{"id":191101,"date":"2025-02-14T07:11:37","date_gmt":"2025-02-14T07:11:37","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=191101"},"modified":"2025-02-14T07:11:39","modified_gmt":"2025-02-14T07:11:39","slug":"for-an-aqueous-solution-of-hf","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/14\/for-an-aqueous-solution-of-hf\/","title":{"rendered":"For an aqueous solution of HF"},"content":{"rendered":"\n

For an aqueous solution of HF, determine the van’t Hoff factor assuming\u2026 A solution is made by dissolving 0.0300 mol of HF in 1.00 kg of water. The solution was found to freeze at -0.0644 degree C. Calculate the value of i and estimate the percent ionization of HF in this solution.<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

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

I cannot access the URL you’ve provided, but I can still guide you through solving the problem step by step!<\/p>\n\n\n\n

Step 1: Freezing Point Depression Equation<\/h3>\n\n\n\n

To calculate the van’t Hoff factor (i) and percent ionization of HF, we will use the freezing point depression formula:<\/p>\n\n\n\n

[
\\Delta T_f = i \\cdot K_f \\cdot m
]<\/p>\n\n\n\n

Where:<\/p>\n\n\n\n

    \n
  • (\\Delta T_f) is the freezing point depression, which is the difference between the freezing point of pure water (0\u00b0C) and the freezing point of the solution.<\/li>\n\n\n\n
  • (i) is the van’t Hoff factor, which represents the number of particles the solute dissociates into.<\/li>\n\n\n\n
  • (K_f) is the cryoscopic constant (freezing point depression constant) for water, which is 1.86\u00b0C\u00b7kg\/mol.<\/li>\n\n\n\n
  • (m) is the molality of the solution, defined as moles of solute per kilogram of solvent.<\/li>\n<\/ul>\n\n\n\n

    Step 2: Calculate Freezing Point Depression<\/h3>\n\n\n\n

    The freezing point of pure water is 0\u00b0C. The solution freezes at -0.0644\u00b0C, so the freezing point depression is:<\/p>\n\n\n\n

    [
    \\Delta T_f = 0\u00b0C – (-0.0644\u00b0C) = 0.0644\u00b0C
    ]<\/p>\n\n\n\n

    Step 3: Determine Molality<\/h3>\n\n\n\n

    The molality (m) is given by:<\/p>\n\n\n\n

    [
    m = \\frac{\\text{moles of solute}}{\\text{mass of solvent in kg}} = \\frac{0.0300 \\text{ mol}}{1.00 \\text{ kg}} = 0.0300 \\text{ mol\/kg}
    ]<\/p>\n\n\n\n

    Step 4: Use the Freezing Point Depression Equation<\/h3>\n\n\n\n

    Now, we can plug values into the equation:<\/p>\n\n\n\n

    [
    0.0644\u00b0C = i \\cdot 1.86 \\cdot 0.0300
    ]<\/p>\n\n\n\n

    Solve for (i):<\/p>\n\n\n\n

    [
    i = \\frac{0.0644}{1.86 \\cdot 0.0300} = \\frac{0.0644}{0.0558} = 1.15
    ]<\/p>\n\n\n\n

    Step 5: Estimate Percent Ionization<\/h3>\n\n\n\n

    HF is a weak acid and only partially dissociates in water. The van’t Hoff factor (i) corresponds to the number of ions in solution. For HF, the dissociation is:<\/p>\n\n\n\n

    [
    \\text{HF} \\rightleftharpoons \\text{H}^+ + \\text{F}^-
    ]<\/p>\n\n\n\n

    For 100% ionization, (i = 2) (one HF molecule dissociates into two ions). The observed value of (i = 1.15) suggests partial dissociation. The percent ionization can be calculated by comparing the observed (i) to the expected value for full dissociation:<\/p>\n\n\n\n

    [
    \\text{Percent Ionization} = \\left( \\frac{i – 1}{1} \\right) \\times 100 = (1.15 – 1) \\times 100 = 15\\%
    ]<\/p>\n\n\n\n

    Conclusion<\/h3>\n\n\n\n
      \n
    • The van’t Hoff factor (i) is 1.15.<\/li>\n\n\n\n
    • The percent ionization of HF in the solution is approximately 15%.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"

      For an aqueous solution of HF, determine the van’t Hoff factor assuming\u2026 A solution is made by dissolving 0.0300 mol of HF in 1.00 kg of water. The solution was found to freeze at -0.0644 degree C. Calculate the value of i and estimate the percent ionization of HF in this solution. The Correct Answer […]<\/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-191101","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191101","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=191101"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191101\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=191101"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=191101"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=191101"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}