What is the concentration of a solution prepared by diluting 25.0 mL of HCL 0.750 mol/L to a final volume of 500.mL?
mol HCl = M x L = 0.750 M x 0.025 L = ??
Then Molarity = mols/L = ??/0.500
0.750 M x 0.025 L = 0.01 mol
0.01 mol/0.500L = 0.02...units?
a 0.40 M HCl solution prepared from 25 mL of a 6.0 M HCl solution
To find the concentration of a solution prepared by dilution, you can use the formula:
C1V1 = C2V2
where:
C1 = initial concentration
V1 = initial volume
C2 = final concentration
V2 = final volume
In this case, the initial concentration (C1) is 0.750 mol/L and the initial volume (V1) is 25.0 mL. The final volume (V2) is 500 mL. We want to find the final concentration (C2).
First, we need to convert the initial volume and the final volume to the same units. Let's convert both volumes to liters:
V1 = 25.0 mL = 25.0 mL * (1 L / 1000 mL) = 0.025 L
V2 = 500 mL = 500 mL * (1 L / 1000 mL) = 0.500 L
Now we can plug these values into the formula:
(0.750 mol/L)(0.025 L) = C2(0.500 L)
To find C2, we solve for it:
C2 = (0.750 mol/L)(0.025 L) / 0.500 L
C2 = 0.0375 mol
Therefore, the concentration of the solution prepared by diluting 25.0 mL of HCl 0.750 mol/L to a final volume of 500 mL is 0.0375 mol/L.