To find the molar concentration (or molarity) of the solution, we need to convert the given molal concentration into molar concentration.
Molal concentration (m) is defined as the number of moles of solute per kilogram of solvent. In this case, the given molal concentration is 6.25 m, which means there are 6.25 moles of solute per kilogram of solvent (water in this case).
First, we need to convert the density of the solution (1.300 g/mL) to the mass of the solution.
Given:
Density of the solution = 1.300 g/mL
To convert the density to mass, we can use the formula:
mass = density x volume
Since the density is given in grams per milliliter (g/mL), we need to convert the volume of the solution to milliliters (mL).
Assuming the solution has a volume of 1 liter (1000 mL), the mass of the solution can be calculated as:
mass = 1.300 g/mL x 1000 mL = 1300 g
Next, we need to find the mass of the solvent (water) in the solution. We can assume that the density of water is 1 g/mL.
Using the formula:
mass = density x volume
The mass of the water can be calculated as:
mass = 1 g/mL x 1000 mL = 1000 g
Now, we have the mass of the solute (H2SO4) and the solvent (water), and we can calculate the molar concentration (molarity).
To convert molal concentration to molar concentration, we need to consider the molecular weight (molar mass) of the solute. The molecular weight of H2SO4 is 98.09 g/mol.
The equation for converting molal concentration to molar concentration is:
Molarity (M) = (molal concentration x molecular weight) / solvent mass
Molarity (M) = (6.25 m x 98.09 g/mol) / 1000 g
Calculating the result:
Molarity (M) = 0.613 M
Therefore, the molar concentration of the solution is 0.613 M.