To address the question correctly, let's evaluate each statement about the balance between hydronium ions ([tex]\(\left[ H_3O^+ \right]\)[/tex]) and hydroxide ions ([tex]\(\left[ OH^- \right]\)[/tex]) in different types of solutions.
1. In neutral solutions, [tex]\(\left[ H_3O^+ \right] = \left[ OH^- \right]\)[/tex]:
- This statement is true. A neutral solution has equal concentrations of hydronium and hydroxide ions. At 25°C, the concentration of each ion in pure water is [tex]\(1 \times 10^{-7} \)[/tex] M.
2. In bases, [tex]\(\left[ OH^- \right]\)[/tex] is less than [tex]\(\left[ H_3O^+ \right]\)[/tex]:
- This statement is false. In a basic solution, the concentration of hydroxide ions is greater than the concentration of hydronium ions, meaning [tex]\(\left[ OH^- \right] > \left[ H_3O^+ \right]\)[/tex].
3. In bases, [tex]\(\left[ OH^- \right] = \left[ H_3O^+ \right]\)[/tex]:
- This statement is also false. In basic solutions, the concentrations of [tex]\(\left[ OH^- \right]\)[/tex] and [tex]\(\left[ H_3O^+ \right]\)[/tex] are not equal; the hydroxide ion concentration is higher.
4. In bases, [tex]\(\left[ OH^- \right]\)[/tex] is greater than [tex]\(\left[ H_3O^+ \right]\)[/tex]:
- This statement is true. By definition, basic solutions have a higher concentration of hydroxide ions compared to hydronium ions.
5. In acids, [tex]\(\left[ OH^- \right] \)[/tex] is greater than [tex]\(\left[ H_3O^+ \right]\)[/tex]:
- This statement is false. In an acidic solution, the concentration of hydronium ions is greater than that of hydroxide ions, meaning [tex]\(\left[ H_3O^+ \right] > \(\left[ OH^- \right]\)[/tex].
Thus, the correct statements from the given list are:
1. In neutral solutions, [tex]\(\left[ H_3O^+ \right] = \left[ OH^- \right]\)[/tex].
4. In bases, [tex]\(\left[ OH^- \right]\)[/tex] is greater than [tex]\(\left[ H_3O^+ \right]\)[/tex].
So, the correctly identified statements are:
1 and 4.
