Molarity of H2SO4 solution with given density


To determine the molarity of a H2SO4 solution with a given density, we need to take into account the density and the percentage weight of the solution. Let's break the problem down step by step:

Step 1: Determine the molar mass of H2SO4
The molar mass of H2SO4 can be calculated by adding up the atomic masses of its constituent elements:

H2SO4 = (2 * 1.00784 g/mol) + (32.06 g/mol) + (4 * 16.00 g/mol) = 98.09 g/mol

Step 2: Calculate the mass of H2SO4 in the solution
To determine the mass of H2SO4 in the solution, we need to consider the density and the percentage weight.

Given density = 1.84 g/cc
This means that for every 1 cc of solution, we have a mass of 1.84 g.

Step 3: Calculate the mass of H2SO4 in one cc of the solution
Since the solution is 98% weight, we can calculate the mass of H2SO4 in one cc of the solution as follows:

Mass of H2SO4 in one cc = 1.84 g * 0.98 = 1.8032 g

Step 4: Calculate the moles of H2SO4 in one cc of the solution
To calculate the moles of H2SO4, we divide the mass of H2SO4 in one cc by its molar mass:

Moles of H2SO4 in one cc = 1.8032 g / 98.09 g/mol = 0.01838 mol

Step 5: Calculate the molarity of the solution
Molarity is defined as moles of solute divided by the volume of the solution in liters. Since we have the moles of H2SO4 in one cc, we need to convert the volume to liters:

Volume of solution in liters = 1 cc / 1000 = 0.001 L

Molarity of H2SO4 solution = Moles of H2SO4 / Volume of solution in liters
Molarity of H2SO4 solution = 0.01838 mol / 0.001 L = 18.38 M

Conclusion:
The molarity of the H2SO4 solution with a density of 1.84 g/cc and 98% weight is 18.38 M.