{"id":208376,"date":"2025-04-26T13:58:44","date_gmt":"2025-04-26T13:58:44","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=208376"},"modified":"2025-04-26T13:58:46","modified_gmt":"2025-04-26T13:58:46","slug":"how-many-grams-of-ironiii-nitrate-feno33","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/04\/26\/how-many-grams-of-ironiii-nitrate-feno33\/","title":{"rendered":"How many grams of iron(III) nitrate (Fe(NO3)3"},"content":{"rendered":"\n

How many grams of iron(III) nitrate (Fe(NO3)3, molar mass=241.88 g\/mol) are required to make 198.0 mL of a 0.130 M solution? Enter<\/p>\n\n\n\n

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

To determine the grams of iron(III) nitrate (Fe(NO\u2083)\u2083) required to make 198.0 mL of a 0.130 M solution, we need to follow these steps:<\/p>\n\n\n\n

1. Use the formula for molarity:<\/h3>\n\n\n\n

Molarity (M) is defined as the number of moles of solute (in this case, Fe(NO\u2083)\u2083) per liter of solution. The formula is:<\/p>\n\n\n\n

[
\\text{Molarity (M)} = \\frac{\\text{moles of solute}}{\\text{volume of solution (L)}}
]<\/p>\n\n\n\n

Rearranging this formula to find moles of solute:<\/p>\n\n\n\n

[
\\text{moles of solute} = \\text{Molarity (M)} \\times \\text{Volume (L)}
]<\/p>\n\n\n\n

2. Convert volume to liters:<\/h3>\n\n\n\n

Given that the volume of the solution is 198.0 mL, we first convert it to liters:<\/p>\n\n\n\n

[
198.0 \\, \\text{mL} = 198.0 \\, \\text{mL} \\times \\frac{1 \\, \\text{L}}{1000 \\, \\text{mL}} = 0.198 \\, \\text{L}
]<\/p>\n\n\n\n

3. Calculate moles of Fe(NO\u2083)\u2083:<\/h3>\n\n\n\n

Now, using the given molarity of 0.130 M and the volume in liters (0.198 L), we can calculate the moles of iron(III) nitrate:<\/p>\n\n\n\n

[
\\text{moles of Fe(NO\u2083)\u2083} = 0.130 \\, \\text{M} \\times 0.198 \\, \\text{L} = 0.02574 \\, \\text{moles}
]<\/p>\n\n\n\n

4. Convert moles to grams:<\/h3>\n\n\n\n

To find the mass of Fe(NO\u2083)\u2083 required, we use the molar mass of Fe(NO\u2083)\u2083, which is given as 241.88 g\/mol. The mass can be calculated as:<\/p>\n\n\n\n

[
\\text{mass of Fe(NO\u2083)\u2083} = \\text{moles of Fe(NO\u2083)\u2083} \\times \\text{molar mass}
]<\/p>\n\n\n\n

[
\\text{mass of Fe(NO\u2083)\u2083} = 0.02574 \\, \\text{moles} \\times 241.88 \\, \\text{g\/mol} = 6.23 \\, \\text{grams}
]<\/p>\n\n\n\n

Final Answer:<\/h3>\n\n\n\n

You need 6.23 grams<\/strong> of iron(III) nitrate (Fe(NO\u2083)\u2083) to make 198.0 mL of a 0.130 M solution.<\/p>\n\n\n\n

Explanation:<\/h3>\n\n\n\n
    \n
  • Step 1<\/strong>: We use the molarity equation to relate the amount of solute (in moles) to the volume of solution.<\/li>\n\n\n\n
  • Step 2<\/strong>: We converted the volume from mL to L to align with the molarity unit of L.<\/li>\n\n\n\n
  • Step 3<\/strong>: The moles of Fe(NO\u2083)\u2083 were calculated by multiplying the molarity (0.130 M) by the volume in liters (0.198 L).<\/li>\n\n\n\n
  • Step 4<\/strong>: To convert moles to grams, we used the molar mass (241.88 g\/mol) and multiplied it by the number of moles. This gives the required mass in grams.<\/li>\n<\/ul>\n\n\n\n

    Thus, the answer is clear and shows all the required steps to arrive at the final value of 6.23 grams of Fe(NO\u2083)\u2083 needed.<\/p>\n","protected":false},"excerpt":{"rendered":"

    How many grams of iron(III) nitrate (Fe(NO3)3, molar mass=241.88 g\/mol) are required to make 198.0 mL of a 0.130 M solution? Enter The correct answer and explanation is : To determine the grams of iron(III) nitrate (Fe(NO\u2083)\u2083) required to make 198.0 mL of a 0.130 M solution, we need to follow these steps: 1. Use […]<\/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-208376","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/208376","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=208376"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/208376\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=208376"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=208376"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=208376"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}