The concetrated sulfric aside we use laboratory is 98 percent,by mass. Calculate molarity and molality of acid solution.desity 1.83 g/ ml.

For molarity in steps.

mass of 1,000 mL = 1.83 g/mL x 1000 mL = 1830 g
mass of H2SO4 in that 1830 g = 1830 x 0.98 = about 1793 g.
mols H2SO4 = g/molar mass = 1793/98 = about 18.3 so
18.3 mols/L = 18.3 M.
For molality. m = moles/kg solvent.
moles = 18.3. You have total mass of 1830 and that minus 1793 g H2SO4 = 37 g solvent. Then mols/kg solvent = 18.3/0.037 = ?

Did you know?

Did you know that molarity and molality are two different measures used to express the concentration of a solution? In the case of a concentrated sulfuric acid solution used in laboratories, which has a mass percentage of 98%, we can calculate both the molarity and molality. To calculate the molarity, we need to know the molecular weight of sulfuric acid and convert the given mass percentage into grams. By dividing the grams of sulfuric acid by the molecular weight, and then dividing by the volume of the solution in liters, we can determine the molarity. On the other hand, to calculate the molality, we use the given density of the solution, along with its mass percentage, to determine the grams of sulfuric acid in 1 kilogram (1000 grams) of the solution. Dividing this value by the molecular weight gives us the number of moles of sulfuric acid, which can then be divided by the mass of the solvent (in kilograms) to find the molality. These two measures allow scientists to precisely express the concentration of a solution and play a vital role in various laboratory experiments.