At 25 °C, what is the hydroxide ion concentration, [OH¯], in an aqueous solution with a hydrogen ion concentration of [H*]=3.3 × 10-4 M? [OH"] M

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**Question:**

At 25°C, what is the hydroxide ion concentration, [OH⁻], in an aqueous solution with a hydrogen ion concentration of [H⁺] = 3.3 × 10⁻⁴ M?

**Answer box:**
```
[OH⁻] = ___________________ M
```

**Explanation:**
This question requires understanding the relationship between hydrogen ion concentration and hydroxide ion concentration in an aqueous solution at 25°C. Typically, this is involving the use of the water dissociation constant, Kw, which is 1.0 × 10⁻¹⁴ at 25°C. 

For a solution at 25°C:
\[ [H⁺] \cdot [OH⁻] = 1.0 \times 10^{-14} \]

Given:
\[ [H⁺] = 3.3 \times 10^{-4} \text{ M} \]

To find \[ [OH⁻] \], rearrange the formula to:
\[ [OH⁻] = \frac{1.0 \times 10^{-14}}{[H⁺]} \]

Substitute the given [H⁺] value into the equation:
\[ [OH⁻] = \frac{1.0 \times 10^{-14}}{3.3 \times 10^{-4}} \]

Calculate:
\[ [OH⁻] = 3.03 \times 10^{-11} \text{ M} \]
Transcribed Image Text:**Question:** At 25°C, what is the hydroxide ion concentration, [OH⁻], in an aqueous solution with a hydrogen ion concentration of [H⁺] = 3.3 × 10⁻⁴ M? **Answer box:** ``` [OH⁻] = ___________________ M ``` **Explanation:** This question requires understanding the relationship between hydrogen ion concentration and hydroxide ion concentration in an aqueous solution at 25°C. Typically, this is involving the use of the water dissociation constant, Kw, which is 1.0 × 10⁻¹⁴ at 25°C. For a solution at 25°C: \[ [H⁺] \cdot [OH⁻] = 1.0 \times 10^{-14} \] Given: \[ [H⁺] = 3.3 \times 10^{-4} \text{ M} \] To find \[ [OH⁻] \], rearrange the formula to: \[ [OH⁻] = \frac{1.0 \times 10^{-14}}{[H⁺]} \] Substitute the given [H⁺] value into the equation: \[ [OH⁻] = \frac{1.0 \times 10^{-14}}{3.3 \times 10^{-4}} \] Calculate: \[ [OH⁻] = 3.03 \times 10^{-11} \text{ M} \]
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