How much 12 M HCl do you add to 1 L of water to obtain 0.2 HCl? Use this same approach to do the math for the dilution of 5.5 M of barium hydroxide solution to 0.5 M barium hydroxide solution.
To determine the amount of 12 M HCl needed to obtain a 0.2 M HCl solution, we can use the formula:
C1V1 = C2V2
Where:
C1 is the initial concentration of the HCl solution (12 M)
V1 is the volume of the HCl solution needed
C2 is the desired concentration of the HCl solution (0.2 M)
V2 is the final volume of the diluted HCl solution (1 L)
Rearranging the formula, we have:
V1 = (C2V2) / C1
Substituting the given values:
V1 = (0.2 M * 1 L) / 12 M
V1 = 0.0167 L (or 16.7 mL)
Therefore, you would need to add 16.7 mL of the 12 M HCl solution to 1 L of water to obtain a 0.2 M HCl solution.
Using the same approach, we can calculate the amount of 5.5 M barium hydroxide solution needed to obtain a 0.5 M barium hydroxide solution.
Again, using the formula:
C1V1 = C2V2
Where:
C1 is the initial concentration of the barium hydroxide solution (5.5 M)
V1 is the volume of the barium hydroxide solution needed
C2 is the desired concentration of the barium hydroxide solution (0.5 M)
V2 is the final volume of the diluted barium hydroxide solution
Rearranging the formula, we have:
V1 = (C2V2) / C1
Substituting the given values:
V1 = (0.5 M * V2) / 5.5 M
Since the final volume (V2) is not provided, we cannot solve for the exact volume needed without that information. You would need to know the final volume to calculate the volume of the 5.5 M barium hydroxide solution required.
Please provide the final volume, and I will gladly assist you in calculating the required volume of the 5.5 M barium hydroxide solution.