To determine which solution is the most concentrated, we compare the concentrations given in molarity (M), which is a measure of the number of moles of solute per liter of solution.
Let's list the concentrations provided for each solution:
1. [tex]\(2.0 \text{ mL}\)[/tex] of [tex]\(10 \text{ M} \, \text{H}_2\text{SO}_4\)[/tex]
2. [tex]\(5.0 \text{ mL}\)[/tex] of [tex]\(1.0 \text{ M} \, \text{PbSO}_4\)[/tex]
3. [tex]\(2.0 \text{ mL}\)[/tex] of [tex]\(10.5 \text{ M} \, \text{H}_2\text{O}_2\)[/tex]
4. [tex]\(100 \text{ mL}\)[/tex] of [tex]\(10 \text{ M} \, \text{NaCl}\)[/tex]
Since the molarities of the solutions are already provided, we will directly compare these values:
1. [tex]\( \text{H}_2\text{SO}_4 \)[/tex] has a concentration of [tex]\(10 \text{ M}\)[/tex].
2. [tex]\( \text{PbSO}_4 \)[/tex] has a concentration of [tex]\(1.0 \text{ M}\)[/tex].
3. [tex]\( \text{H}_2\text{O}_2 \)[/tex] has a concentration of [tex]\(10.5 \text{ M}\)[/tex].
4. [tex]\( \text{NaCl} \)[/tex] has a concentration of [tex]\(10 \text{ M}\)[/tex].
The most concentrated solution is the one with the highest molarity. Comparing the given concentrations, we have:
- [tex]\(10 \text{ M}\)[/tex] for [tex]\( \text{H}_2\text{SO}_4 \)[/tex]
- [tex]\(1.0 \text{ M}\)[/tex] for [tex]\( \text{PbSO}_4 \)[/tex]
- [tex]\(10.5 \text{ M}\)[/tex] for [tex]\( \text{H}_2\text{O}_2 \)[/tex]
- [tex]\(10 \text{ M}\)[/tex] for [tex]\( \text{NaCl} \)[/tex]
The highest molarity among these values is [tex]\(10.5 \text{ M}\)[/tex]. Therefore, the most concentrated solution is:
[tex]\(2.0 \text{ mL}\)[/tex] of [tex]\(10.5 \text{ M} \, \text{H}_2\text{O}_2\)[/tex].
