5-7: A 10.34 molal aqueous nitric acid solution was prepared. (Density of nitric acid = 1.51 g/mL, density of water = 1.0 g/mL, and the MW of nitric acid = 63 g/mol) 5. How many grams of HNO3 were used to prepare the solution? 6. What is the Molarity of the solution? 7. What is the concentration (%v/v) of the solution?
5-7: A 10.34 molal aqueous nitric acid solution was prepared. (Density of nitric acid = 1.51 g/mL, density of water = 1.0 g/mL, and the MW of nitric acid = 63 g/mol) 5. How many grams of HNO3 were used to prepare the solution? 6. What is the Molarity of the solution? 7. What is the concentration (%v/v) of the solution?
Chapter1: Matter, Measurements, And Calculations
Section: Chapter Questions
Problem 1.126E
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5-7: A 10.34 molal aqueous nitric acid solution was prepared.
(Density of nitric acid = 1.51 g/mL, density of water = 1.0 g/mL, and the MW of nitric acid = 63 g/mol)
5. How many grams of HNO3 were used to prepare the solution?
6. What is the Molarity of the solution?
7. What is the concentration (%v/v) of the solution?
8-10: An aqueous solution of HNO3 was prepared having a molal concentration of 6.29.
(Atomic weights: H=1 amu, N=14 amu, O=16 amu, density of H2O = 1g/mL, density of HNO3 = 1.51 g/ml)
8. How many grams of HNO3 was used to prepare the said concentration?
9. What is the molarity of the aqueous HNO3 solution?
10. The % v/v of the prepared HNO3 solution is __________.
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