The concentrated sulfuric acid we use in the laboratory is 98.0 percent
H2SO4 by mass. Calculate the molality and molarity of the
acid solution. The density of the solution is 1.83 g/mL.
Consider 1 L = 1000 mL of solution
Mass of solution = volume x density
= 1000 x 1.83 = 1830 g
Mass of H2SO4 = 98.0/100 x 1830 = 1793.4 g
Moles of H2SO4 = mass/molar mass of H2SO4
= 1793.4/98.08 = 18.3 mol
Molarity = moles of H2SO4/volume of solution in L
= 18.3/1 = 18.3 M
Mass of water = 1830 - 1793.4 = 36.6 g = 0.0366 kg
Molality = moles of H2SO4/mass of water in kg
= 18.3/0.0366
= 500 mol/kg = 500m
The concentrated sulfuric acid we use in the laboratory is 98.0 percent
there's two questions :) Calculate the percent by mass of the solute in the following aqueous solution. 2.50 g of NaBr in 88.2 g of solution Be sure to answer all parts. An old sample of concentrated sulfuric acid to be used in the laboratory is approximately 98.4 percent H2SO4 by mass. Calculate the molality and molarity of the acid solution. The density of the solution is 1.83 g/mL.
Cadliy U.2JI2Cl 207nu will ILS THUlalily! 4. Concentrated sulfuric acid has a density of 1.83 g/mL. If the concentrated acid is 97% H2SO4, what is its molarity and normality? TE ! noneontatado adil.dadah dimillad... n
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