Calculate [H3O+] in each aqueous solution at 25 °C, and classify each solution as acidic or basic. a. [OH-] = 1.1 * 10^-9 M b. [OH-] = 2.9 * 10^-2 M c. [OH-] = 6.9 * 10^-12 M

Verified step by step guidance

1. Use the water dissociation constant at 25 °C, which is Kw = 1.0 \times 10^{-14} \text{ M}^2, to find [H_3O^+].
2. For each solution, apply the formula [H_3O^+] = \frac{Kw}{[OH^-]} to calculate the hydronium ion concentration.
3. Substitute the given [OH^-] values into the formula: a. [OH^-] = 1.1 \times 10^{-9} \text{ M}, b. [OH^-] = 2.9 \times 10^{-2} \text{ M}, c. [OH^-] = 6.9 \times 10^{-12} \text{ M}.
4. Determine the nature of each solution: If [H_3O^+] > 1.0 \times 10^{-7} \text{ M}, the solution is acidic; if [H_3O^+] < 1.0 \times 10^{-7} \text{ M}, the solution is basic.
5. Classify each solution based on the calculated [H_3O^+]: a. Compare [H_3O^+] to 1.0 \times 10^{-7} \text{ M}, b. Compare [H_3O^+] to 1.0 \times 10^{-7} \text{ M}, c. Compare [H_3O^+] to 1.0 \times 10^{-7} \text{ M}.