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How many milliliters of 0.150 M H2SOA (sulfuric acid) are required to react with 8.20 g or sodium hydrogen carbonate, NaHCO3, according to the following unbalanced equation? H,SO4 2 NAHCO3 Na,SO,+ 2 H,0 2 H20 + 2 CO2 ->

How many milliliters of 0.150 M H2SOA (sulfuric acid) are required to react with 8.20 g or sodium hydrogen carbonate, NaHCO3, according to the following unbalanced equation? H,SO4 2 NAHCO3 Na,SO,+ 2 H,0 2 H20 + 2 CO2 ->

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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**Problem 3** **Question:** How many milliliters of 0.150 M H₂SO₄ (sulfuric acid) are required to react with 8.20 g of sodium hydrogen carbonate, NaHCO₃, according to the following unbalanced equation? \[ \text{H}_2\text{SO}_4 + 2 \text{NaHCO}_3 \rightarrow \text{Na}_2\text{SO}_4 + 2 \text{H}_2\text{O} + 2 \text{CO}_2 \] **Additional Information/Notes:** - The concentration of the acid solution is provided as 0.150 M (Molarity). - The mass of sodium hydrogen carbonate is 8.20 g. No graphs or diagrams are present in the image. To solve the problem, follow these steps: 1. Calculate the moles of NaHCO₃ using its molar mass. 2. Determine the moles of H₂SO₄ needed using stoichiometry from the balanced equation. 3. Use the molarity of H₂SO₄ to find the volume required in milliliters.
Transcribed Image Text:**Problem 3** **Question:** How many milliliters of 0.150 M H₂SO₄ (sulfuric acid) are required to react with 8.20 g of sodium hydrogen carbonate, NaHCO₃, according to the following unbalanced equation? \[ \text{H}_2\text{SO}_4 + 2 \text{NaHCO}_3 \rightarrow \text{Na}_2\text{SO}_4 + 2 \text{H}_2\text{O} + 2 \text{CO}_2 \] **Additional Information/Notes:** - The concentration of the acid solution is provided as 0.150 M (Molarity). - The mass of sodium hydrogen carbonate is 8.20 g. No graphs or diagrams are present in the image. To solve the problem, follow these steps: 1. Calculate the moles of NaHCO₃ using its molar mass. 2. Determine the moles of H₂SO₄ needed using stoichiometry from the balanced equation. 3. Use the molarity of H₂SO₄ to find the volume required in milliliters.
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