15.00mL sample of a solution of H2SO4 of unknown concentration was titrated with 0.3200 N NaOH. The titration required 21.30mL of the base.

What was the normality of the acid solution?
what was the molarity of the acid solution?

To determine the normality of the acid solution, we need to use the equation:

Normality (N) = Molarity (M) × Number of equivalents (n)

Since H2SO4 is a diprotic acid (can donate two protons), the number of equivalents for H2SO4 is 2.

First, let's calculate the normality of the acid solution:

Normality (H2SO4) = Molarity (NaOH) × Number of equivalents (NaOH)

The molarity of NaOH is given as 0.3200 N (N stands for Normal).

Normality (H2SO4) = 0.3200 N × 2

Normality (H2SO4) = 0.6400 N

Next, let's calculate the molarity of the acid solution using the formula:

Molarity (M) = Normality (N) × Molecular weight (MW) / Volume (L)

The molecular weight of H2SO4 is:
2(Atomic weight of hydrogen) + Atomic weight of sulfur + 4(Atomic weight of oxygen)
= 2(1.01 g/mol) + 32.07 g/mol + 4(16.00 g/mol)
= 98.09 g/mol

Converting the given volume from mL to L:
15.00 mL = 15.00 mL / 1000 mL/L
= 0.01500 L

Now, let's calculate the molarity of the acid solution:

Molarity (H2SO4) = Normality (H2SO4) × Molecular weight (H2SO4) / Volume (H2SO4)

Molarity (H2SO4) = 0.6400 N × 98.09 g/mol / 0.01500 L

Molarity (H2SO4) ≈ 4.235 M

Therefore, the normality of the acid solution is 0.6400 N, and the molarity of the acid solution is approximately 4.235 M.

To find the normality of the acid solution, you need to use the formula:

Normality = (N1 x V1) / V2

Where:
N1 is the normality of the base solution (NaOH in this case),
V1 is the volume of the base solution used in the titration,
V2 is the volume of the acid solution used in the titration.

Given:
N1 = 0.3200 N (normality of NaOH solution)
V1 = 21.30 mL (volume of NaOH solution used)
V2 = 15.00 mL (volume of acid solution used)

Substituting the given values into the formula, we have:

Normality = (0.3200 N x 21.30 mL) / 15.00 mL

Calculating this, we get the normality of the acid solution.

To find the molarity of the acid solution, you need to convert the normality to molarity using the formula:

Molarity = Normality x Gram Equivalent Weight

The gram equivalent weight (GEW) of H2SO4 is the molar mass divided by the number of equivalents of acid per mole. In this case, H2SO4 has a molar mass of 98.09 g/mol and two equivalents of acid per mole.

GEW = 98.09 g/mol / 2 equivalents/mol

Substituting the value of GEW and the calculated normality into the formula, we have:

Molarity = Normality x GEW

Calculating this, we get the molarity of the acid solution.

By following these steps, you should be able to find both the normality and molarity of the acid solution.

H2SO4 + 2NaOH ==> Na2SO4 + 2H2O

mols NaOH = M x L = ? (Note: the M and N of NaOH are the same.)
Using the coefficients in the balanced equation, convert mols NaOH to mols H2SO4. That will be mols H2SO4 = 1/2 mols NaOH.
Then M H2SO4 = mols H2SO4/L H2SO4 = ?

To convert to N,
N = M*#H titrated. #H in this case is 2 so N = M*2