68% of Nitric acid by mass in aqueous solution means that 68g [[68 × 100]/100] of Nitric acid present in 100g of solution. Therefore the molarity of the sample is 16.24 M.
63.01 grams of HNO3 is equal to 1 mole. 1 gram of HNO3 will be equal to 1/63.01 moles. Therefore, we can say that 1 liter of Nitric acid contains 15.6976 moles or in other words molarity of 70% (w/w) Nitric acid is equal to 15.6976 M.
What is the density of 65% Nitric acid?
Physicochemical Information
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68% means 68g oh HNO3 is present in 100g of solution. Volume of solution = Mass / Density. = 100 / 1.504 = 66.49ml.May 30, 2011
What is concentration of nitric acid?
Ordinary nitric acid is about 68% with a density of 1.4. At this concentration it forms a constant boiling mixture (boiling point 120°C). Concentrated nitric acid is about 98% and has a density 1.51.
How do you calculate concentration concentration?
Divide the mass of the solute by the total volume of the solution. Write out the equation C = m/V, where m is the mass of the solute and V is the total volume of the solution. Plug in the values you found for the mass and volume, and divide them to find the concentration of your solution.