Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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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.
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Transcribed Image Text:**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.
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