the solution<\/strong><\/h3>\n\n\n\nThe total number of moles in the solution is the sum of the moles of NaOH and the moles of water:Total moles=0.922\u2009mol NaOH+3.5\u2009mol water=4.422\u2009mol\\text{Total moles} = 0.922 \\, \\text{mol NaOH} + 3.5 \\, \\text{mol water} = 4.422 \\, \\text{mol}Total moles=0.922mol NaOH+3.5mol water=4.422mol<\/p>\n\n\n\n
6. Calculate the mole percent of NaOH<\/strong><\/h3>\n\n\n\nThe mole percent of NaOH is given by the ratio of the moles of NaOH to the total moles of the solution, multiplied by 100:Mole percent of NaOH=(Moles of NaOHTotal moles)\u00d7100=(0.9224.422)\u00d7100=20.85%\\text{Mole percent of NaOH} = \\left( \\frac{\\text{Moles of NaOH}}{\\text{Total moles}} \\right) \\times 100 = \\left( \\frac{0.922}{4.422} \\right) \\times 100 = 20.85\\%Mole percent of NaOH=(Total molesMoles of NaOH\u200b)\u00d7100=(4.4220.922\u200b)\u00d7100=20.85%<\/p>\n\n\n\n
Final Answer:<\/h3>\n\n\n\n
The mole percent of NaOH in the solution is 20.85%<\/strong>.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"An aqueous solution is 36.9% by mass sodium hydroxide and has a density of 1.03 g mL What is the mole percent of NaOH? The Correct Answer and Explanation is: To calculate the mole percent of sodium hydroxide (NaOH) in a 36.9% by mass aqueous NaOH solution with a density of 1.03 g\/mL, follow these […]<\/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-266277","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266277","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=266277"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266277\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=266277"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=266277"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=266277"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
3. Calculate the number of moles of NaOH<\/strong><\/h3>\n\n\n\nTo find the number of moles of NaOH, use its molar mass. The molar mass of NaOH is:<\/p>\n\n\n\n
\n- NaOH: 22.99 (Na) + 15.999 (O) + 1.008 (H) = 39.997 g\/mol<\/li>\n<\/ul>\n\n\n\n
Now, calculate the moles of NaOH:Moles of NaOH=Mass of NaOHMolar Mass of NaOH=36.9\u2009g39.997\u2009g\/mol=0.922\u2009mol\\text{Moles of NaOH} = \\frac{\\text{Mass of NaOH}}{\\text{Molar Mass of NaOH}} = \\frac{36.9 \\, \\text{g}}{39.997 \\, \\text{g\/mol}} = 0.922 \\, \\text{mol}Moles of NaOH=Molar Mass of NaOHMass of NaOH\u200b=39.997g\/mol36.9g\u200b=0.922mol<\/p>\n\n\n\n
4. Calculate the moles of water (H\u2082O)<\/strong><\/h3>\n\n\n\nThe molar mass of water (H\u2082O) is:<\/p>\n\n\n\n
\n- H\u2082O: 2 \u00d7 1.008 (H) + 15.999 (O) = 18.015 g\/mol<\/li>\n<\/ul>\n\n\n\n
Now, calculate the moles of water:Moles of water=Mass of waterMolar Mass of water=63.1\u2009g18.015\u2009g\/mol=3.5\u2009mol\\text{Moles of water} = \\frac{\\text{Mass of water}}{\\text{Molar Mass of water}} = \\frac{63.1 \\, \\text{g}}{18.015 \\, \\text{g\/mol}} = 3.5 \\, \\text{mol}Moles of water=Molar Mass of waterMass of water\u200b=18.015g\/mol63.1g\u200b=3.5mol<\/p>\n\n\n\n
5. Calculate the total moles of the solution<\/strong><\/h3>\n\n\n\nThe total number of moles in the solution is the sum of the moles of NaOH and the moles of water:Total moles=0.922\u2009mol NaOH+3.5\u2009mol water=4.422\u2009mol\\text{Total moles} = 0.922 \\, \\text{mol NaOH} + 3.5 \\, \\text{mol water} = 4.422 \\, \\text{mol}Total moles=0.922mol NaOH+3.5mol water=4.422mol<\/p>\n\n\n\n
6. Calculate the mole percent of NaOH<\/strong><\/h3>\n\n\n\nThe mole percent of NaOH is given by the ratio of the moles of NaOH to the total moles of the solution, multiplied by 100:Mole percent of NaOH=(Moles of NaOHTotal moles)\u00d7100=(0.9224.422)\u00d7100=20.85%\\text{Mole percent of NaOH} = \\left( \\frac{\\text{Moles of NaOH}}{\\text{Total moles}} \\right) \\times 100 = \\left( \\frac{0.922}{4.422} \\right) \\times 100 = 20.85\\%Mole percent of NaOH=(Total molesMoles of NaOH\u200b)\u00d7100=(4.4220.922\u200b)\u00d7100=20.85%<\/p>\n\n\n\n
Final Answer:<\/h3>\n\n\n\n
The mole percent of NaOH in the solution is 20.85%<\/strong>.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"An aqueous solution is 36.9% by mass sodium hydroxide and has a density of 1.03 g mL What is the mole percent of NaOH? The Correct Answer and Explanation is: To calculate the mole percent of sodium hydroxide (NaOH) in a 36.9% by mass aqueous NaOH solution with a density of 1.03 g\/mL, follow these […]<\/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-266277","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266277","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=266277"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266277\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=266277"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=266277"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=266277"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Now, calculate the moles of NaOH:Moles of NaOH=Mass of NaOHMolar Mass of NaOH=36.9\u2009g39.997\u2009g\/mol=0.922\u2009mol\\text{Moles of NaOH} = \\frac{\\text{Mass of NaOH}}{\\text{Molar Mass of NaOH}} = \\frac{36.9 \\, \\text{g}}{39.997 \\, \\text{g\/mol}} = 0.922 \\, \\text{mol}Moles of NaOH=Molar Mass of NaOHMass of NaOH\u200b=39.997g\/mol36.9g\u200b=0.922mol<\/p>\n\n\n\n
4. Calculate the moles of water (H\u2082O)<\/strong><\/h3>\n\n\n\nThe molar mass of water (H\u2082O) is:<\/p>\n\n\n\n
\n- H\u2082O: 2 \u00d7 1.008 (H) + 15.999 (O) = 18.015 g\/mol<\/li>\n<\/ul>\n\n\n\n
Now, calculate the moles of water:Moles of water=Mass of waterMolar Mass of water=63.1\u2009g18.015\u2009g\/mol=3.5\u2009mol\\text{Moles of water} = \\frac{\\text{Mass of water}}{\\text{Molar Mass of water}} = \\frac{63.1 \\, \\text{g}}{18.015 \\, \\text{g\/mol}} = 3.5 \\, \\text{mol}Moles of water=Molar Mass of waterMass of water\u200b=18.015g\/mol63.1g\u200b=3.5mol<\/p>\n\n\n\n
5. Calculate the total moles of the solution<\/strong><\/h3>\n\n\n\nThe total number of moles in the solution is the sum of the moles of NaOH and the moles of water:Total moles=0.922\u2009mol NaOH+3.5\u2009mol water=4.422\u2009mol\\text{Total moles} = 0.922 \\, \\text{mol NaOH} + 3.5 \\, \\text{mol water} = 4.422 \\, \\text{mol}Total moles=0.922mol NaOH+3.5mol water=4.422mol<\/p>\n\n\n\n
6. Calculate the mole percent of NaOH<\/strong><\/h3>\n\n\n\nThe mole percent of NaOH is given by the ratio of the moles of NaOH to the total moles of the solution, multiplied by 100:Mole percent of NaOH=(Moles of NaOHTotal moles)\u00d7100=(0.9224.422)\u00d7100=20.85%\\text{Mole percent of NaOH} = \\left( \\frac{\\text{Moles of NaOH}}{\\text{Total moles}} \\right) \\times 100 = \\left( \\frac{0.922}{4.422} \\right) \\times 100 = 20.85\\%Mole percent of NaOH=(Total molesMoles of NaOH\u200b)\u00d7100=(4.4220.922\u200b)\u00d7100=20.85%<\/p>\n\n\n\n
Final Answer:<\/h3>\n\n\n\n
The mole percent of NaOH in the solution is 20.85%<\/strong>.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"An aqueous solution is 36.9% by mass sodium hydroxide and has a density of 1.03 g mL What is the mole percent of NaOH? The Correct Answer and Explanation is: To calculate the mole percent of sodium hydroxide (NaOH) in a 36.9% by mass aqueous NaOH solution with a density of 1.03 g\/mL, follow these […]<\/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-266277","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266277","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=266277"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266277\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=266277"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=266277"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=266277"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Now, calculate the moles of water:Moles of water=Mass of waterMolar Mass of water=63.1\u2009g18.015\u2009g\/mol=3.5\u2009mol\\text{Moles of water} = \\frac{\\text{Mass of water}}{\\text{Molar Mass of water}} = \\frac{63.1 \\, \\text{g}}{18.015 \\, \\text{g\/mol}} = 3.5 \\, \\text{mol}Moles of water=Molar Mass of waterMass of water\u200b=18.015g\/mol63.1g\u200b=3.5mol<\/p>\n\n\n\n
5. Calculate the total moles of the solution<\/strong><\/h3>\n\n\n\nThe total number of moles in the solution is the sum of the moles of NaOH and the moles of water:Total moles=0.922\u2009mol NaOH+3.5\u2009mol water=4.422\u2009mol\\text{Total moles} = 0.922 \\, \\text{mol NaOH} + 3.5 \\, \\text{mol water} = 4.422 \\, \\text{mol}Total moles=0.922mol NaOH+3.5mol water=4.422mol<\/p>\n\n\n\n
6. Calculate the mole percent of NaOH<\/strong><\/h3>\n\n\n\nThe mole percent of NaOH is given by the ratio of the moles of NaOH to the total moles of the solution, multiplied by 100:Mole percent of NaOH=(Moles of NaOHTotal moles)\u00d7100=(0.9224.422)\u00d7100=20.85%\\text{Mole percent of NaOH} = \\left( \\frac{\\text{Moles of NaOH}}{\\text{Total moles}} \\right) \\times 100 = \\left( \\frac{0.922}{4.422} \\right) \\times 100 = 20.85\\%Mole percent of NaOH=(Total molesMoles of NaOH\u200b)\u00d7100=(4.4220.922\u200b)\u00d7100=20.85%<\/p>\n\n\n\n
Final Answer:<\/h3>\n\n\n\n
The mole percent of NaOH in the solution is 20.85%<\/strong>.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"An aqueous solution is 36.9% by mass sodium hydroxide and has a density of 1.03 g mL What is the mole percent of NaOH? The Correct Answer and Explanation is: To calculate the mole percent of sodium hydroxide (NaOH) in a 36.9% by mass aqueous NaOH solution with a density of 1.03 g\/mL, follow these […]<\/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-266277","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266277","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=266277"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266277\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=266277"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=266277"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=266277"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
The mole percent of NaOH is given by the ratio of the moles of NaOH to the total moles of the solution, multiplied by 100:Mole percent of NaOH=(Moles of NaOHTotal moles)\u00d7100=(0.9224.422)\u00d7100=20.85%\\text{Mole percent of NaOH} = \\left( \\frac{\\text{Moles of NaOH}}{\\text{Total moles}} \\right) \\times 100 = \\left( \\frac{0.922}{4.422} \\right) \\times 100 = 20.85\\%Mole percent of NaOH=(Total molesMoles of NaOH\u200b)\u00d7100=(4.4220.922\u200b)\u00d7100=20.85%<\/p>\n\n\n\n
Final Answer:<\/h3>\n\n\n\n
The mole percent of NaOH in the solution is 20.85%<\/strong>.<\/p>\n\n\n\n An aqueous solution is 36.9% by mass sodium hydroxide and has a density of 1.03 g mL What is the mole percent of NaOH? The Correct Answer and Explanation is: To calculate the mole percent of sodium hydroxide (NaOH) in a 36.9% by mass aqueous NaOH solution with a density of 1.03 g\/mL, follow these […]<\/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-266277","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266277","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=266277"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266277\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=266277"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=266277"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=266277"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}<\/figure>\n","protected":false},"excerpt":{"rendered":"