**Title: Analysis of Antacid Reaction with HCl****Introduction**In this experiment, a student prepares a mixture by dissolving 0.326 g of a powdered antacid in 32.36 mL of 0.1034 M HCl. The mixture is then boiled to remove carbon dioxide and, after cooling, bromophenol blue indicator is added, turning the solution yellow. **Procedure and Calculations**1. **Calculate the Total Number of Moles of HCl Added** - The mixture contains 32.36 mL of 0.1034 M HCl. Use the formula: \[ \text{Moles of HCl} = \text{Volume (L)} \times \text{Molarity (mol/L)} \] - Convert the volume from mL to L: 32.36 mL = 0.03236 L. - Moles of HCl = 0.03236 L × 0.1034 mol/L.2. **Source of CO₂** - The CO₂ likely originates from the antacid reacting with the acid, often involving carbonate or bicarbonate compounds.3. **Total Moles of OH⁻ Added** - 11.72 mL of 0.1506 M NaOH is used to change the indicator color from yellow to blue. - Convert volume to L: 11.72 mL = 0.01172 L. - Moles of OH⁻ = 0.01172 L × 0.1506 mol/L.4. **Calculate the Difference in Moles** - Find the difference between the moles of HCl and moles of NaOH added.5. **Moles of HCl Reacted and Equivalents of Antacid** - Determine how many moles of HCl reacted with the antacid and calculate the equivalents of antacid present.6. **Equivalents of Antacid per Gram** - Calculate the number of equivalents of antacid per gram using the relation of moles of HCl reacted.7. **Cost per Equivalent of Antacid** - Given the antacid costs $5.99 per 100 tablets and the average mass per tablet is 650 mg, calculate the cost per equivalent: - Determine the total mass of tablets and divide by the total equivalents to get cost per equivalent.

Show all calculations clearly. A student dissolves 0.326 g of a powdered antacid in 32.36 mL of 0.1034 M HCI. The student boils the mixture and then allows it to cool. Finally, the student adds bromophenol blue indicator to the mixture, which turns yellow. 1. Calculate the total number of moles of HCI added to the antacid. 2. Boiling the mixture helps get rid of dissolved CO2. What is the source of most of this CO2? 3. Suppose that 11.72 mL of 0.1506 M NaOH is required to turn the solution from yellow to blue. Calculate the total moles of OH added.

Show all calculations clearly. A student dissolves 0.326 g of a powdered antacid in 32.36 mL of 0.1034 M HCI. The student boils the mixture and then allows it to cool. Finally, the student adds bromophenol blue indicator to the mixture, which turns yellow. 1. Calculate the total number of moles of HCI added to the antacid. 2. Boiling the mixture helps get rid of dissolved CO2. What is the source of most of this CO2? 3. Suppose that 11.72 mL of 0.1506 M NaOH is required to turn the solution from yellow to blue. Calculate the total moles of OH added.

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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