You have a 10 M acidic solution. However, you need that solution to be 0.25 M. How many ml of 10 M should be diluted to obtain 300 ml of 0.25 M acid solution?
The dilution formula is
mL x M = mL x M
A solution of ethanol (C2H5OH) in water is prepared by dissolving 87.4 mL of ethanol (density = 0.79 g/cm3) in enough water to make 250.0 mL of solution. What is the molarity of the ethanol in this solution?
35.6
To calculate how many milliliters (ml) of a 10 M acidic solution you should dilute to obtain 300 ml of a 0.25 M acid solution, you can use the formula for dilution:
C1V1 = C2V2
Where:
C1 = initial concentration of the solution (in this case, 10 M)
V1 = volume of the initial solution to be diluted (this is what we need to find)
C2 = final concentration of the solution (in this case, 0.25 M)
V2 = final volume of the solution (in this case, 300 ml)
Rearranging the formula to solve for V1:
V1 = (C2V2) / C1
Substituting the values into the formula:
V1 = (0.25 M * 300 ml) / 10 M
V1 = (75 ml * 1)
V1 = 75 ml
Therefore, to obtain 300 ml of a 0.25 M acid solution, you would need to dilute 75 ml of the 10 M acidic solution with an appropriate diluent.