How would you prepare 100 mL of a 0.01N sulfuric acid solution?

Technically you can't do this without knowing the reaction; however, you probably meant to use both H as in

2NaOH + H2SO4 ==> Na2SO4 + 2H2O

So how many equivalents do you want? That's N x L = 0.01N x 0.1L = 0.001 equivalents.
Then g = eq x eq wt = 0.001 x 49 = ?

You can work this in 1 step if you put both of these formulas together to obtain mL x N x meqwt=- grams
100 x 0.01 x 0.049 = ?

To prepare a 0.01N sulfuric acid solution, you will need to follow these steps:

Step 1: Determine the molecular weight of sulfuric acid
To calculate the normality (N) of a solution, you need to know the molecular weight of the compound. The molecular weight of sulfuric acid (H₂SO₄) is 98.09 g/mol.

Step 2: Calculate the amount of sulfuric acid needed
The normality (N) of a solution is defined as the number of gram equivalents of solute per liter of solution. In this case, a 0.01N solution means that there are 0.01 gram equivalents of sulfuric acid per liter of solution.

To calculate the weight of sulfuric acid needed to prepare a 0.01N solution, you can use the formula:

Weight of sulfuric acid (g) = (N x V x MW) / 1000

Where:
N = Normality of the solution
V = Volume of the solution (in liters)
MW = Molecular weight of sulfuric acid

In this case, you want to prepare 100 mL (0.1 L) of a 0.01N sulfuric acid solution. Plugging in the values, the calculation would be:

Weight of sulfuric acid (g) = (0.01 x 0.1 x 98.09) / 1000
Weight of sulfuric acid (g) = 0.09809 g

Therefore, you will need approximately 0.09809 grams of sulfuric acid to prepare a 0.01N solution.

Step 3: Dissolve the sulfuric acid in water
To prepare the 0.01N sulfuric acid solution, you need to dissolve the calculated amount of sulfuric acid (0.09809 grams) in enough water to make a total volume of 100 mL.

Make sure to use proper laboratory techniques while handling sulfuric acid, such as wearing gloves, protective eyewear, and working in a well-ventilated area.

Note: It is always recommended to double-check your calculations and use accurate measuring techniques to ensure the desired concentration of the solution.