Calculate the mass of potassium hydrogen phthalate, KHC8H4O4 (MM is 204.2 g\/mol) needed to react completely with 20 mL of 0.1 M NaOH solution.<\/p>\n\n\n\n
The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n Answer:<\/strong><\/p>\n\n\n\n To find the mass of potassium hydrogen phthalate (KHP)<\/strong> needed to react with 20 mL of 0.1 M NaOH<\/strong>, we use stoichiometry.<\/p>\n\n\n\n KHP (KHC\u2088H\u2084O\u2084) is a monoprotic acid<\/strong>; it donates one proton:<\/p>\n\n\n\n $$ This shows a 1:1 molar ratio<\/strong> between KHP and NaOH.<\/p>\n\n\n\n $$ $$ $$ Potassium hydrogen phthalate (KHC\u2088H\u2084O\u2084), commonly known as KHP, is a solid, acidic compound often used as a primary standard<\/strong> in acid-base titrations because of its high purity and stable molecular weight. In this case, KHP is being used to neutralize a sodium hydroxide (NaOH) solution<\/strong>, allowing precise determination of the amount of base present or required.<\/p>\n\n\n\n To find out how much KHP is required to react with a known amount of NaOH, we first write the balanced chemical equation. Since KHP contains one acidic hydrogen, it reacts with NaOH in a 1:1 molar ratio. This is key to determining how many moles of KHP are needed.<\/p>\n\n\n\n Given 20 mL (or 0.020 L) of a 0.1 M NaOH solution, we calculate the moles of NaOH using the formula:<\/p>\n\n\n\n $$ Because of the 1:1 ratio, 0.002 mol of KHP are required to completely react with the NaOH. The mass of KHP can be found by multiplying these moles by its molar mass, which is 204.2 g\/mol:<\/p>\n\n\n\n $$ Therefore, 0.4084 grams<\/strong> of KHP are required to exactly neutralize 20 mL of 0.1 M NaOH. This calculation is essential in standardizing NaOH solutions accurately in laboratory settings. Would you like a visual diagram of this reaction and calculation?<\/p>\n","protected":false},"excerpt":{"rendered":" Calculate the mass of potassium hydrogen phthalate, KHC8H4O4 (MM is 204.2 g\/mol) needed to react completely with 20 mL of 0.1 M NaOH solution. The correct answer and explanation is : Answer: To find the mass of potassium hydrogen phthalate (KHP) needed to react with 20 mL of 0.1 M NaOH, we use stoichiometry. Step […]<\/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-210831","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/210831","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=210831"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/210831\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=210831"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=210831"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=210831"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\nStep 1: Write the balanced reaction<\/strong><\/h3>\n\n\n\n
\\text{KHC}_8\\text{H}_4\\text{O}_4 + \\text{NaOH} \\rightarrow \\text{KNaC}_8\\text{H}_4\\text{O}_4 + \\text{H}_2\\text{O}
$$<\/p>\n\n\n\n
\n\n\n\nStep 2: Calculate moles of NaOH<\/strong><\/h3>\n\n\n\n
\\text{Moles of NaOH} = Molarity \\times Volume (L) = 0.1\\ \\text{mol\/L} \\times 0.020\\ \\text{L} = 0.002\\ \\text{mol}
$$<\/p>\n\n\n\n
\n\n\n\nStep 3: Use 1:1 ratio to find moles of KHP<\/strong><\/h3>\n\n\n\n
\\text{Moles of KHP} = 0.002\\ \\text{mol}
$$<\/p>\n\n\n\n
\n\n\n\nStep 4: Calculate mass of KHP<\/strong><\/h3>\n\n\n\n
\\text{Mass} = \\text{Moles} \\times \\text{Molar Mass} = 0.002\\ \\text{mol} \\times 204.2\\ \\text{g\/mol} = \\boxed{0.4084\\ \\text{g}}
$$<\/p>\n\n\n\n
\n\n\n\nExplanation (300 words)<\/strong><\/h2>\n\n\n\n
\\text{moles} = M \\times V = 0.1\\ \\text{mol\/L} \\times 0.020\\ \\text{L} = 0.002\\ \\text{mol}
$$<\/p>\n\n\n\n
\\text{Mass} = 0.002 \\times 204.2 = 0.4084\\ \\text{g}
$$<\/p>\n\n\n\n