At 25 °C, what is the hydroxide ion concentration, [OH], in an aqueous solution with a hydrogen ion concentration of [H]-1.8 x 10-6 M? Macmillan L [OH-] = M
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![**Transcription for Educational Website:**
**Problem Statement:**
At 25°C, what is the hydroxide ion concentration, \([OH^-]\), in an aqueous solution with a hydrogen ion concentration of \([H^+]=1.8 \times 10^{-6}\) M?
\[ [OH^-] = \underline{\hspace{3cm}} \text{M} \]
**Explanation:**
To find the hydroxide ion concentration, \([OH^-]\), we can use the water dissociation constant, \(K_w\), which is \(1.0 \times 10^{-14}\) at 25°C. The relationship between hydrogen ions and hydroxide ions in water is given by the equation:
\[ K_w = [H^+][OH^-] \]
Using the given hydrogen ion concentration:
\[ (1.8 \times 10^{-6} \, \text{M}) \times [OH^-] = 1.0 \times 10^{-14} \]
Solving for \([OH^-]\) will provide the hydroxide ion concentration.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8da5c625-81d8-4db3-9f61-2b28dd7af5ea%2Fb4c2f03d-8231-4693-9e58-c3af22f9be80%2Fy48kzg_processed.jpeg&w=3840&q=75)
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