To determine which of the given solutions has the highest concentration of [tex]\( \text{H}^+ \)[/tex] ions, let's analyze each option. HCl is a strong acid, meaning it dissociates completely in water, so the concentration of [tex]\( \text{H}^+ \)[/tex] ions is equal to the concentration of the HCl solution itself.
Here are the given options:
- A. [tex]\( 0.001 \, M \, \text{HCl} \)[/tex]
- B. [tex]\( 10 \, M \, \text{HCl} \)[/tex]
- C. [tex]\( 0.1 \, M \, \text{HCl} \)[/tex]
- D. [tex]\( 0.01 \, M \, \text{HCl} \)[/tex]
Let's list the concentrations of [tex]\( \text{H}^+ \)[/tex] ions for each option:
- For option A: The concentration of [tex]\( \text{H}^+ \)[/tex] ions is [tex]\( 0.001 \, M \)[/tex].
- For option B: The concentration of [tex]\( \text{H}^+ \)[/tex] ions is [tex]\( 10 \, M \)[/tex].
- For option C: The concentration of [tex]\( \text{H}^+ \)[/tex] ions is [tex]\( 0.1 \, M \)[/tex].
- For option D: The concentration of [tex]\( \text{H}^+ \)[/tex] ions is [tex]\( 0.01 \, M \)[/tex].
Comparing all these concentrations, we see that [tex]\( 10 \, M \)[/tex] is the highest concentration among the given options.
Therefore, the solution with the highest concentration of [tex]\( \text{H}^+ \)[/tex] ions is:
B. [tex]\( 10 \, M \, \text{HCl} \)[/tex].
