{"id":38546,"date":"2025-06-26T10:46:33","date_gmt":"2025-06-26T10:46:33","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=38546"},"modified":"2025-06-26T10:46:35","modified_gmt":"2025-06-26T10:46:35","slug":"f-26-75-ml-of-0-03-m-permanganate-solution-mno4%e2%88%92-is-needed-to-oxidize-25-ml-of-unknown-fe2-solution-in-an-acidic-solution","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/f-26-75-ml-of-0-03-m-permanganate-solution-mno4%e2%88%92-is-needed-to-oxidize-25-ml-of-unknown-fe2-solution-in-an-acidic-solution\/","title":{"rendered":"f 26.75 mL of 0.03 M permanganate solution (MnO4\u2212) is needed to oxidize 25 mL of unknown\u00a0Fe2+\u00a0solution in an acidic solution"},"content":{"rendered":"\n
f 26.75 mL of 0.03 M permanganate solution (MnO4\u2212) is needed to oxidize 25 mL of unknown Fe2+ solution in an acidic solution<\/pre>\n\n\n\n
\"\"<\/figure>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
To solve the problem, we need to determine two things:<\/p>\n\n\n\n
    \n
  1. The molar concentration of Fe\u00b2\u207a<\/strong> in the unknown solution.<\/li>\n\n\n\n
  2. The molar mass of the Fe(II) compound<\/strong> used to prepare the solution.<\/li>\n<\/ol>\n\n\n\n
    Step 1: Write and balance the redox reaction<\/h3>\n\n\n\n
    In acidic conditions:<\/p>\n\n\n\n
    MnO4\u2212+5Fe2++8H+\u2192Mn2++5Fe3++4H2O\\text{MnO}_4^- + 5\\text{Fe}^{2+} + 8\\text{H}^+ \\rightarrow \\text{Mn}^{2+} + 5\\text{Fe}^{3+} + 4\\text{H}_2\\text{O}<\/p>\n\n\n\n
    This tells us that 1 mole of permanganate reacts with 5 moles of Fe\u00b2\u207a.<\/p>\n\n\n\n
    Step 2: Moles of MnO\u2084\u207b used<\/h3>\n\n\n\n
    Given volume = 26.75 mL = 0.02675 L Given concentration = 0.03 mol\/L<\/p>\n\n\n\n
    Moles MnO4\u2212=0.03\u00d70.02675=8.025\u00d710\u22124 mol\\text{Moles MnO}_4^- = 0.03 \\times 0.02675 = 8.025 \\times 10^{-4} \\text{ mol}<\/p>\n\n\n\n
    Step 3: Moles of Fe\u00b2\u207a in 25 mL solution<\/h3>\n\n\n\n
    From the balanced equation,<\/p>\n\n\n\n
    Moles Fe2+=5\u00d7Moles MnO4\u2212=5\u00d78.025\u00d710\u22124=0.0040125 mol\\text{Moles Fe}^{2+} = 5 \\times \\text{Moles MnO}_4^- = 5 \\times 8.025 \\times 10^{-4} = 0.0040125 \\text{ mol}<\/p>\n\n\n\n
    Now calculate molar concentration of Fe\u00b2\u207a<\/strong> in 25 mL = 0.025 L:<\/p>\n\n\n\n
    Concentration of Fe2+=0.00401250.025=0.1605 mol\/L\\text{Concentration of Fe}^{2+} = \\frac{0.0040125}{0.025} = 0.1605 \\text{ mol\/L}<\/p>\n\n\n\n
    Step 4: Determine molar mass<\/h3>\n\n\n\n
    Given mass of Fe(II) compound = 0.72 g<\/p>\n\n\n\n
    Molar mass=0.72 g0.0040125 mol\u2248179.4 g\/mol\\text{Molar mass} = \\frac{0.72 \\text{ g}}{0.0040125 \\text{ mol}} \\approx 179.4 \\text{ g\/mol}<\/p>\n\n\n\n
    Step 5: Identify compound and calculate percent error<\/h3>\n\n\n\n
    From the table, the closest match is FeSO\u2084\u00b74H\u2082O (169.93 g\/mol)<\/strong>.<\/p>\n\n\n\n
    Percent error=\u2223179.4\u2212169.93\u2223169.93\u00d7100\u22485.57%\\text{Percent error} = \\frac{|179.4 – 169.93|}{169.93} \\times 100 \\approx 5.57\\%<\/p>\n\n\n\n
    Final Answers:<\/h3>\n\n\n\n
      \n
    • [Fe\u00b2\u207a] = 0.1605 mol\/L<\/strong><\/li>\n\n\n\n
    • Molar mass = 179.4 g\/mol<\/strong><\/li>\n\n\n\n
    • Closest match: FeSO\u2084\u00b74H\u2082O<\/strong><\/li>\n\n\n\n
    • Percent error = 5.57%<\/strong><\/li>\n<\/ul>\n\n\n\n
      \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
      f 26.75 mL of 0.03 M permanganate solution (MnO4\u2212) is needed to oxidize 25 mL of unknown Fe2+ solution in an acidic solution The Correct Answer and Explanation is: To solve the problem, we need to determine two things: Step 1: Write and balance the redox reaction In acidic conditions: MnO4\u2212+5Fe2++8H+\u2192Mn2++5Fe3++4H2O\\text{MnO}_4^- + 5\\text{Fe}^{2+} + 8\\text{H}^+ \\rightarrow \\text{Mn}^{2+} […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-38546","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/38546","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=38546"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/38546\/revisions"}],"predecessor-version":[{"id":38579,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/38546\/revisions\/38579"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=38546"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=38546"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=38546"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}