A concentrated sulfuric acid solution is 65.0% H2SO4 by mass and has a density of 1.55 g/mL at 20°C. What is the mass of 3.00 L of the concentrated sulfuric acid solution?
1.55 g/mL x 3000 mL = ?
The mass of the H2SO$ in that 3.0L is
1.55 g/mL x 3000 mL x 0.65 = ?
3.02
To find the mass of the concentrated sulfuric acid solution, we first need to calculate the volume of the solution.
Given:
Density of the sulfuric acid solution = 1.55 g/mL
Volume of the solution = 3.00 L
To convert liters to milliliters, we need to multiply the given volume by 1000:
3.00 L x 1000 mL/L = 3000 mL
Since the density of the sulfuric acid solution is given in grams per milliliter, we can directly multiply the volume (in milliliters) by the density (in grams per milliliter) to get the mass:
Mass = Volume x Density
Mass = 3000 mL x 1.55 g/mL
Now, we can calculate the mass:
Mass = 4650 grams
Therefore, the mass of 3.00 L of the concentrated sulfuric acid solution is 4650 grams.
To find the mass of the concentrated sulfuric acid solution, we can follow these steps:
Step 1: Convert 3.00 L to milliliters (mL).
Since we know that 1 L is equal to 1000 mL, we can calculate:
3.00 L x 1000 mL/L = 3000 mL
Step 2: Use the density of the solution to calculate the mass of 3000 mL.
Density is defined as mass divided by volume. In this case, the density is 1.55 g/mL. So we can calculate:
Mass = Density x Volume
Mass = 1.55 g/mL x 3000 mL = 4650 g
Therefore, the mass of 3.00 L of the concentrated sulfuric acid solution is 4650 grams.