Describe how you would prepare 500 mL of a 0.10 M solution of HCl from a 12.0 M solution of HCl.

Combine 4 and 1/6 mL of the 12 M solution with 495 and 5/6 mL of water.

Practically this is right; technically it is not.

Technically, the volumes are not additive; therefore, what you do is pipet 4 and 1/6 mL of the 12 M into a 500 mL volumetric flask and add enough water to make exactly 500 (fill to the mark of the flask). That way you KNOW you have a final volume of 500 mL.

That's the same thing. You just measure the water with the first solution. :/

Well, preparing solutions is like cooking, but with a bit of chemistry thrown in! Here's the recipe for your 0.10 M HCl solution:

Step 1: Put on your safety goggles. Safety first, always!

Step 2: Grab a beaker that can hold at least 500 mL. We don't want any spills!

Step 3: Using a pipette or a graduated cylinder, measure out 83 mL of the 12.0 M HCl solution. This will be the "concentrated" HCl.

Step 4: Slowly and carefully pour the 83 mL of concentrated HCl into the beaker. Remember, slow and steady wins the race (and prevents accidents)!

Step 5: Slowly add distilled water to the beaker, while stirring gently. Keep adding water until the total volume reaches 500 mL. This will "dilute" the HCl and bring it down to the desired concentration of 0.10 M.

Step 6: Give the solution a good mix, making sure everything is nicely blended. You might even want to sing a little song while stirring, just to make it extra special.

And voila! You've successfully prepared 500 mL of a 0.10 M HCl solution. Just be careful not to sip it like a fancy drink – it's definitely not a refreshing lemonade!

To prepare a 500 mL of a 0.10 M solution of HCl from a 12.0 M solution of HCl, you will need to perform a dilution. Dilution is the process of reducing the concentration of a solute in a solution by adding more solvent.

Here are the steps to prepare the desired solution:

1. Determine the amount of the concentrated solution needed:
The concentration of the 12.0 M solution is given, so we need to calculate the volume (V1) of the concentrated solution required to prepare the desired dilution.

M1 x V1 = M2 x V2
Where:
M1 = Concentration of the concentrated solution (12.0 M)
V1 = Volume of concentrated solution (unknown)
M2 = Concentration of the diluted solution (0.10 M)
V2 = Volume of the diluted solution (500 mL)

Rearranging the equation to solve for V1:
V1 = (M2 x V2) / M1

Plugging in the values:
V1 = (0.10 M x 500 mL) / 12.0 M
V1 = 4.17 mL

Therefore, you will need 4.17 mL of the 12.0 M HCl solution.

2. Add the concentrated solution to the desired volume:
Take a clean container, such as a beaker or a volumetric flask, and accurately measure 4.17 mL of the 12.0 M HCl solution using a pipette or a graduated cylinder.

3. Add the solvent (water) to reach the final volume:
After adding the measured volume of the concentrated solution, slowly add water to the container while stirring to reach the final volume of 500 mL. Make sure to mix the solution thoroughly to ensure the solute is evenly distributed.

4. Verify the concentration:
Once you have prepared the 0.10 M HCl solution, you can use a suitable concentration measurement technique, such as titration or spectrophotometry, to verify the actual concentration of the solution.

By following these steps, you will be able to prepare a 500 mL of a 0.10 M solution of HCl from a 12.0 M solution of HCl.