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.