{"id":195733,"date":"2025-02-28T17:30:31","date_gmt":"2025-02-28T17:30:31","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=195733"},"modified":"2025-02-28T17:30:34","modified_gmt":"2025-02-28T17:30:34","slug":"a-solution-of-kci-is-saturated-at-50c","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/28\/a-solution-of-kci-is-saturated-at-50c\/","title":{"rendered":"A solution of KCI is saturated at 50\u00b0C"},"content":{"rendered":"\n

A solution of KCI is saturated at 50\u00b0C. Use Table 9.1<\/p>\n\n\n\n

(a) How many grams of solute are dissolved in 100 g of water?<\/p>\n\n\n\n

(b) What is the total mass of the solution?<\/p>\n\n\n\n

(c) What is the mass percent of this solution at 50\u00b0C?<\/p>\n\n\n\n

(d) If the solution is heated to 100\u00b0C, how much more KCl can be dissolved in the solu- tion without adding more water?<\/p>\n\n\n\n

(e) If the solution is saturated at 100\u00baC and then cooled to 30\u00b0C, how many grams of solute will precipitate out?<\/p>\n\n\n\n

Table 9.1
Temperature Effect on Solubility of Four Salts in Water, g solute\/100 g water<\/p>\n\n\n\n

 <\/td><\/td><\/td><\/td><\/td><\/td><\/td><\/td><\/td><\/td><\/td><\/td><\/tr>
<\/td>27.6<\/td>31.0<\/td>34.0<\/td>37.0<\/td>40.0<\/td>42.6<\/td>45.5<\/td>48.3<\/td>51.1<\/td>54.0<\/td>55.6<\/td><\/tr>
<\/td>35.7<\/td>35.8<\/td>36.0<\/td>36.3<\/td>36.6<\/td>37.0<\/td>37.3<\/td>37.8<\/td>38.4<\/td>39.0<\/td>39.8<\/td><\/tr>
<\/td>53.5<\/td>59.5<\/td>65.2<\/td>70.6<\/td>75.5<\/td>80.2<\/td>85.5<\/td>90.0<\/td>95.0<\/td>99.2<\/td>104.0<\/td><\/tr>
<\/td>31.6<\/td>33.3<\/td>35.7<\/td>38.2<\/td>40.7<\/td>43.6<\/td>46.6<\/td>49.4<\/td>52.6<\/td>55.7<\/td>58.8<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

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

Based on Table 9.1, we will analyze the solubility of KCl in water at different temperatures and answer each question accordingly.<\/p>\n\n\n\n

Given Solubility Data:<\/h3>\n\n\n\n
    \n
  • At 50\u00b0C<\/strong>, the solubility of KCl is 42.6 g per 100 g of water<\/strong>.<\/li>\n\n\n\n
  • At 100\u00b0C<\/strong>, the solubility of KCl is 55.6 g per 100 g of water<\/strong>.<\/li>\n\n\n\n
  • At 30\u00b0C<\/strong>, the solubility of KCl is 37.0 g per 100 g of water<\/strong>.<\/li>\n<\/ul>\n\n\n\n

    (a) How many grams of solute are dissolved in 100 g of water?<\/h3>\n\n\n\n

    From the table, at 50\u00b0C<\/strong>, the solubility of KCl is 42.6 g per 100 g of water<\/strong>. This means in 100 g of water, 42.6 g of KCl<\/strong> is dissolved.<\/p>\n\n\n\n

    (b) What is the total mass of the solution?<\/h3>\n\n\n\n

    The solution consists of 100 g of water<\/strong> and 42.6 g of KCl<\/strong>. Total mass=100+42.6=142.6 g\\text{Total mass} = 100 + 42.6 = 142.6 \\text{ g}<\/p>\n\n\n\n

    (c) What is the mass percent of this solution at 50\u00b0C?<\/h3>\n\n\n\n

    Mass percent of KCl is calculated as: mass of solutetotal mass of solution\u00d7100\\frac{\\text{mass of solute}}{\\text{total mass of solution}} \\times 100 42.6142.6\u00d7100=29.9%\\frac{42.6}{142.6} \\times 100 = 29.9\\%<\/p>\n\n\n\n

    So, the mass percent is 29.9%<\/strong>.<\/p>\n\n\n\n

    (d) If the solution is heated to 100\u00b0C, how much more KCl can be dissolved without adding more water?<\/h3>\n\n\n\n

    At 100\u00b0C<\/strong>, the solubility of KCl is 55.6 g per 100 g of water<\/strong>. Since we already have 42.6 g<\/strong> dissolved, the additional amount that can dissolve is: 55.6\u221242.6=13.0 g55.6 – 42.6 = 13.0 \\text{ g}<\/p>\n\n\n\n

    So, 13.0 g more KCl<\/strong> can be dissolved.<\/p>\n\n\n\n

    (e) If the solution is saturated at 100\u00b0C and then cooled to 30\u00b0C, how many grams of solute will precipitate out?<\/h3>\n\n\n\n

    At 100\u00b0C<\/strong>, the solution contains 55.6 g of KCl per 100 g of water<\/strong>. When cooled to 30\u00b0C<\/strong>, the solubility decreases to 37.0 g per 100 g of water<\/strong>. The amount of KCl that precipitates is: 55.6\u221237.0=18.6 g55.6 – 37.0 = 18.6 \\text{ g}<\/p>\n\n\n\n

    So, 18.6 g of KCl will precipitate out<\/strong>.<\/p>\n\n\n\n

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

    Solubility is the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature. The solubility of KCl increases with temperature, meaning more KCl dissolves at higher temperatures. When a saturated solution is cooled, the solubility decreases, causing the excess solute to precipitate out. This is why when a 100\u00b0C saturated solution is cooled to 30\u00b0C, 18.6 g of KCl precipitates<\/strong>.<\/p>\n\n\n\n

    Now, I’ll generate an image to illustrate the solubility trend of KCl.<\/p>\n\n\n\n

    Here is a graph illustrating the solubility of KCl in water at different temperatures. The red points highlight key temperatures mentioned in the problem: 30\u00b0C, 50\u00b0C, and 100\u00b0C<\/strong>, where changes in solubility affect precipitation and dissolution of KCl. Let me know if you need any further clarification!<\/p>\n\n\n\n

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

    A solution of KCI is saturated at 50\u00b0C. Use Table 9.1 (a) How many grams of solute are dissolved in 100 g of water? (b) What is the total mass of the solution? (c) What is the mass percent of this solution at 50\u00b0C? (d) If the solution is heated to 100\u00b0C, how much more […]<\/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-195733","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/195733","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=195733"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/195733\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=195733"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=195733"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=195733"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}