Concentrated sulfuric acid is 18.4 molar and has a density of 1.84 grams per milliliter. After dilution with water to 5.20 molar the solution has a density of 1.38 grams per milliliter. This concentration of H2SO4 is often used in lead storage batteries(like a car battery).
1.Calculate the volume of concentrated H2SO4 needed to make 1.00L of 5.20 molar solution.
2.Calculate the % concentration H2SO4 in the concentrated solution.
1. mL x M = mL x M
2. 18.4 M = 18.4 moles/L soln
18.4 moles = 18.4*98 g/mol = 1803 grams H2SO4 in 1 L solution. The mass of 1 L solution is 1.84 g/mL x 1000 mL = 1840 grams.
%H2SO4 = (mass H2SO4/total mass soln)*100 = ??
1. To calculate the volume of concentrated H2SO4 needed to make 1.00L of a 5.20 molar solution, we can use the formula:
Volume (L) = Molarity (mol/L) / Concentration (mol/L)
Given that the final volume is 1.00L and the final concentration is 5.20 molar, we can plug in these values into the formula:
Volume (L) = 5.20 mol/L / 18.4 mol/L
Simplifying, we get:
Volume (L) = 0.283 L
Therefore, approximately 0.283 liters (or 283 milliliters) of concentrated H2SO4 is needed.
2. To calculate the percentage concentration of H2SO4 in the concentrated solution, we can use the formula:
% Concentration = (Actual Concentration / Maximum Concentration) * 100
Given that the actual concentration of the concentrated H2SO4 solution is 18.4 molar, and assuming that 100% sulfuric acid has a molarity of 18.4 mol/L, we can plug in these values into the formula:
% Concentration = (18.4 mol/L / 18.4 mol/L) * 100
Simplifying, we get:
% Concentration = 100%
Therefore, the concentrated solution has a 100% concentration of H2SO4.
To calculate the volume of concentrated H2SO4 needed to make 1.00L of a 5.20 molar solution, you can use the formula:
M1V1 = M2V2
Where M1 is the initial molarity of the concentrated H2SO4, V1 is the volume of the concentrated H2SO4 needed, M2 is the final molarity of the diluted solution, and V2 is the final volume of the diluted solution.
1. In this case, M1 = 18.4 M, V1 is what we want to find, M2 = 5.20 M, and V2 = 1.00 L. Plugging these values into the formula:
(18.4 M)(V1) = (5.20 M)(1.00 L)
V1 = (5.20 M)(1.00 L) / 18.4 M
V1 ≈ 0.283 L (rounded to 3 decimal places)
Therefore, you would need approximately 0.283 liters (or 283 milliliters) of concentrated H2SO4 to make 1.00 liter of a 5.20 molar solution.
2. To calculate the % concentration of H2SO4 in the concentrated solution, you can use the formula:
% concentration = (mass of solute / mass of solution) x 100
In this case, the solute is H2SO4, and the solution is the concentrated sulfuric acid. We are given the density of the concentrated sulfuric acid, which allows us to calculate the mass of the solution.
The density of the concentrated sulfuric acid is given as 1.84 g/mL. This means that for every milliliter of solution, we have 1.84 grams.
To calculate the mass of the solution, we can use the volume of the concentrated H2SO4 needed (V1) that we calculated earlier:
Mass of solution = volume x density = 0.283 L x 1.84 g/mL
Mass of solution ≈ 0.521 g (rounded to 3 decimal places)
The mass of the solute (H2SO4) can be calculated using the molarity and the molar mass of H2SO4, which is 98.09 g/mol.
Mass of solute = molarity x volume x molar mass = 18.4 M x 0.283 L x 98.09 g/mol
Mass of solute ≈ 482.16 g (rounded to 3 decimal places)
Now, we can substitute these values into the formula for % concentration:
% concentration = (mass of solute / mass of solution) x 100
% concentration = (482.16 g / 0.521 g) x 100
% concentration ≈ 92.61% (rounded to 2 decimal places)
Therefore, the concentrated solution has a % concentration of approximately 92.61% H2SO4.