## Pre-Lab Exercises### 1. Preparation of a 0.0500M NaOH Solution**Objective:** Describe how you would prepare 500.0 mL of a 0.0500M solution of sodium hydroxide (NaOH) from pure NaOH crystals. Include necessary calculations and describe the preparation procedure.**Procedure:**- **Calculate the Mass of NaOH Required:** 1. Use the formula: \[ \text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}} \] 2. Rearrange to find moles: \[ \text{moles of NaOH} = \text{Molarity} \times \text{Volume (L)} \] 3. Moles of NaOH required = 0.0500 mol/L × 0.500 L = 0.0250 mol 4. Calculate the mass of NaOH in grams using its molar mass (approximately 40.00 g/mol): \[ \text{mass of NaOH} = \text{moles} \times \text{molar mass} \] \[ \text{mass of NaOH} = 0.0250 \text{ mol} \times 40.00 \text{ g/mol} = 1.000 \text{ g} \]- **Prepare the Solution:** 1. Weigh 1.000 g of pure NaOH crystals accurately using a balance. 2. Dissolve the NaOH crystals in a small volume of distilled water in a beaker. 3. Transfer the solution to a 500.0 mL volumetric flask. 4. Add distilled water to the flask until the bottom of the meniscus is at the 500.0 mL mark. 5. Cap the flask and invert it several times to ensure thorough mixing.**Conclusion:** By following the above steps, a 0.0500M NaOH solution is successfully prepared using proper laboratory techniques.

The given data contains, Volume of NaOH = 500 mlMolarity of NaOH =0.0500 M

Answered: II Pre-Lab Exercises 1. Describe how y…

II Pre-Lab Exercises 1. Describe how y ou would make 500.0 ml. of a 0.0500M solution of NaOH from pure NaOH crystals. Show the calculations needed, and describe how you would make the solution.

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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