a 25% by mass H2SO4 solution has a density of 1.07 g/cm3 how much solution contains 13.37 g of H2SO4
To find out how much solution contains 13.37 g of H2SO4, we can use the information given about the concentration (25% by mass) and density (1.07 g/cm^3) of the solution.
1. Begin by determining the mass of the solution needed to achieve 13.37 g of H2SO4. Since the solution is 25% by mass H2SO4, we can use the following formula to calculate the mass of the solution:
Mass of H2SO4 / % concentration = Mass of Solution
13.37 g / 0.25 = 53.48 g
So, 53.48 g of the solution will contain 13.37 g of H2SO4.
2. Next, we can use the density of the solution to find the volume of 53.48 g of solution. The density is given as 1.07 g/cm^3, which means that 1 cm^3 of the solution weighs 1.07 g.
Volume = Mass / Density = 53.48 g / 1.07 g/cm^3 = 50 cm^3
Therefore, 53.48 g of the solution would have a volume of 50 cm^3.
To find out how much solution contains 13.37 g of H2SO4, we need to convert the mass percentage of the solution into the mass of H2SO4.
The mass percentage is given as 25% by mass, which means that 25 g of H2SO4 is present in every 100 g of the solution.
To determine the mass of H2SO4 in the solution, we can set up a ratio:
25 g H2SO4 / 100 g solution = 13.37 g H2SO4 / X g solution
Solving for X, we can cross-multiply and get:
25 g H2SO4 * X g solution = 13.37 g H2SO4 * 100 g solution
X g solution = (13.37 g H2SO4 * 100 g solution) / 25 g H2SO4
Performing the calculations:
X g solution = (1337 g * 100 g) / 25 g
X g solution = 5332 g
Therefore, 5332 g of the solution contains 13.37 g of H2SO4.
mL x density x (%/100) = 13.37
Solve for mL of the solution.