Calculate the mass of citric acid required to make 50.0 mL of a 0.100 M solution. The formula of citric acid is H3C6H507. The formula weight of citric acid is Why must NaOH solutions be standardized before being used to do titrations? What indicator is used for the titrations of this experiment? What is its color change? \u2022 If you accidentally forgot to rinse out the 10mL graduated cylinder after measuring the citric acid, what effect would this have on the NaOH placed in the cylinder? Calculate the molarity of the citric acid solution prepared by dissolving 1.0 gram of citric acid in 50.0 mL of solution. The formula of citric acid is H3C6H507. Data and Results Table for the Titration of NaOH with citric acid Data or Calculation Trial 1 Trial 2 Trial 3 (if necessary) Vol Citric acid 3.0 ml 3.0 mL Moles citric acid (calc) Volume NaOH (initial reading) Volume NaOH (final reading) Volume NaOH used (calc) Moles NaOH (calc) Molarity NaOH (calc) Balance the chemical equation for the reaction of citric acid and sodium hydroxide. H3C6H507 + NaOH H2O + Na3C6H507 Show detailed calculations that include units for the following: Moles citric acid Moles NaOH Molarity of NaOH. Average Molarity of NaOH Data and Results Table for the Titration of Diluted Vinegar with NaOH Data or Calculation Trial 1 Trial 2 Trial 3 (if necessary) Volume diluted Vinegar Volume NaOH (initial) Volume NaOH (final) Volume NaOH used (calc) Moles NaOH (calc) Moles HC2H302 (calc) Molarity of HC2H302 (calc) Balance the chemical equation for the reaction of citric acid and sodium hydroxide. HC2H302 + NaOH H2O + NaC2H302 Show detailed calculations that include units for the following: Moles NaOH Moles acetic acid Molarity of acetic acid in diluted vinegar. Molarity of acetic acid in vinegar.<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n Here\u2019s the breakdown of the calculations and explanations for the provided chemistry questions:<\/p>\n\n\n\n To make a 0.100 M solution of citric acid (H\u2083C\u2086H\u2085O\u2087), we use: NaOH is hygroscopic, meaning it absorbs moisture from the air, which can alter its concentration. Standardizing ensures the actual concentration is known for accurate titrations.<\/p>\n\n\n\n Phenolphthalein is commonly used. It changes from colorless (acidic)<\/strong> to pink (basic)<\/strong>.<\/p>\n\n\n\n Residual citric acid would react with NaOH, consuming more NaOH than necessary. This would lead to an overestimation of NaOH concentration.<\/p>\n\n\n\n Given 1.0 g citric acid in 50.0 mL: [ Using the reaction stoichiometry, 3 moles of NaOH react with 1 mole of citric acid.<\/p>\n\n\n\n [ [ [ 1 mole NaOH reacts with 1 mole HC\u2082H\u2083O\u2082.<\/p>\n\n\n\n [ Account for dilution factor.<\/p>\n\n\n\n These calculations ensure precise results for titration experiments, highlighting the importance of standardization, clean equipment, and proper stoichiometric relationships.<\/p>\n","protected":false},"excerpt":{"rendered":" Calculate the mass of citric acid required to make 50.0 mL of a 0.100 M solution. The formula of citric acid is H3C6H507. The formula weight of citric acid is Why must NaOH solutions be standardized before being used to do titrations? What indicator is used for the titrations of this experiment? What is its […]<\/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-186942","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186942","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=186942"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186942\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=186942"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=186942"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=186942"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\n1. Mass of Citric Acid Required<\/strong><\/h3>\n\n\n\n
[
\\text{Molarity (M)} = \\frac{\\text{moles}}{\\text{volume (L)}}
]
Rearranging for moles:
[
\\text{moles} = \\text{Molarity} \\times \\text{volume (L)} = 0.100 \\, \\text{M} \\times 0.0500 \\, \\text{L} = 0.00500 \\, \\text{moles}
]
Mass of citric acid:
[
\\text{mass} = \\text{moles} \\times \\text{molar mass (192.12 g\/mol)} = 0.00500 \\, \\text{mol} \\times 192.12 \\, \\text{g\/mol} = 0.9606 \\, \\text{g}
]
Answer:<\/strong> 0.9606 g of citric acid is required.<\/p>\n\n\n\n
\n\n\n\n2. Why Standardize NaOH?<\/strong><\/h3>\n\n\n\n
\n\n\n\n3. Indicator and Color Change<\/strong><\/h3>\n\n\n\n
\n\n\n\n4. Effect of Not Rinsing Graduated Cylinder<\/strong><\/h3>\n\n\n\n
\n\n\n\n5. Molarity of Citric Acid Solution<\/strong><\/h3>\n\n\n\n
Moles of citric acid:
[
\\text{moles} = \\frac{\\text{mass}}{\\text{molar mass}} = \\frac{1.0 \\, \\text{g}}{192.12 \\, \\text{g\/mol}} = 0.00521 \\, \\text{mol}
]
Molarity:
[
\\text{Molarity} = \\frac{\\text{moles}}{\\text{volume (L)}} = \\frac{0.00521 \\, \\text{mol}}{0.0500 \\, \\text{L}} = 0.1042 \\, \\text{M}
]
Answer:<\/strong> 0.104 M<\/p>\n\n\n\n
\n\n\n\n6. Balanced Chemical Equations<\/strong><\/h3>\n\n\n\n
\n
[
\\text{H\u2083C\u2086H\u2085O\u2087 + 3NaOH \u2192 Na\u2083C\u2086H\u2085O\u2087 + 3H\u2082O}
]<\/li>\n\n\n\n
[
\\text{HC\u2082H\u2083O\u2082 + NaOH \u2192 NaC\u2082H\u2083O\u2082 + H\u2082O}
]<\/li>\n<\/ol>\n\n\n\n
\n\n\n\n7. Calculations for Titrations<\/strong><\/h3>\n\n\n\n
Moles of Citric Acid:<\/h4>\n\n\n\n
\\text{moles} = \\text{Molarity} \\times \\text{volume (L)}
]<\/p>\n\n\n\nMoles of NaOH:<\/h4>\n\n\n\n
Molarity of NaOH:<\/h4>\n\n\n\n
\\text{Molarity (NaOH)} = \\frac{\\text{moles NaOH}}{\\text{volume (L)}}
]<\/p>\n\n\n\nAverage Molarity:<\/h4>\n\n\n\n
\\text{Average Molarity} = \\frac{\\text{Sum of Molarities}}{\\text{Number of Trials}}
]<\/p>\n\n\n\n
\n\n\n\n8. Acetic Acid in Vinegar<\/strong><\/h3>\n\n\n\n
Moles of NaOH:<\/h4>\n\n\n\n
\\text{moles} = \\text{Molarity} \\times \\text{volume (L)}
]<\/p>\n\n\n\nMoles of Acetic Acid:<\/h4>\n\n\n\n
Molarity of Acetic Acid (Diluted):<\/h4>\n\n\n\n
\\text{Molarity} = \\frac{\\text{moles}}{\\text{volume (L)}}
]<\/p>\n\n\n\nMolarity of Acetic Acid (Original):<\/h4>\n\n\n\n