To calculate the mass of KMnO\u2084 (potassium permanganate)<\/strong> required to make 414 mL of a 0.02 M solution<\/strong>, follow these steps:<\/p>\n\n\n\n We need the volume in liters (L), because molarity (M) is moles per liter.414\u2009mL=0.414\u2009L414\\, \\text{mL} = 0.414\\, \\text{L}414mL=0.414L<\/p>\n\n\n\n Molarity (M) = moles of solute \/ liters of solution<\/p>\n\n\n\n Rearranged:moles of KMnO\u2084=M\u00d7V=0.02\u00d70.414=0.00828\u2009mol\\text{moles of KMnO\u2084} = M \\times V = 0.02 \\times 0.414 = 0.00828\\, \\text{mol}moles of KMnO\u2084=M\u00d7V=0.02\u00d70.414=0.00828mol<\/p>\n\n\n\n Use atomic masses from the periodic table:<\/p>\n\n\n\n Molar mass of KMnO\u2084=39.10+54.94+64.00=158.04\u2009g\/mol\\text{Molar mass of KMnO\u2084} = 39.10 + 54.94 + 64.00 = 158.04\\, \\text{g\/mol}Molar mass of KMnO\u2084=39.10+54.94+64.00=158.04g\/mol<\/p>\n\n\n\n Now use the number of moles and multiply by the molar mass:mass=moles\u00d7molar mass=0.00828\u00d7158.04=1.3073\u2009g\\text{mass} = \\text{moles} \\times \\text{molar mass} = 0.00828 \\times 158.04 = 1.3073\\, \\text{g}mass=moles\u00d7molar mass=0.00828\u00d7158.04=1.3073g<\/p>\n\n\n\n 1.3073\u2009g\\boxed{1.3073\\, \\text{g}}1.3073g\u200b<\/p>\n\n\n\n To prepare a chemical solution with precision, it is essential to use proper units and conversion steps. The molarity (M) represents the number of moles of solute per liter of solution. Here, we are given a volume of 414 milliliters, which needs to be converted to liters because the molarity unit includes liters, not milliliters.<\/p>\n\n\n\n After converting to 0.414 liters, we multiply this by the given molarity (0.02 M) to find the moles of KMnO\u2084 needed. This gives 0.00828 moles. Next, we calculate the molar mass of KMnO\u2084 by summing the atomic masses of potassium (K), manganese (Mn), and four oxygen (O) atoms. This totals 158.04 g\/mol.<\/p>\n\n\n\n Multiplying the number of moles by the molar mass gives us the mass of KMnO\u2084 required for the solution. This results in 1.3073 grams<\/strong>.<\/p>\n\n\n\n Since an analytical balance that reads to 0.0001 grams is used, the answer is rounded to four decimal places to ensure measurement precision. This approach ensures accurate and reliable preparation of a chemical solution, which is critical in laboratory settings where small errors can impact experimental outcomes.<\/p>\n\n\n\n Calculate the mass of KMnO(in g) required to make 414 mL of 0.02 M KMnOsolution. (Note: To make the concentration as accurate as possible, an analytical balance will be used to weigh KMnO. The analytical balance can read to 0.0001 g. So, keep four decimal places in the answer.) Answer: The Correct Answer and Explanation […]<\/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-38864","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/38864","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=38864"}],"version-history":[{"count":2,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/38864\/revisions"}],"predecessor-version":[{"id":38867,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/38864\/revisions\/38867"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=38864"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=38864"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=38864"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\nStep 1: Convert mL to L<\/strong><\/h3>\n\n\n\n
\n\n\n\nStep 2: Use the molarity formula<\/strong><\/h3>\n\n\n\n
\n\n\n\nStep 3: Find the molar mass of KMnO\u2084<\/strong><\/h3>\n\n\n\n
\n
\n\n\n\nStep 4: Calculate the mass<\/strong><\/h3>\n\n\n\n
\n\n\n\nFinal Answer:<\/strong><\/h3>\n\n\n\n
\n\n\n\nExplanation <\/strong><\/h3>\n\n\n\n
![\"\"](\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1075.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"