3. Concentrated nitric acid is 70.4% HNO, by mass and has a density of 1.42 g/mL. What is the molarity of concentrated nitric acid? a. 11.2 M b. 55.5 M c. 7.87 M d. 14.6 M e. 15.9 M
The percentage by weight of nitric acid, HNO3, in a sample of concentrated nitric acid is to be determined. Initially a NaOH solution was standardized by titration with a sample of potassium hydrogen phthalate, KHC8H4O4, a monoprotic acid often used as a primary standard. A sample of pure KHC8H4O4 weighing 1.518 grams was dissolved in water and titrated with the NaOH solution. To reach the equivalence point, 26.90 millilitres of base was required. Calculate the molarity of the NaOH solution....
Find the molarity of nitric acid in a reagent labeled “70.0 wt% HNO3, density = 1.413 g/mL.
dont understand how to calculate.
Concentrated nitric acid - look up Prepare a 2% nitric acid solution with a !liter From concentrated nitric acid solution Calibration curve 10 parts per million standard solution 1 part per billion 10 part per billion 5 part per billion 20 part per billion 100 part per billion
Concentrated nitric acid - look up Prepare a 2% nitric acid solution with a !liter From concentrated nitric acid solution Calibration curve 10 parts per million standard...
What are the mole fractions of HNO3 in a concentrated solution of nitric acid (59.3 % HNO3 by mass)? Please outline the steps to answer this question
A solution is made by adding 42.0 mL of concentrated hydrochloric acid (37.3 wt%, density 1.19 g/mL) to some water in a volumetric flask, and then adding water to the mark to make exactly 250 mL of solution. Calculate the concentration of this solution in molarity
What mass in g) of a concentrated solution of nitric acid (69.0% HNO, by mass) is needed to prepare 406.5 g of a 11.7% solution of HNO, by mass? x 9 Supporting Materials Periodic Table Supplemental Data Constants and Factors Submit Answer
Nitric acid is usually purchased in a concentrated form that is 70.3% HNO3 by mass and has a density of 1.41 g/mL. How much concentrated solution would you take to prepare 1.30 L of 0.105 M HNO3by mixing with water?
Nitric acid is usually purchased in a concentrated form that is 70.3% HNO3 by mass and has a density of 1.41 g/mL. How much concentrated solution would you take to prepare 1.05 L of 0.120 M HNO3 by mixing with water?
A sample of concentrated nitric acid has a density of 1.41 g/mL and contains 70.0%HNO; by mass. What mass of HNO3 is present per liter of solution?