Final answer:
The molarity of the sulfuric acid solution is 0.459 M, and the normality is 0.918 N.
Step-by-step explanation:
Molarity is defined as the number of moles of solute per liter of solution. To calculate the molarity of the sulfuric acid solution, we need to determine the number of moles of sulfuric acid and the volume of the solution. The molarity (M) is given by the formula:
Molarity (M) = Moles of Solute / Volume of Solution (in liters)
The number of moles of sulfuric acid can be calculated using its molar mass, which is 98.09 g/mol. Given that the mass of the sulfuric acid is 45 g and the volume of the solution is 1 liter, we have:
Number of moles = Mass of Solute / Molar Mass = 45 g / 98.09 g/mol = 0.459 moles
Therefore, the molarity of the sulfuric acid solution is:
Molarity = Moles of Solute / Volume of Solution = 0.459 moles / 1 liter = 0.459 M
Normality is a measure of the number of equivalents of solute per liter of solution. Since sulfuric acid is a diprotic acid, each mole of sulfuric acid can donate two equivalents of protons. Therefore, the normality (N) of the sulfuric acid solution is twice the molarity:
Normality = Molarity × 2 = 0.459 M × 2 = 0.918 N