Calculate either [H₂O+] or [OH-] for each of the solutions at 25 °C.

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Chapter1: Chemical Foundations
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**Exercise: Calculating Ion Concentrations at 25°C**

Calculate either \([H_3O^+]\) or \([OH^-]\) for each of the solutions at 25°C.

**Solution A:**

- Given: \([OH^-] = 3.17 \times 10^{-7}\) M
- Required: \([H_3O^+]\)

\[ \text{Use } K_w = [H_3O^+][OH^-] = 1.0 \times 10^{-14} \text{ at 25°C} \]

**Solution B:**

- Given: \([H_3O^+] = 7.95 \times 10^{-9}\) M
- Required: \([OH^-]\)

\[ \text{Use } K_w = [H_3O^+][OH^-] = 1.0 \times 10^{-14} \text{ at 25°C} \]

**Solution C:**

- Given: \([H_3O^+] = 6.01 \times 10^{-4}\) M
- Required: \([OH^-]\)

\[ \text{Use } K_w = [H_3O^+][OH^-] = 1.0 \times 10^{-14} \text{ at 25°C} \]

**Question:**

Which of these solutions are basic at 25°C?

- Solution C: \([H_3O^+] = 6.01 \times 10^{-4}\) M
- Solution B: \([H_3O^+] = 7.95 \times 10^{-9}\) M
- Solution A: \([OH^-] = 3.17 \times 10^{-7}\) M
Transcribed Image Text:**Exercise: Calculating Ion Concentrations at 25°C** Calculate either \([H_3O^+]\) or \([OH^-]\) for each of the solutions at 25°C. **Solution A:** - Given: \([OH^-] = 3.17 \times 10^{-7}\) M - Required: \([H_3O^+]\) \[ \text{Use } K_w = [H_3O^+][OH^-] = 1.0 \times 10^{-14} \text{ at 25°C} \] **Solution B:** - Given: \([H_3O^+] = 7.95 \times 10^{-9}\) M - Required: \([OH^-]\) \[ \text{Use } K_w = [H_3O^+][OH^-] = 1.0 \times 10^{-14} \text{ at 25°C} \] **Solution C:** - Given: \([H_3O^+] = 6.01 \times 10^{-4}\) M - Required: \([OH^-]\) \[ \text{Use } K_w = [H_3O^+][OH^-] = 1.0 \times 10^{-14} \text{ at 25°C} \] **Question:** Which of these solutions are basic at 25°C? - Solution C: \([H_3O^+] = 6.01 \times 10^{-4}\) M - Solution B: \([H_3O^+] = 7.95 \times 10^{-9}\) M - Solution A: \([OH^-] = 3.17 \times 10^{-7}\) M
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