A solution of sulfuric acid is 40.0% by mass and it has a density of 1.30g/mL, what is the molarity of the solution?
assume on liter...
mass=1300g, of which 1300*.4 is H2SO4
Molarity= 1300*.4/molmassH2SO4*1
0.4g H2SO4/1g solution X 1.30g solution/ 1mL solution X 1 mol H2SO4/98.09 g H2SO4 X 1000mL/1L=5.3 M
To find the molarity of a solution, we need to know the mass of the solute (sulfuric acid) and the volume of the solution.
First, we need to calculate the mass of sulfuric acid in the solution. We know that the solution is 40.0% sulfuric acid by mass, so if we have 100 grams of the solution, 40.0 grams of it will be sulfuric acid.
Next, we need to calculate the volume of the solution. We are given the density of the solution, which is 1.30 g/mL. This means that if we have 1 mL of the solution, it will weigh 1.30 grams.
Let's assume we have 100 mL of the solution. Using the density, we can calculate the mass of the solution:
Mass of solution = Volume of solution x Density
Mass of solution = 100 mL x 1.30 g/mL
Mass of solution = 130 grams
Now we know that out of the 130 grams of the solution, 40.0 grams is sulfuric acid. We can use this information to calculate the molarity.
Molarity = moles of solute / volume of solution (L)
To find the moles of solute, we need to use the molar mass of sulfuric acid, which is 98.09 g/mol.
moles of sulfuric acid = mass of sulfuric acid / molar mass of sulfuric acid
moles of sulfuric acid = 40.0 g / 98.09 g/mol
moles of sulfuric acid = 0.407 mol
Now we can calculate the molarity:
Molarity = 0.407 mol / 0.100 L
Molarity = 4.07 M
Therefore, the molarity of the sulfuric acid solution is 4.07 M.