How many grams of H2SO4 are contained in 4.5 L of .30N (N standing for normality) sulfuric acid?

Help would be much appreciated.

To determine the number of grams of H2SO4 in 4.5 L of 0.30N sulfuric acid, we need to follow these steps:

Step 1: Understand the concept of normality (N)
Normality (N) is a measure of the concentration of a solution and is expressed in equivalents per liter (eq/L). It differs from molarity (M) as it takes into account the number of equivalents of the solute involved in the reaction.

Step 2: Calculate the molarity (M) of the solution
To find the molarity from the given normality, we need to determine the equivalent weight of sulfuric acid (H2SO4). Since sulfuric acid has two acidic hydrogen atoms, its equivalent weight will be half the molar mass (98.09 g/mol) of H2SO4.

Equivalent weight = Molar mass / Acidity (number of acidic hydrogen atoms)
Equivalent weight = 98.09 g/mol / 2 = 49.045 g/eq

Now, we can calculate the molarity (M) using the formula:

Normality (N) = Molarity (M) × Acidity (number of acidic hydrogen atoms)

0.30N = M × 2
M = 0.30N / 2 = 0.15 M

Step 3: Calculate the number of moles of H2SO4
Molarity (M) is defined as moles of solute per liter of solution. Since we have 4.5 L of the solution, we can calculate the number of moles of H2SO4 (n) using the formula:

Moles (n) = Molarity (M) × Volume (V in L)

Moles (n) = 0.15 mol/L × 4.5 L = 0.675 mol

Step 4: Calculate the mass of H2SO4
To find the mass of H2SO4, we need to multiply the number of moles (n) by the molar mass of H2SO4 (98.09 g/mol):

Mass = Moles × Molar mass
Mass = 0.675 mol × 98.09 g/mol = 66.25 g

Therefore, there are approximately 66.25 grams of H2SO4 in 4.5 L of 0.30N sulfuric acid.