Calculate the mority of H₂SO₄ of density of 1.84g/mol and of 98.00% of H2SO₄

To calculate the molarity of sulfuric acid (H₂SO₄) with a given density and concentration, we can follow a systematic approach. Molarity (M) is defined as the number of moles of solute per liter of solution. Here’s how we can break down the calculation step by step.

Step 1: Understand the Given Information

We have the following data:

• Density of H₂SO₄ solution: 1.84 g/mL
• Concentration of H₂SO₄: 98.00%

Step 2: Calculate the Mass of H₂SO₄ in 1 Liter of Solution

First, we need to find out how much H₂SO₄ is present in 1 liter (1000 mL) of the solution. Using the density, we can calculate the mass of the solution:

Mass of solution = Density × Volume

Mass of solution = 1.84 g/mL × 1000 mL = 1840 g

Next, we calculate the mass of H₂SO₄ in this solution using the concentration:

Mass of H₂SO₄ = Concentration × Mass of solution

Mass of H₂SO₄ = 0.98 × 1840 g = 1803.2 g

Step 3: Convert Mass of H₂SO₄ to Moles

To find the number of moles of H₂SO₄, we use its molar mass. The molar mass of H₂SO₄ is approximately 98.09 g/mol. Now we can calculate the moles:

Moles of H₂SO₄ = Mass of H₂SO₄ / Molar mass of H₂SO₄

Moles of H₂SO₄ = 1803.2 g / 98.09 g/mol ≈ 18.37 moles

Step 4: Calculate the Molarity

Now that we have the number of moles, we can find the molarity:

Molarity (M) = Moles of solute / Volume of solution in liters

Molarity = 18.37 moles / 1 L = 18.37 M

Final Result

The molarity of the sulfuric acid solution is approximately 18.37 M. This high molarity indicates that the solution is very concentrated, which is typical for concentrated sulfuric acid solutions.

In summary, by using the density and concentration of the solution, we calculated the mass of H₂SO₄ in a liter of solution, converted that mass to moles, and finally determined the molarity. This method can be applied to other solutions as well, making it a valuable skill in chemistry.