{"id":267186,"date":"2025-07-23T10:22:29","date_gmt":"2025-07-23T10:22:29","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=267186"},"modified":"2025-07-23T10:22:32","modified_gmt":"2025-07-23T10:22:32","slug":"silver-nitrate-can-react-with-potassium-chloride-in-aqueous-solution-to-produce-silver-chloride-as-shown","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/23\/silver-nitrate-can-react-with-potassium-chloride-in-aqueous-solution-to-produce-silver-chloride-as-shown\/","title":{"rendered":"Silver nitrate can react with potassium chloride in aqueous solution to produce silver chloride, as shown"},"content":{"rendered":"\n
Silver nitrate can react with potassium chloride in aqueous solution to produce silver chloride, as shown: AgNO3 (aq) + KCl(aq) --> AgCl(s) + KNO3 (aq) The reaction of 230 mL of AgNO3 (aq) with excess aqueous potassium chloride produces 14.70 g of precipitate. The concentration of the AgNO3(aq) solution is _________ mol\/L. answer to one digit after the decimal point<\/pre>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
To find the concentration of the AgNO3 solution, we will follow these steps:<\/p>\n\n\n\n
Step 1: Write the balanced equation<\/h3>\n\n\n\n
The given reaction is:AgNO3(aq)+KCl(aq)\u2192AgCl(s)+KNO3(aq)\\text{AgNO}_3 (aq) + \\text{KCl} (aq) \\rightarrow \\text{AgCl} (s) + \\text{KNO}_3 (aq)AgNO3\u200b(aq)+KCl(aq)\u2192AgCl(s)+KNO3\u200b(aq)<\/p>\n\n\n\n
This shows a 1:1 molar ratio between AgNO3 and AgCl.<\/p>\n\n\n\n
Step 2: Calculate moles of AgCl produced<\/h3>\n\n\n\n
We know the mass of AgCl precipitate is 14.70 g. To find the moles of AgCl, we use the molar mass of AgCl:Molar mass of AgCl=107.87\u2009g\/mol (Ag)+35.45\u2009g\/mol (Cl)=143.32\u2009g\/mol\\text{Molar mass of AgCl} = 107.87 \\, \\text{g\/mol (Ag)} + 35.45 \\, \\text{g\/mol (Cl)} = 143.32 \\, \\text{g\/mol}Molar mass of AgCl=107.87g\/mol (Ag)+35.45g\/mol (Cl)=143.32g\/mol<\/p>\n\n\n\n
Now calculate the moles of AgCl:Moles of AgCl=Mass of AgClMolar mass of AgCl=14.70\u2009g143.32\u2009g\/mol=0.1025\u2009mol\\text{Moles of AgCl} = \\frac{\\text{Mass of AgCl}}{\\text{Molar mass of AgCl}} = \\frac{14.70 \\, \\text{g}}{143.32 \\, \\text{g\/mol}} = 0.1025 \\, \\text{mol}Moles of AgCl=Molar mass of AgClMass of AgCl\u200b=143.32g\/mol14.70g\u200b=0.1025mol<\/p>\n\n\n\n
Step 3: Calculate moles of AgNO3<\/h3>\n\n\n\n
From the balanced equation, we know that 1 mole of AgNO3 produces 1 mole of AgCl. Therefore, the moles of AgNO3 are the same as the moles of AgCl:Moles of AgNO3=0.1025\u2009mol\\text{Moles of AgNO3} = 0.1025 \\, \\text{mol}Moles of AgNO3=0.1025mol<\/p>\n\n\n\n
Step 4: Calculate the concentration of AgNO3<\/h3>\n\n\n\n
We are given the volume of AgNO3 solution as 230 mL (or 0.230 L). The concentration (C) of AgNO3 is given by:C=Moles of AgNO3Volume of solution in liters=0.1025\u2009mol0.230\u2009L=0.4457\u2009mol\/LC = \\frac{\\text{Moles of AgNO3}}{\\text{Volume of solution in liters}} = \\frac{0.1025 \\, \\text{mol}}{0.230 \\, \\text{L}} = 0.4457 \\, \\text{mol\/L}C=Volume of solution in litersMoles of AgNO3\u200b=0.230L0.1025mol\u200b=0.4457mol\/L<\/p>\n\n\n\n
Final Answer:<\/h3>\n\n\n\n
The concentration of the AgNO3 solution is approximately 0.4 mol\/L<\/strong> when rounded to one decimal place.<\/p>\n\n\n\n
\"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
Silver nitrate can react with potassium chloride in aqueous solution to produce silver chloride, as shown: AgNO3 (aq) + KCl(aq) –> AgCl(s) + KNO3 (aq) The reaction of 230 mL of AgNO3 (aq) with excess aqueous potassium chloride produces 14.70 g of precipitate. The concentration of the AgNO3(aq) solution is _________ mol\/L. answer to one […]<\/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-267186","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267186","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=267186"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267186\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=267186"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=267186"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=267186"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}