{"id":182309,"date":"2025-01-13T16:15:46","date_gmt":"2025-01-13T16:15:46","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=182309"},"modified":"2025-01-13T16:15:48","modified_gmt":"2025-01-13T16:15:48","slug":"solutions-of-ironiii-chloride-and-sodium-hydroxide-were-mixed-in-a-series-of-precipita-tion-reactions","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/13\/solutions-of-ironiii-chloride-and-sodium-hydroxide-were-mixed-in-a-series-of-precipita-tion-reactions\/","title":{"rendered":"Solutions of iron(III) chloride and sodium hydroxide were mixed in a series of precipita- tion reactions"},"content":{"rendered":"\n

Solutions of iron(III) chloride and sodium hydroxide were mixed in a series of precipita- tion reactions, as described in this experiment. (a) Name the two possible products in this precipitation reaction and predict their empir- ical formulas. (b) Which product is likely to be insoluble in water and precipitate out as a red solid? (c) What volume ratio of reactants gave the most precipitate (see Table 1)? Explain. Table 1. Test tube. 1 2. 3 6. FeCl,, 0.1 M, mL 5 10 12 15 17 20 24 NaOH, 0.1 M, mL 55 50 48 45 43 40 36 Volume of precipitate, mL 1 10 14 20 4 1<\/p>\n\n\n\n

The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n

When solutions of iron(III) chloride (FeCl\u2083) and sodium hydroxide (NaOH) are mixed, a precipitation reaction occurs, leading to the formation of iron(III) hydroxide (Fe(OH)\u2083) and sodium chloride (NaCl).<\/p>\n\n\n\n

(a) Name the two possible products in this precipitation reaction and predict their empirical formulas.<\/strong><\/p>\n\n\n\n

The two products are:<\/p>\n\n\n\n

    \n
  1. Iron(III) hydroxide<\/strong>: This compound forms as a reddish-brown precipitate when NaOH is added to FeCl\u2083. Its empirical formula is Fe(OH)\u2083.<\/li>\n\n\n\n
  2. Sodium chloride<\/strong>: This is a soluble salt formed in the reaction. Its empirical formula is NaCl.<\/li>\n<\/ol>\n\n\n\n

    (b) Which product is likely to be insoluble in water and precipitate out as a red solid?<\/strong><\/p>\n\n\n\n

    Iron(III) hydroxide (Fe(OH)\u2083) is insoluble in water and precipitates out as a reddish-brown solid when NaOH is added to FeCl\u2083.<\/p>\n\n\n\n

    (c) What volume ratio of reactants gave the most precipitate (see Table 1)? Explain.<\/strong><\/p>\n\n\n\n

    To determine the volume ratio of FeCl\u2083 to NaOH that produced the most precipitate, we need to analyze the data provided in Table 1:<\/p>\n\n\n\n

    Test Tube<\/th>FeCl\u2083 (0.1 M) Volume (mL)<\/th>NaOH (0.1 M) Volume (mL)<\/th>Volume of Precipitate (mL)<\/th><\/tr><\/thead>
    1<\/td>5<\/td>55<\/td>1<\/td><\/tr>
    2<\/td>10<\/td>50<\/td>10<\/td><\/tr>
    3<\/td>12<\/td>48<\/td>14<\/td><\/tr>
    4<\/td>15<\/td>45<\/td>20<\/td><\/tr>
    5<\/td>17<\/td>43<\/td>4<\/td><\/tr>
    6<\/td>20<\/td>40<\/td>1<\/td><\/tr>
    7<\/td>24<\/td>36<\/td>0<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

    From the table, the maximum volume of precipitate (20 mL) was obtained in Test Tube 4, where 15 mL of FeCl\u2083 solution was mixed with 45 mL of NaOH solution.<\/p>\n\n\n\n

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

    The precipitation reaction between FeCl\u2083 and NaOH is governed by the stoichiometric relationship:<\/p>\n\n\n\n

    [ \\text{FeCl}_3 + 3\\text{NaOH} \\rightarrow \\text{Fe(OH)}_3 + 3\\text{NaCl} ]<\/p>\n\n\n\n

    This equation indicates that one mole of FeCl\u2083 reacts with three moles of NaOH.<\/p>\n\n\n\n

    In Test Tube 4, the molar amounts of FeCl\u2083 and NaOH are:<\/p>\n\n\n\n

      \n
    • FeCl\u2083: ( 0.1\\,\\text{M} \\times 0.015\\,\\text{L} = 0.0015\\,\\text{mol} )<\/li>\n\n\n\n
    • NaOH: ( 0.1\\,\\text{M} \\times 0.045\\,\\text{L} = 0.0045\\,\\text{mol} )<\/li>\n<\/ul>\n\n\n\n

      The molar ratio of FeCl\u2083 to NaOH is 1:3, which matches the stoichiometric requirement. This optimal ratio ensures that both reactants are completely consumed, leading to the maximum formation of Fe(OH)\u2083 precipitate.<\/p>\n\n\n\n

      In other test tubes, deviations from this ratio result in less precipitate formation. For example, in Test Tube 5, the molar ratio is approximately 1:2.53, leading to only 4 mL of precipitate. In Test Tube 7, the molar ratio is about 1:1.5, resulting in no precipitate formation.<\/p>\n\n\n\n

      Therefore, the volume ratio of FeCl\u2083 to NaOH that produced the most precipitate is 1:3, corresponding to Test Tube 4.<\/p>\n","protected":false},"excerpt":{"rendered":"

      Solutions of iron(III) chloride and sodium hydroxide were mixed in a series of precipita- tion reactions, as described in this experiment. (a) Name the two possible products in this precipitation reaction and predict their empir- ical formulas. (b) Which product is likely to be insoluble in water and precipitate out as a red solid? (c) […]<\/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-182309","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182309","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=182309"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182309\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=182309"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=182309"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=182309"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}