Answer :
To find the volume of 71% concentrated nitric acid needed to prepare 10 liters of a 2.00 M solution, calculate the molarity of the concentrated acid and then apply the dilution formula. It results in approximately 12.66 liters of concentrated acid, which is an overestimate due to the adjusted percentage in the example.
To calculate the volume of concentrated nitric acid (HNO3) needed to prepare a dilute solution, you must use the concept of molarity and the dilution formula M1V1 = M2V2, where M1 and M2 are the molarities of the concentrated and dilute solutions, respectively, and V1 and V2 are the corresponding volumes.
First, calculate the molarity of the concentrated nitric acid using its density and percentage by mass:
Molarity (M) = [(71%) (1.42 g/mL) / (63.01 g/mol)] imes 10
Therefore, M = 1.58 M (approximate, since the example uses 69.8%).
Then, use the dilution formula to find the volume of concentrated acid needed to prepare 10 liters of a 2.00 M solution:
1.58 M imes V1 = 2.00 M imes 10 L
V1 = (2.00 M imes 10 L) / 1.58 M
V1 = 12.66 L (approximate based on exact molarity).
