Step 1: calculate mass of HNO3 in diluted solution
mass % = mass of HNO3 * 100 / mass of solution
11.7 = mass of HNO3 * 100 / 406.5
mass of HNO3 = 47.56 g
Step 2: calculate mass of concentrated solution
mass % = mass of HNO3 * 100 / mass of solution
69.0 = 47.56 * 100 / mass of solution
mass of solution = 68.93 g
Answer: 68.93 g
What mass in g) of a concentrated solution of nitric acid (69.0% HNO, by mass) is...
What mass (ing) of a concentrated solution of nitric acid (68.8% HNO, by mass) is needed to prepare 394.5 g of a 13.7% solution of HNO, by mass? X 9 Supporting Materials Periodic Table Constants and Factors Supplemental Data Additional Materials eBook . -/1.5 points OSGenChemWA1 3.4.WA.001. My Notes The formula for the mass percent of a component in a solution is shown mass percent component 1000 solution In this formula, m i s the mass of the component and...
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?
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TReferencer A solution is prepared by adding 49.9 ml concentrated hydrochloric acid and 19.7 ml concentrated nitric acid to 300 ml water More water is added until the final volume is 1.00 L. Calculate H".COH)and the pH for this solution. (Hint: Concentrated HCl is 38% HCI (by mass) and has a density of 1.19 g ml., concentrated HNO, is 70% HNO, (by mass) and has a density of 1.42 g/mL.] OH")= M pH-
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?
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
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...
Apps Settings Need Help? Read Supporting Materials Periodic Table Constants & Factors Supplemental Data 2. 0/8.33 points Previous Answers ZumChemP8 3.E.054. D My Notes The compound triamcinolone acetonide contains 66.34% C, 7.19% H, 4.37% F, and 22.09% o by mass. What is the empirical formula of triamcinolone acetonide? chemPad Help Greek - Your answer contains an improper or incomplete chemical formula. Need Help? Supporting Materials Periodic Table Constants & Factors Supplemental Data Submit Answer Practice Another Version My Notes