A chemist needs 33.5 g of concentrated sulfuric acid for an experiment. The density of concentrated sulfuric acid is 1.84 g/mL. What volume of the acid is required? I know this is a conversion problem I'm just confused on where the numbers go.
If the concd H2SO4 is 100%, then
1.84 g/mL x ?mL = 33.5g
Solve for ?mL.
tatti kar lo
To solve this conversion problem, you need to use the given density of the concentrated sulfuric acid to calculate the volume of acid needed.
Density is defined as the mass of a substance (in this case, concentrated sulfuric acid) per unit volume. The formula for density is:
Density = Mass / Volume.
In this case, the given density of the concentrated sulfuric acid is 1.84 g/mL, which means for every 1 mL of the acid, it has a mass of 1.84 grams.
You are given that the chemist needs 33.5 grams of the acid. To find the volume of acid needed, you can rearrange the density formula to solve for volume:
Volume = Mass / Density.
Now let's substitute the given values into the equation:
Volume = 33.5 g / 1.84 g/mL.
Dividing the mass (33.5 g) by the density (1.84 g/mL), the units cancel out, leaving you with the volume in milliliters (mL):
Volume = 18.15 mL.
So, the chemist needs 18.15 mL of the concentrated sulfuric acid for the experiment.