Calculation of Normality of H2SO4 Solution

Given:
Mass of H2SO4 = 0.98 g
Volume of solution = 500 mL = 0.5 L

Molar mass of H2SO4 = 2(1.008) + 32.06 + 4(16.00) = 98.08 g/mol
Number of moles of H2SO4 = mass/molar mass = 0.98/98.08 = 0.01 mol

Normality (N) = (number of equivalents of solute/volume of solution in L)

Since H2SO4 is a diprotic acid, it can donate two H+ ions per molecule, which means it has two equivalents per mole. Therefore, the number of equivalents of H2SO4 present in the solution is:

Number of equivalents of H2SO4 = 2 x number of moles of H2SO4 = 2 x 0.01 = 0.02 eq

Putting the values in the above formula, we get:

N = 0.02 eq/0.5 L = 0.04 N

Therefore, the correct answer is (b) 0.04N.

Explanation:

The normality of a solution is defined as the number of equivalents of a solute present in one liter of the solution. In this question, we are given the mass of H2SO4 and the volume of the solution. Using this information, we can calculate the number of moles of H2SO4 present in the solution. Since H2SO4 is a diprotic acid, it has two equivalents per mole. Therefore, we need to multiply the number of moles by 2 to get the number of equivalents of H2SO4 present in the solution. Finally, we can use the formula for normality to calculate the normality of the solution.