At 25 °C, what is the hydroxide ion concentration, [OH-], in an aqueous solution with a hydrogen ion concentration of [H]-5.0 x 10⁹ M? [OH-] = 3.33 X10-7 Incorrect Attem 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⁺] = 5.0 × 10⁻⁹ M?
**Student Answer:**
\[ \text{[OH⁻]} = 3.33 \times 10^{-7} \, \text{M} \]
**Result:**
Incorrect
In this image, there is a question about calculating the hydroxide ion concentration in an aqueous solution. The hydrogen ion concentration is given as 5.0 × 10⁻⁹ M. The student attempted to solve the problem and submitted the answer 3.33 × 10⁻⁷ M, which was marked as incorrect.
To correctly find the hydroxide ion concentration ([OH⁻]), one can use the ion product of water (Kw) at 25°C, which is 1.0 × 10⁻¹⁴. The relationship between the hydrogen ion concentration and the hydroxide ion concentration is given by:
\[ \text{Kw} = [H⁺][OH⁻] \]
Given [H⁺] = 5.0 × 10⁻⁹ M:
\[ 1.0 \times 10^{-14} = (5.0 \times 10^{-9})[OH⁻] \]
\[ [OH⁻] = \frac{1.0 \times 10^{-14}}{5.0 \times 10^{-9}} \]
\[ [OH⁻] = 2.0 \times 10^{-6} \, \text{M} \]
Thus, the correct hydroxide ion concentration should be 2.0 × 10⁻⁶ M.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdc325aa0-3b4d-4100-824a-15814ab6662e%2Fa76a22c5-9c36-4953-adf7-ae5dd238fbf1%2Fx43hai_processed.jpeg&w=3840&q=75)
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