concentrated sulfuric acid is typically 18.1 M H2 SO4. Calculate the volume in mL of concentrated sulfuric acid needed to prepare 125 mL of a 0.100 M H2SO 4 solution
mL1 x M1 = mL2 x M2
c1*v1= c2*v2 if c1=18.10m, v2=?, c2= 0.01m, v2=125ml. v2=0.01*125/18.1 v2=0.069ml
To calculate the volume of concentrated sulfuric acid needed to prepare a 0.100 M H2SO4 solution, we can use the formula:
M1 * V1 = M2 * V2
Where:
M1 = concentration of the concentrated sulfuric acid (18.1 M)
V1 = volume of the concentrated sulfuric acid needed (in mL)
M2 = desired concentration of the diluted solution (0.100 M)
V2 = desired volume of the diluted solution (125 mL)
Rearranging the formula, we can solve for V1:
V1 = (M2 * V2) / M1
Substituting the given values:
V1 = (0.100 M * 125 mL) / 18.1 M
Calculating this expression:
V1 = (0.100 mol/L * 0.125 L) / 18.1 mol/L
V1 = 0.0125 mol / 18.1 mol/L
V1 ≈ 0.000691 mol
Since 1 mole of sulfuric acid has a volume of 98 mL, we can convert this to mL:
V1 = 0.000691 mol * 98 mL/mol
V1 ≈ 0.0676 mL
Therefore, approximately 0.0676 mL of concentrated sulfuric acid is needed to prepare 125 mL of a 0.100 M H2SO4 solution.
To calculate the volume of concentrated sulfuric acid needed, you can use the formula:
M1V1 = M2V2
where:
M1 = initial concentration
V1 = initial volume
M2 = final concentration
V2 = final volume
Given:
M1 = 18.1 M
V1 = unknown
M2 = 0.100 M
V2 = 125 mL
Let's plug these values into the formula and solve for V1:
(18.1 M)(V1) = (0.100 M)(125 mL)
Divide both sides of the equation by 18.1 M to isolate V1:
V1 = (0.100 M)(125 mL) / 18.1 M
Calculating this expression gives:
V1 = (0.100)(125) / 18.1 mL
V1 ≈ 0.692 m
Therefore, you would need approximately 0.692 mL of concentrated sulfuric acid to prepare 125 mL of a 0.100 M H2SO4 solution.