17. The density of nitric acid (which is HNO3 in water) is 1.42 g/mL. The m/m% of HNO, in nitric acid is 69% m/m. H...
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
Introductory chemistry 20 A nitric acid solution containing 71.0% HNO3 (by mass) has a density of 1.42 g/mL. ow many moles of HNO, are present in 2.36 L of this solution? b) Determine the molarity of the acid.
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?
71. A solution of nitric acid has a density of 1.5 g/mL and is 20% by weight HNO3. a. What is the molarity of this solution of HNO;? b. What volume of this solution should be taken in order to prepare of 5.0 L of a solution of 0.15 M nitric acid by dilution with water? In order to obtain a precise concentration, the 0.15 M HNO solution is standardized against pure Hgo (molar mass = 216.59 g/mol) by titrating...
21. Commercial grade fuming nitric acid contains about 90% HNO3 by mass with a density of 1. 50 g/mL, calculate the molarity of the HNO, solution. A. 0.214 M B. 21.4M c. 2.14 M
17. A titration of 20.00 mL of 0.075 M HNO3 (nitric acid) with 0.0250 M NaOH is performed. The pH at 30.00 mL of NaOH added is (a) 1.02 (b) 1.82 (c) 7.00 (d) 3.55 (e) 10.5
17. A titration of 20.00 mL of 0.075 M HNO3 (nitric acid) with 0.0250 M NaOH is performed. The pH at 30.00 mL of NaOH added is (a) 1.02 (b) 1.82 (c) 7.00 (d) 3.55 (e) 10.5 18. A titration of 20.00 mL of 0.075 M HNO2 (nitrous acid) with 0.0250 M NaOH is performed. Given that K, for nitrous acid is 4.5 x 104, the pH at 30.00 mL of NaOH added is (a) 1.94 (b) 7.00 (c) 3.35...
B. Commercial nitric acid comes in a concentration of 16.0 mol/L. The density of this solution is 1.42 g/mL Calculate the percent (w/w) of nitric acid, HNO3, in this solution. How many milliliters of the concentrated acid have to be taken to prepared 250 g of a solution that is 10.0%(w/w) HNO3? C. Citric acid, H3C6H5O7, occurs in plants. Lemons contain 5% to 8% citric acid by mass. The acid is added to beverages and candy. An aqueous solution...
A 250 mL flask contains a 8.0% (m/v) nitric acid solution. Which TWO of the following ratios are NOT equivalent to the concentration? Select one or more: 8g HNO/100 mL soln 20 g HNO3/250 mL soln 80 g HNO/1 L soln 40 g HNO,/0.50 L soln 8 g HNO/1 mL soln 80 mg HN0/1 mL soln 0.08 g HNO/1 mL soln 8 g HNO3/1 L soln
Question 6 Not yet answered Marked out of 2.00 Y Flag question Common commercial acids and bases are aqueous solutions with the following properties: nitric acid density 1.42 g/cm3 and 69% solute by mass. Calculate the mole fraction. Answer Question 6 Not yet answered Marked out of 2.00 Y Flag question Common commercial acids and bases are aqueous solutions with the following properties: nitric acid density 1.42 g/cm3 and 69% solute by mass. Calculate the mole fraction. Answer