Let's break down the solution step by step.
### Part 7.2.1: Calculate the number of moles of [tex]\( \text{H}_2\text{SO}_4 \)[/tex] present in this solution
1. Given data:
- Mass of [tex]\( \text{H}_2\text{SO}_4 \)[/tex] = 7.35 g
- Molar mass of [tex]\( \text{H}_2\text{SO}_4 \)[/tex] = 98.079 g/mol
2. Formula to calculate moles:
[tex]\[
\text{Moles} = \frac{\text{mass}}{\text{molar mass}}
\][/tex]
3. Calculation:
[tex]\[
\text{Moles of } \text{H}_2\text{SO}_4 = \frac{7.35 \text{ g}}{98.079 \text{ g/mol}} = 0.0749 \text{ moles}
\][/tex]
### Part 7.2.2: Calculate the mass of [tex]\( \text{NaOH} \)[/tex] added to the [tex]\( \text{H}_2\text{SO}_4 \)[/tex] solution
1. Balanced chemical equation:
[tex]\[
\text{H}_2\text{SO}_4 (aq) + 2 \text{NaOH} (s) \rightarrow \text{Na}_2\text{SO}_4 (aq) + 2 \text{H}_2\text{O} (l)
\][/tex]
2. Number of moles of [tex]\( \text{H}_2\text{SO}_4 \)[/tex]:
[tex]\[
\text{Moles of } \text{H}_2\text{SO}_4 = 0.0749 \text{ moles}
\][/tex]
3. Since the reaction requires 2 moles of [tex]\( \text{NaOH} \)[/tex] for every 1 mole of [tex]\( \text{H}_2\text{SO}_4 \)[/tex]:
[tex]\[
\text{Moles of } \text{NaOH} \text{ needed} = 2 \times \text{Moles of } \text{H}_2\text{SO}_4 = 2 \times 0.0749 = 0.1499 \text{ moles}
\][/tex]
4. Molar mass of [tex]\( \text{NaOH} \)[/tex]:
[tex]\[
\text{Molar mass of } \text{NaOH} = 39.997 \text{ g/mol}
\][/tex]
5. Formula to calculate mass:
[tex]\[
\text{Mass} = \text{moles} \times \text{molar mass}
\][/tex]
6. Calculation:
[tex]\[
\text{Mass of } \text{NaOH} = 0.1499 \text{ moles} \times 39.997 \text{ g/mol} = 5.995 \text{ grams}
\][/tex]
Therefore:
- The number of moles of [tex]\( \text{H}_2\text{SO}_4 \)[/tex] in the solution is [tex]\(0.0749\)[/tex] moles.
- The mass of [tex]\( \text{NaOH} \)[/tex] added to the [tex]\( \text{H}_2\text{SO}_4 \)[/tex] solution is [tex]\(5.995\)[/tex] grams.
