Help with #6 please ### Prelab Calculations1. **Determine the Mass of CaCl₂·2H₂O:** - Objective: Use a four-place analytical balance to weigh out the precise amount needed to prepare 100 mL of a 0.1005 M solution of Ca²⁺. - Molecular Weight: 147.02 g/mole2. **Determine the Mass of KCl:** - Objective: Use a four-place analytical balance to weigh out the amount needed to prepare 100 mL of a 1 M solution of KCl. - Molecular Weight: 74.5513 g/mole3. **Solubility Recording:** - Task: Record the solubility of calcium carbonate in water (expressed in mg/L) in your notebook.4. **Calculate the Calcium Carbonate Not in Solution:** - Task: Compute the amount of calcium carbonate (in mg) that remains undissolved if a tablet is dissolved in 250 mL of water. - Note: The tablet’s label claims it contains 600 mg of calcium per tablet.5. **Solubility Increase Inquiry:** - Analyze what substances could be added to a solution to increase the solubility of calcium carbonate (CaCO₃) in water.6. **Net Ionic Equation:** - Task: Write the net ionic equation for calcium carbonate in acidified water.### Additional Information- **Calcium Source:** The calcium in the tablet is calcium carbonate (CaCO₃).- **Quantitation Requirement:** Calcium, as the Ca²⁺ ion, must be in solution to accurately measure (mg calcium/tablet) using an Ion Selective Electrode (ISE).

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1. Determine the mass of CaCl2:2H2O (MW 147.02 g/mole) to weigh out using a four- place analytical balance to prepare 100 mL of a 0.1005 M solution of Ca2+. 2. Determine the mass of KCI to weigh out using a four-place analytical balance to prepare 100 mL of a 1 M solution of KCI (MW 74.5513 g/mole). 3. Record the solubility of calcium carbonate in water (mg/L) in your notebook. 4. Calculate the amount of calcium carbonate (mg) not in solution if a tablet is dissolved in 250 mL of water and the tablet's label claim is 600 mg calcium / tablet. The source of calcium in the tablet to be analyzed is calcium carbonate (CaCO3). Calcium, as the Ca+2 ion, must be solution to accurately quantitate the (mg calcium / tablet) using an ISE. 5. What could be added to a solution to increase the solubility of CaCO3 in water? 6. Write the net ionic equation for calcium carbonate in acidified water.

1. Determine the mass of CaCl2:2H2O (MW 147.02 g/mole) to weigh out using a four- place analytical balance to prepare 100 mL of a 0.1005 M solution of Ca2+. 2. Determine the mass of KCI to weigh out using a four-place analytical balance to prepare 100 mL of a 1 M solution of KCI (MW 74.5513 g/mole). 3. Record the solubility of calcium carbonate in water (mg/L) in your notebook. 4. Calculate the amount of calcium carbonate (mg) not in solution if a tablet is dissolved in 250 mL of water and the tablet's label claim is 600 mg calcium / tablet. The source of calcium in the tablet to be analyzed is calcium carbonate (CaCO3). Calcium, as the Ca+2 ion, must be solution to accurately quantitate the (mg calcium / tablet) using an ISE. 5. What could be added to a solution to increase the solubility of CaCO3 in water? 6. Write the net ionic equation for calcium carbonate in acidified water.

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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