You are asked to prepare 0.15 M HCl from a 36% W/v stock solution.Describe the procedure of the preparation.

0.15 M HCl = 0.15 x 36.5 molar mass = 5.475 g HCl/L solution.

We have 36% w/v which means 36 g HCl/100 mL solution. Therefore, each mL of this solution contains 0.36 g HCl. How many mL must we take to contain 5.475 g HCl? We must take 5.475 g x (1 mL/0.36 g) = 15.21 mL of the 36% soln. Therefore, 15.21 mL of 36% HCl soln made to a final volume of 1 L will be 0.15 M HCl. Check.
15.21 mL x 36 g HCl/100 mL = 5.475 g HCl.
5.475 g HCl x (1 mol HCl/36.5 g HCl) = 0.15 M.
You should redo the problem but use the exact molar mass HCl. I rounded.
Check my thinking.

Well, preparing 0.15 M HCl from a 36% W/v stock solution is like playing with acids, but don't worry, I won't turn this into a circus act! Here's what you need to do:

Step 1: Safety First!
Make sure you're wearing gloves, goggles, and a lab coat. We definitely don't want any accidental clown transformations!

Step 2: Calculate the Amounts
To prepare 0.15 M HCl, you'll need to know the volume of the stock solution. Let's say you need 100 ml of the new solution.

Step 3: Grab Your Beaker
Measure 100 ml of the 36% W/v HCl stock solution using a beaker. Keep your hands steady, no clown juggling tricks here!

Step 4: Mix It Up
Add the 100 ml of stock solution to a larger container, like a volumetric flask. Now, put on your serious face, and add some distilled water to the flask until you reach the 1-liter mark. Give it a gentle swirl to mix everything together.

Step 5: Voila!
Congratulations, you've created a 0.15 M HCl solution! Give yourself a round of applause. Just make sure not to squirt it at anyone, unless they're dressed as an orange or desperately need a chemical facial!

Remember, always handle acids with caution and follow proper lab protocols. Safety first, laughs second!

To prepare 0.15 M HCl from a 36% w/v stock solution, you will follow the steps below:

Step 1: Calculate the mass of the stock solution needed.
To find the mass of the stock solution needed, you will use the equation:

Mass of Stock Solution = (Volume of Final Solution * Desired Concentration) / % Concentration

In this case, the desired concentration is 0.15 M and the stock solution concentration is 36% w/v. Let's assume you need to prepare 100 mL of the final solution.

Mass of Stock Solution = (0.1 L * 0.15 mol/L) / 0.36

Step 2: Convert the mass of the stock solution to volume.
To convert the mass of the stock solution to volume, you will use its density. Let's assume the density of HCl is 1.18 g/mL.

Volume of Stock Solution = Mass of Stock Solution / Density

Step 3: Add the appropriate amount of stock solution to a container.
Measure the calculated volume of the stock solution using a graduated cylinder or pipette and add it to a clean container.

Step 4: Dilute the stock solution to the desired final volume.
To dilute the stock solution to the desired final volume, use distilled water. In this case, you will dilute to 100 mL.

Step 5: Mix thoroughly.
Gently swirl or stir the solution until it is well mixed.

Step 6: Verify the concentration.
You can use a pH meter or titration to verify that the concentration of the final solution is indeed 0.15 M.

The step-by-step procedure above outlines how to prepare a 0.15 M HCl solution from a 36% w/v stock solution.

To prepare a 0.15 M HCl (Hydrochloric acid) solution from a 36% W/V (weight/volume) stock solution, you will need the following materials and steps:

Materials needed:
1. 36% W/V HCl stock solution
2. Distilled water
3. Measuring cylinder or pipette
4. Stirring rod
5. Beaker or flask
6. Balance (if precise measurements are desired)

Procedure:

1. Determine the volume of the 0.15 M HCl solution you want to prepare. For instance, let's say you want to make 250 mL of the solution.

2. Calculate the amount of HCl required using the formula: Moles = Molarity x Volume (in liters).

In this case: Moles = 0.15 mol/L x 0.25 L = 0.0375 mol

3. Determine the mass of HCl required by multiplying the number of moles with the molar mass of HCl, which is approximately 36.46 g/mol.

Mass = 0.0375 mol x 36.46 g/mol = 1.3695 g

4. Weigh out the calculated mass of the 36% W/V HCl stock solution using a balance and transfer it to a beaker or flask.

5. Add distilled water to make up the desired final volume of the solution (250 mL, in this case). To do this, subtract the volume of the stock solution from the final volume required.

Water volume = Final volume - Stock solution volume
Water volume = 250 mL - Volume of stock solution

6. Calculate the volume of the stock solution to be added by dividing the mass of the stock solution by its density.

Volume of stock solution = Mass of stock solution / Density of stock solution

7. Using a measuring cylinder or pipette, measure the calculated volume of the stock solution determined in step 6 and add it to the beaker or flask containing the weighed stock solution.

8. Add the calculated volume of distilled water (determined in step 5) to the beaker or flask containing the stock solution.

9. Use a stirring rod to mix the contents thoroughly and ensure homogeneity.

10. Label the container with the concentration, date, and any other relevant information.

Congratulations! You have now prepared a 0.15 M HCl solution from a 36% W/V HCl stock solution. Note that safety precautions, such as working in a well-ventilated area and wearing appropriate PPE (personal protective equipment), should always be observed when handling chemicals.