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Unformatted text preview: Solving 2.501000 933.9 2.677 = Molality is 2.68 m Problem 22: The concentrated sulfuric acid we use in the laboratory is 98.0 percent H 2 SO 4 mass. Calculate the molality and molarity of the acid solution. The density of the solution is 1.83 g/mL 1 L of this solution must weigh 1830g The mass of the sulfuric acid in the 1L must be 1793 g. .98 1830 1.793 10 3 = The mass of water in the one 1L of solution must be 37 g 1830 179337 = The molar mass of sulfuric acid is 98 g/mole 1793 98 18.296 = Since 18.3 moles of sulfuric acid are present in 1L, then the molarity is 18.3 M. Let x be the number of moles of sulfuric acid that would be present in 1000 g of water Solving for x 18.3 37 x 1000 18.31000 37 494.595 = The solution is 494 m...
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This note was uploaded on 04/07/2008 for the course CHEMISTRY 112 taught by Professor Donato during the Spring '08 term at CofC.
 Spring '08
 Donato
 Mole

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