find the molarity of 0.087 f of H2SO4 in 3.4 L of water? what is the answer
I will be happy to critique your work.
See earlier post.
To find the molarity of a solution, we need to know the number of moles of the solute (H2SO4 in this case) and the volume of the solution (water) in liters.
First, we'll convert the given concentration of H2SO4 from "f" (formal) to molarity. The conversion factor between the two is:
1 f = 1 mol/L
Therefore, 0.087 f of H2SO4 is equivalent to 0.087 mol/L.
Next, we have the volume of the solution, which is 3.4 L of water.
Now, we can apply the formula for molarity:
Molarity (M) = Moles of solute (mol) / Volume of solution (L)
Plugging in the values, we get:
Molarity = 0.087 mol/L / 3.4 L
Calculating this gives us:
Molarity ≈ 0.026 M
Therefore, the molarity of 0.087 f of H2SO4 in 3.4 L of water is approximately 0.026 M.