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) given its density and concentration, we can follow a systematic approach. Molarity is defined as the number of moles of solute per liter of solution. Here’s how we can break it down step by step.

Step 1: Understanding the Given Information

We have the following data:

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

Step 2: Convert Density to g/L

Since molarity is expressed in moles per liter, we first convert the density from grams per milliliter to grams per liter:

1.84 g/mL = 1.84 g/mL × 1000 mL/L = 1840 g/L

Step 3: Calculate the Mass of H₂SO₄ in the Solution

Next, we need to find out how much of that mass is actually H₂SO₄. Since the solution is 98.00% H₂SO₄ by mass, we can calculate the mass of H₂SO₄ in one liter of solution:

Mass of H₂SO₄ = 1840 g/L × 0.9800 = 1807.2 g/L

Step 4: Calculate the Number of Moles of H₂SO₄

Now, we need to convert the mass of H₂SO₄ to moles. The molar mass of H₂SO₄ is approximately 98.09 g/mol. We can use this to find the number of moles:

Number of moles = Mass (g) / Molar mass (g/mol) = 1807.2 g / 98.09 g/mol ≈ 18.41 moles

Step 5: Calculate the Molarity

Finally, we can find the molarity by dividing the number of moles of H₂SO₄ by the volume of the solution in liters:

Molarity (M) = Moles of solute / Volume of solution (L) = 18.41 moles / 1 L = 18.41 M

Final Result

The molarity of the sulfuric acid solution is approximately 18.41 M. This high molarity indicates that sulfuric acid is a very concentrated solution, which is important to keep in mind when handling it in a laboratory setting.