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In the table below, the experimental data collected by Students A, B and C are given on lines 1, 2 and 3. Calculate the missing values for these students, and enter these values on lines 4 to 8. Be sure to use the correct number of significant figures. In the spaces marked "Set-up", show your work to calculate the values for Student A only. Complete all the calculations and then average the results of the three trials. On the assigned date, submit to your instructor the report form (page 2) and the complete calculations for the exercises on page 3. |DATA|| Student A Student B Student C Line# 1 Weight of the evaporating dish 46.075 g 51.857 g 48.432 g 2 Volume of the salt solution 5.00 mL5.00 mL5.00 mL 3 Weight of the dish and residue after evaporation 4Weight of dry sodium chloride Set-up: Line #3 – Line #1 46.587 g 52.355 g 48.937 g 5Moles of sodium chloride Set-up: Line #4÷58.5 g/mol moles moles moles 6Volume of solution in liters Set-up: #2 1000 mL

In the table below, the experimental data collected by Students A, B and C are given on lines 1, 2 and 3. Calculate the missing values for these students, and enter these values on lines 4 to 8. Be sure to use the correct number of significant figures. In the spaces marked "Set-up", show your work to calculate the values for Student A only. Complete all the calculations and then average the results of the three trials. On the assigned date, submit to your instructor the report form (page 2) and the complete calculations for the exercises on page 3. |DATA|| Student A Student B Student C Line# 1 Weight of the evaporating dish 46.075 g 51.857 g 48.432 g 2 Volume of the salt solution 5.00 mL5.00 mL5.00 mL 3 Weight of the dish and residue after evaporation 4Weight of dry sodium chloride Set-up: Line #3 – Line #1 46.587 g 52.355 g 48.937 g 5Moles of sodium chloride Set-up: Line #4÷58.5 g/mol moles moles moles 6Volume of solution in liters Set-up: #2 1000 mL

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
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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**Concentration of a Solution: Educational Exercise** **Discussion:** This virtual experiment involves determining the concentration of salt (sodium chloride, NaCl) in an aqueous solution. Concentration may be expressed in various ways, and this experiment studies two systems: molarity (M) and weight/volume percent (%w/v). **Report Form** Name: ____________ Section: ____________ Date: ____________ In the table below, experimental data collected by Students A, B, and C are provided on lines 1, 2, and 3. Calculate the missing values for these students and enter these values on lines 4 to 8. Use the correct number of significant figures. In the spaces marked “Set-up,” show your work to calculate the values for Student A only. Complete all the calculations and then average the results of the three trials. On the assigned date, submit to your instructor the report form (page 2) and the complete calculations for the exercises on page 3. --- **DATA** | Line# | | Student A | Student B | Student C | |-------|--------------------------------|-----------|-----------|-----------| | 1 | Weight of the evaporating dish | 46.075 g | 51.857 g | 48.432 g | | 2 | Volume of the salt solution | 5.00 mL | 15.00 mL | 15.00 mL | | 3 | Weight of the dish and residue after evaporation | 46.587 g | 52.355 g | 48.937 g | | 4 | Weight of dry sodium chloride | Set-up: Line #3 – Line #1 | | | | 5 | Moles of sodium chloride | Set-up: Line #4 ÷ 58.5 g/mol | | | | 6 | Volume of solution in liters | Set-up: #2 ÷ 1000 mL | | | | 7 | Molarity (M) of the solution | Set-up: #5 ÷ #6 | | | | 8 | Percent (%w/w) of sodium chloride | Set-up: (#4 ÷ #2) × 100 | | | | 9 | Average (%w/w) of sodium chloride | Set-up: (8A
Transcribed Image Text:**Concentration of a Solution: Educational Exercise** **Discussion:** This virtual experiment involves determining the concentration of salt (sodium chloride, NaCl) in an aqueous solution. Concentration may be expressed in various ways, and this experiment studies two systems: molarity (M) and weight/volume percent (%w/v). **Report Form** Name: ____________ Section: ____________ Date: ____________ In the table below, experimental data collected by Students A, B, and C are provided on lines 1, 2, and 3. Calculate the missing values for these students and enter these values on lines 4 to 8. Use the correct number of significant figures. In the spaces marked “Set-up,” show your work to calculate the values for Student A only. Complete all the calculations and then average the results of the three trials. On the assigned date, submit to your instructor the report form (page 2) and the complete calculations for the exercises on page 3. --- **DATA** | Line# | | Student A | Student B | Student C | |-------|--------------------------------|-----------|-----------|-----------| | 1 | Weight of the evaporating dish | 46.075 g | 51.857 g | 48.432 g | | 2 | Volume of the salt solution | 5.00 mL | 15.00 mL | 15.00 mL | | 3 | Weight of the dish and residue after evaporation | 46.587 g | 52.355 g | 48.937 g | | 4 | Weight of dry sodium chloride | Set-up: Line #3 – Line #1 | | | | 5 | Moles of sodium chloride | Set-up: Line #4 ÷ 58.5 g/mol | | | | 6 | Volume of solution in liters | Set-up: #2 ÷ 1000 mL | | | | 7 | Molarity (M) of the solution | Set-up: #5 ÷ #6 | | | | 8 | Percent (%w/w) of sodium chloride | Set-up: (#4 ÷ #2) × 100 | | | | 9 | Average (%w/w) of sodium chloride | Set-up: (8A
**Problem:** 3. 5.0 mL of a potassium chloride solution is transferred to an evaporating dish and the water evaporated. The weight of KCl is 0.75 g. a. Calculate the molarity b. Calculate the percent (w/v) KCl --- **Solution:** **a. Calculate the molarity** To calculate the molarity (M), use the formula: \[ \text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}} \] 1. **Find the moles of KCl**: - The molar mass of KCl is approximately 74.55 g/mol. - Moles of KCl = \[ \frac{0.75 \text{ g}}{74.55 \text{ g/mol}} \] 2. **Convert volume to liters**: - Volume = 5.0 mL = 0.005 L 3. **Calculate the molarity**: - Molarity (M) = \[ \frac{\text{moles of KCl}}{0.005 \text{ L}} \] **b. Calculate the percent (w/v) KCl** Percent (w/v) is calculated using the formula: \[ \text{Percent (w/v)} = \left( \frac{\text{mass of solute (g)}}{\text{volume of solution (mL)}} \right) \times 100 \] 1. Substituting the given values: - Mass of KCl = 0.75 g - Volume of solution = 5.0 mL - Percent (w/v) = \[ \left( \frac{0.75 \text{ g}}{5.0 \text{ mL}} \right) \times 100 \] This setup lays a foundational understanding for solving problems involving the concentration of solutions and can be applied to various chemical calculations.
Transcribed Image Text:**Problem:** 3. 5.0 mL of a potassium chloride solution is transferred to an evaporating dish and the water evaporated. The weight of KCl is 0.75 g. a. Calculate the molarity b. Calculate the percent (w/v) KCl --- **Solution:** **a. Calculate the molarity** To calculate the molarity (M), use the formula: \[ \text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}} \] 1. **Find the moles of KCl**: - The molar mass of KCl is approximately 74.55 g/mol. - Moles of KCl = \[ \frac{0.75 \text{ g}}{74.55 \text{ g/mol}} \] 2. **Convert volume to liters**: - Volume = 5.0 mL = 0.005 L 3. **Calculate the molarity**: - Molarity (M) = \[ \frac{\text{moles of KCl}}{0.005 \text{ L}} \] **b. Calculate the percent (w/v) KCl** Percent (w/v) is calculated using the formula: \[ \text{Percent (w/v)} = \left( \frac{\text{mass of solute (g)}}{\text{volume of solution (mL)}} \right) \times 100 \] 1. Substituting the given values: - Mass of KCl = 0.75 g - Volume of solution = 5.0 mL - Percent (w/v) = \[ \left( \frac{0.75 \text{ g}}{5.0 \text{ mL}} \right) \times 100 \] This setup lays a foundational understanding for solving problems involving the concentration of solutions and can be applied to various chemical calculations.
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