Answer :
To prepare 10 liters of a 2.00 M nitric acid solution from a 71% concentrated nitric acid solution with a density of 1.42 g/mL, approximately 1265.82 mL of the concentrated acid is needed.
The calculating the volume of concentrated nitric acid needed to prepare a specific molarity of a itric acid solution. The given concentration of HNO3 by mass is 71%, and the density is 1.42 g/mL. To find the required volume to prepare a 2.00 M solution, we must first calculate the molarity of the concentrated nitric acid.
The formula to use is: Molarity = [(ext{concentration})(ext{density}) / ext{Molecular weight}] imes 10. From this information, we can calculate the molarity of the concentrated nitric acid:
M = [(71)(1.42) / (63.01)] ×10 = 15.8 M.
Now, using the dilution formula M1V1 = M2V2, where M1 is the molarity of the concentrated solution, V1 is the volume of the concentrated solution you need, M2 is the final molarityof the diluted solution, and V2 is the final volume of the diluted solution. We plug in the known values:
15.8M × V1 = 2.00M ×10,000mL.
Solving for V1 gives us:
V1 = (2.00 M ×10,000 mL) / 15.8 M = 1265.82 mL. So, approximately 1265.82 mL (or 1.26582 L) of the concentrated nitric acid is required to prepare 10 liters of a 2.00 M solution.
