Explain how you would prepare 100.0 mL of 0.500 M NaCl solution. Include the appropriate glassware and calculations.
You want how many mols? That's M x L = 0.500M x 0.100 L = 0.05 mols NaCl.
g NaCl = mols x molar mass = 0.05 x 58.5 = about 3 grams NaCl.
Place 3 g (you do it more accurately) in 100 mL volumetric flask, add some water, swirl to dissolve, make to the mark on the flask, stopper and mix.
To prepare 100.0 mL of a 0.500 M NaCl solution, you will need the following glassware and reagents:
Glassware:
- A 100.0 mL volumetric flask
- A measuring cylinder or pipette for accurate measurement
Reagents:
- Sodium chloride (NaCl)
- Distilled water
Here are the step-by-step instructions along with the calculations:
Step 1: Determine the amount of NaCl needed.
To calculate the amount of NaCl required, we use the formula:
(Desired concentration * Desired volume) = (Concentration of NaCl * Volume of NaCl)
Let's substitute the known values into the formula:
(0.500 M * 100.0 mL) = (x M * 100.0 mL)
Solving for x, the concentration of NaCl:
0.500 M * 100.0 mL = x M * 100.0 mL
50.0 mmol = x M * 100.0 mL
Divide both sides by 100.0 mL to isolate x:
50.0 mmol / 100.0 mL = x M
x = 0.500 M
Therefore, to prepare a 0.500 M NaCl solution of 100.0 mL, you will need 50.0 mmol of NaCl.
Step 2: Weigh out the appropriate amount of NaCl.
Using a balance, weigh out 5.85 grams (which corresponds to 50.0 mmol) of NaCl.
Step 3: Transfer the weighed NaCl to the volumetric flask.
Carefully place the weighed NaCl sample into the volumetric flask. Make sure no NaCl is left behind.
Step 4: Add distilled water to the volumetric flask.
Fill the volumetric flask up to the 100.0 mL mark using distilled water. The water should cover the NaCl completely.
Step 5: Dissolve the NaCl by gently swirling the flask.
Swirl the flask gently to dissolve the NaCl completely. Ensure that all the NaCl particles dissolve in the water.
Step 6: Rinse the glassware and transfer the NaCl solution.
Rinse the glassware with a small portion of the NaCl solution. Then, transfer the solution from the volumetric flask to a suitable storage container or perform any required analysis.
You have now successfully prepared 100.0 mL of a 0.500 M NaCl solution.
To prepare a 100.0 mL of 0.500 M NaCl solution, you will need the following glassware and materials:
1. A 100.0 mL volumetric flask or a suitable container to hold the final solution.
2. An analytical balance to measure the precise amount of NaCl.
3. Distilled water to dilute the NaCl.
Now, let's calculate the amount of NaCl needed to prepare the solution:
1. Molarity (M) is defined as the number of moles of solute per liter of solution. In this case, we want a 0.500 M NaCl solution, which means we need 0.500 moles of NaCl per liter of solution.
2. Calculating the amount of NaCl in moles:
- 0.500 M * 0.100 L (100.0 mL converted to liters) = 0.0500 moles.
3. The molar mass of NaCl is 58.44 g/mol. Multiplying the moles of NaCl with the molar mass gives us the mass of NaCl needed:
- 0.0500 moles * 58.44 g/mol = 2.92 grams.
Lastly, to prepare the solution:
1. Use the balance to accurately measure 2.92 grams of NaCl.
2. Place the weighed NaCl into the volumetric flask using a funnel or other suitable means.
3. Add distilled water slowly and make sure the NaCl is fully dissolved.
4. Continue adding distilled water until the solution reaches the mark on the volumetric flask (the 100.0 mL mark) while swirling it gently to ensure complete mixing.
5. Once the solution is fully prepared, cap the flask, invert it several times to ensure thorough mixing, and label it with the concentration, date, and any other necessary information.
By following these steps and calculations, you will have prepared a 100.0 mL of 0.500 M NaCl solution.