Commercially available concentrated sulfuric acid is 18.0 M H2SO4. Calculate the volume (in mL) of concentrated sulfuric acid required to prepare 1.60 L of 0.320 M H2SO4 solution.
mL x M = mL x M
To calculate the volume of concentrated sulfuric acid required, we can use the formula:
M₁V₁ = M₂V₂
where:
M₁ = initial molarity (18.0 M)
V₁ = initial volume (unknown)
M₂ = final molarity (0.320 M)
V₂ = final volume (1.60 L)
Rearranging the formula to solve for V₁:
V₁ = (M₂ * V₂) / M₁
Now we can substitute the given values into the formula and solve for V₁:
V₁ = (0.320 M * 1.60 L) / 18.0 M
V₁ ≈ 0.0284 L
To convert this volume to milliliters, multiply by 1000:
V₁ ≈ 28.4 mL
Therefore, approximately 28.4 mL of concentrated sulfuric acid is required to prepare 1.60 L of 0.320 M H2SO4 solution.
To calculate the volume of concentrated sulfuric acid required to prepare the desired solution, we will use the formula:
M1V1 = M2V2
Where:
M1 is the initial molarity of the concentrated sulfuric acid solution,
V1 is the volume of the concentrated sulfuric acid solution we want to calculate,
M2 is the final molarity of the desired H2SO4 solution, and
V2 is the final volume of the desired H2SO4 solution.
Given:
M1 = 18.0 M (concentrated sulfuric acid solution)
V1 = unknown
M2 = 0.320 M (desired H2SO4 solution)
V2 = 1.60 L (desired volume of H2SO4 solution)
Rearranging the formula to solve for V1, we get:
V1 = (M2 * V2) / M1
Substituting the given values into the equation, we have:
V1 = (0.320 M * 1.60 L) / 18.0 M
Calculating the numerator:
(0.320 M * 1.60 L) = 0.512
Dividing by the denominator:
0.512 / 18.0 M = 0.02844 L
Since the volume is required in milliliters (mL), we convert liters (L) to milliliters by multiplying by 1000:
0.02844 L * 1000 mL/L = 28.44 mL
Therefore, the volume of concentrated sulfuric acid required to prepare 1.60 L of 0.320 M H2SO4 solution is 28.44 mL.