Describe how you would prepare 2.00 L of an aqueous solution having a pH of 3.60 if you had a supply of 0.100 M HCL

To prepare a 2.00 L aqueous solution with a pH of 3.60 using a supply of 0.100 M HCl, follow these steps:

1. Determine the amount of HCl needed: Convert the desired pH into hydrogen ion concentration (H+) using the equation: [H+] = 10^(-pH). In this case, [H+] = 10^(-3.60) = 2.51 x 10^(-4) M.

2. Calculate the mole amount of HCl required: Since the concentration of the supplied HCl is 0.100 M, you need to find how much of this would give you the desired [H+] concentration. Use the formula: moles = volume x concentration. In this case, moles = 2.00 L x 2.51 x 10^(-4) M = 5.02 x 10^(-4) mol HCl.

3. Calculate the volume of the stock solution needed: To find the volume of the 0.100 M HCl needed to obtain the required moles, use the equation: volume = moles / concentration. In this case, volume = 5.02 x 10^(-4) mol / 0.100 M = 5.02 x 10^(-3) L or 5.02 mL.

4. Take the calculated volume of the 0.100 M HCl and dilute it to 2.00 L: Add the 5.02 mL of the 0.100 M HCl to a container and then add distilled water to reach a final volume of 2.00 L. Be sure to mix well to ensure homogeneity.

5. Verify the pH of the solution: You can use a pH meter or pH indicator paper to check the pH of the solution. If needed, adjust the pH by adding a few drops of either an acid or a base, such as hydrochloric acid or sodium hydroxide, respectively, while monitoring the pH until you achieve the desired pH of 3.60.

By following these steps, you can prepare a 2.00 L aqueous solution with a pH of 3.60 using the supplied 0.100 M HCl.