A sample of commercial concentrated sulfuric acid contains 98 percent H2SO4 by mass and has a density of 1.84 g/mL. then, a) What is the molarity and normality of H2SO4?

To find the molarity of H2SO4, we first need to calculate the molar mass of H2SO4:

H2SO4 = 2(1.01) + 32.06 + 4(16.00) = 98.08 g/mol

Next, we need to calculate the moles of H2SO4 in 1 L of the solution:

1 L of solution = 1000 mL
Mass of H2SO4 in 1 L of solution = 1.84 g/mL * 1000 mL = 1840 g
Mass of H2SO4 in 1 L of solution = 0.98 * 1840 g = 1803.2 g

Moles of H2SO4 = 1803.2 g / 98.08 g/mol = 18.39 mol

Therefore, the molarity of H2SO4 is:

Molarity = moles of solute / volume of solution in L
Molarity = 18.39 mol / 1 L = 18.39 M

To find the normality of H2SO4, we need to consider that H2SO4 is a diprotic acid, so each mole of H2SO4 can donate 2 moles of H+ ions. Therefore, the normality of H2SO4 is twice its molarity:

Normality = 2 * Molarity
Normality = 2 * 18.39 M = 36.78 N

Therefore, the molarity of H2SO4 is 18.39 M and the normality of H2SO4 is 36.78 N.

SOLUTION:

Given:

- Mass percent of H2SO4 = 98%
- Density of solution = 1.84 g/mL

Steps:

1. Calculate the mass of H2SO4 in 1 L of solution:

```
Mass of H2SO4 = (98 g / 100 g) x 1000 mL x (1 g / mL) = 980 g
```

2. Calculate the moles of H2SO4:

```
Moles of H2SO4 = 980 g / 98.08 g/mol = 10 mol
```

3. Calculate the volume of the solution containing 10 moles of H2SO4:

```
Volume = 10 mol / (1.84 g/mL) = 5.43 mL
```

4. Calculate the molarity (M):

```
Molarity = Moles of solute / Volume of solution in liters
= 10 mol / 0.00543 L
= 1841 M
```

5. Calculate the normality (N):

```
Normality = Molarity x Number of equivalents per mole
= 1841 M x 2 (for H2SO4)
= 3682 N
```

Therefore, the molarity of H2SO4 is 1841 M, and the normality is 3682 N.