{"id":33040,"date":"2025-06-23T05:37:34","date_gmt":"2025-06-23T05:37:34","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=33040"},"modified":"2025-06-23T05:37:36","modified_gmt":"2025-06-23T05:37:36","slug":"nahco3-hcl-h2o-nacl-co2-data-59-07-g-mass-of-empty-beaker","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/nahco3-hcl-h2o-nacl-co2-data-59-07-g-mass-of-empty-beaker\/","title":{"rendered":"NaHCO3 + HCl -> H2O + NaCl + CO2 Data: 59.07 g = Mass of Empty Beaker"},"content":{"rendered":"\n

NaHCO3 + HCl -> H2O + NaCl + CO2 Data: 59.07 g = Mass of Empty Beaker ; Mass of Beaker with NaHCO3 = 59.78 g ; Mass of Beaker the Following Day = 59.57 g Questions: 1. Use stoichiometry to calculate the theoretical mass of sodium chloride that should be obtained from the initial mass of sodium hydrogen carbonate used. 2. Calculate the mass of sodium chloride obtained in this experiment. 3. Determine the yield of the experiment. 4. Determine the percent error of the experiment. 5. Determine the theoretical amount of water and carbon dioxide that should be formed from the initial amount of sodium hydrogen carbonate. 6. Calculate the maximum amount of hydrochloric acid that should be used in order not to have an excess. 7. If the density of water is 1 g\/mL and 78.0 mL of water was obtained in this experiment, how many grams of sodium hydrogen carbonate reacted?<\/p>\n\n\n\n

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

Given Reaction:<\/strong><\/h3>\n\n\n\n

NaHCO\u2083 + HCl \u2192 H\u2082O + NaCl + CO\u2082<\/strong><\/p>\n\n\n\n

\n\n\n\n

Provided Data:<\/strong><\/h3>\n\n\n\n
    \n
  • Mass of Empty Beaker = 59.07 g<\/strong><\/li>\n\n\n\n
  • Mass of Beaker with NaHCO\u2083 = 59.78 g<\/strong><\/li>\n\n\n\n
  • Mass of Beaker after Reaction (Following Day) = 59.57 g<\/strong><\/li>\n<\/ul>\n\n\n\n
    \n\n\n\n

    1. Theoretical Mass of Sodium Chloride (NaCl) from Sodium Hydrogen Carbonate (NaHCO\u2083)<\/strong><\/h2>\n\n\n\n

    Molar Masses:<\/strong><\/p>\n\n\n\n

      \n
    • NaHCO\u2083 = 84.01 g\/mol<\/li>\n\n\n\n
    • NaCl = 58.44 g\/mol<\/li>\n<\/ul>\n\n\n\n

      Mass of NaHCO\u2083 Used:<\/strong>
      59.78 g – 59.07 g = 0.71 g<\/strong><\/p>\n\n\n\n

      Moles of NaHCO\u2083:<\/strong>
      0.71 g \u00f7 84.01 g\/mol \u2248 0.00845 mol<\/strong><\/p>\n\n\n\n

      From the balanced equation, molar ratio is 1:1<\/strong>, so moles of NaCl = 0.00845 mol<\/p>\n\n\n\n

      Theoretical Mass of NaCl:<\/strong>
      0.00845 mol \u00d7 58.44 g\/mol \u2248 0.494 g<\/strong><\/p>\n\n\n\n

      \n\n\n\n

      2. Mass of Sodium Chloride Obtained in the Experiment<\/strong><\/h2>\n\n\n\n

      Mass after Reaction = 59.57 g
      Mass of Empty Beaker = 59.07 g<\/p>\n\n\n\n

      Mass of NaCl Obtained:<\/strong>
      59.57 g – 59.07 g = 0.50 g<\/strong><\/p>\n\n\n\n

      \n\n\n\n

      3. Yield of the Experiment<\/strong><\/h2>\n\n\n\n

      Actual Mass of NaCl = 0.50 g<\/strong>
      Theoretical Mass of NaCl = 0.494 g<\/strong><\/p>\n\n\n\n

      Percent Yield:<\/strong>
      (0.50 g \u00f7 0.494 g) \u00d7 100 \u2248 101.2%<\/strong><\/p>\n\n\n\n

      Yield over 100% likely indicates measurement error or impurities<\/em><\/p>\n\n\n\n

      \n\n\n\n

      4. Percent Error of the Experiment<\/strong><\/h2>\n\n\n\n

      Percent Error:<\/strong>
      |Measured Value – Theoretical Value| \u00f7 Theoretical Value \u00d7 100<\/p>\n\n\n\n

      |0.50 g – 0.494 g| \u00f7 0.494 g \u00d7 100 \u2248 1.21%<\/strong><\/p>\n\n\n\n

      \n\n\n\n

      5. Theoretical Amount of Water and Carbon Dioxide Formed<\/strong><\/h2>\n\n\n\n

      From Reaction Stoichiometry:<\/strong> 1 mol NaHCO\u2083 produces:<\/p>\n\n\n\n

        \n
      • 1 mol H\u2082O (18.02 g\/mol)<\/li>\n\n\n\n
      • 1 mol CO\u2082 (44.01 g\/mol)<\/li>\n<\/ul>\n\n\n\n

        Moles of NaHCO\u2083 Used:<\/strong> 0.00845 mol<\/p>\n\n\n\n

        Mass of H\u2082O Produced:<\/strong>
        0.00845 mol \u00d7 18.02 g\/mol \u2248 0.152 g<\/strong><\/p>\n\n\n\n

        Mass of CO\u2082 Produced:<\/strong>
        0.00845 mol \u00d7 44.01 g\/mol \u2248 0.372 g<\/strong><\/p>\n\n\n\n

        \n\n\n\n

        6. Maximum Amount of Hydrochloric Acid Required<\/strong><\/h2>\n\n\n\n

        Molar Mass of HCl = 36.46 g\/mol<\/strong>
        Reaction ratio is 1:1<\/strong><\/p>\n\n\n\n

        Moles of HCl Required = 0.00845 mol<\/strong><\/p>\n\n\n\n

        Mass of HCl Required:<\/strong>
        0.00845 mol \u00d7 36.46 g\/mol \u2248 0.308 g<\/strong><\/p>\n\n\n\n

        \n\n\n\n

        7. Sodium Hydrogen Carbonate Reacted from Water Collected<\/strong><\/h2>\n\n\n\n

        Density of Water = 1 g\/mL<\/strong>
        Volume of Water = 78.0 mL<\/strong><\/p>\n\n\n\n

        Mass of Water = 78.0 g<\/strong><\/p>\n\n\n\n

        From Reaction:<\/strong> 1 mol NaHCO\u2083 produces 1 mol H\u2082O<\/p>\n\n\n\n

        Moles of H\u2082O:<\/strong>
        78.0 g \u00f7 18.02 g\/mol \u2248 4.33 mol<\/strong><\/p>\n\n\n\n

        Moles of NaHCO\u2083 Required:<\/strong> 4.33 mol<\/p>\n\n\n\n

        Mass of NaHCO\u2083 Required:<\/strong>
        4.33 mol \u00d7 84.01 g\/mol \u2248 363.83 g<\/strong><\/p>\n\n\n\n

        Thus, approximately 363.83 g<\/strong> of sodium hydrogen carbonate reacted to produce 78.0 mL of water.<\/p>\n\n\n\n

        \n\n\n\n

        Explanation (Summary)<\/strong><\/h2>\n\n\n\n

        The experiment involved reacting sodium hydrogen carbonate with hydrochloric acid to form sodium chloride, water, and carbon dioxide. Using precise mass measurements and stoichiometry, we calculated the expected yields for each product. The observed mass of sodium chloride closely matched the theoretical value, suggesting the reaction proceeded efficiently, though minor errors or impurities may have contributed to a slightly higher observed mass. Additionally, from water production data, we inferred the quantity of sodium hydrogen carbonate involved, showcasing the power of stoichiometric relationships in practical laboratory scenarios.<\/p>\n\n\n\n

        \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

        NaHCO3 + HCl -> H2O + NaCl + CO2 Data: 59.07 g = Mass of Empty Beaker ; Mass of Beaker with NaHCO3 = 59.78 g ; Mass of Beaker the Following Day = 59.57 g Questions: 1. Use stoichiometry to calculate the theoretical mass of sodium chloride that should be obtained from the initial […]<\/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-33040","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/33040","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=33040"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/33040\/revisions"}],"predecessor-version":[{"id":33042,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/33040\/revisions\/33042"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=33040"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=33040"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=33040"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}