What volume of concentrated hydrochloric acid (12.0 M HCl) is required to make 2.0 liters of a 3.0 M HCl solution?
mL1 x M1 = mL2 x M2
mL1 x 12 = 2000 mL x 3.0 M
Solve for mL1
To determine the volume of concentrated hydrochloric acid required, we can use the formula:
M1 × V1 = M2 × V2
Where:
M1 = Concentration of the concentrated hydrochloric acid (12.0 M)
V1 = Volume of the concentrated hydrochloric acid (unknown)
M2 = Concentration of the final solution (3.0 M)
V2 = Volume of the final solution (2.0 L)
Rearranging the formula to solve for V1:
V1 = (M2 × V2) / M1
Plugging in the given values:
V1 = (3.0 M × 2.0 L) / 12.0 M
V1 = 0.5 L
Therefore, 0.5 liters of concentrated hydrochloric acid is required to make 2.0 liters of a 3.0 M HCl solution.
To find the volume of concentrated hydrochloric acid required, we can use the formula:
C1V1 = C2V2
Where:
C1 = initial concentration of the solution (12.0 M)
V1 = initial volume of the solution (unknown)
C2 = final concentration of the solution (3.0 M)
V2 = final volume of the solution (2.0 L)
We need to solve for V1. Rearranging the formula, we get:
V1 = (C2 * V2) / C1
Plugging in the values, we have:
V1 = (3.0 M * 2.0 L) / 12.0 M
= 0.5 L
Therefore, 0.5 liters of concentrated hydrochloric acid is required to make 2.0 liters of a 3.0 M HCl solution.