Multiple Choice
What is the pH of a solution at ? Assume is a strong base that dissociates completely.
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17. Acid and Base Equilibrium
pH of Strong Acids and Bases
Multiple Choice
What is the pH of a solution at (assume complete dissociation)?
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Verified step by step guidance1
Identify that NaOH is a strong base and dissociates completely in water, so the concentration of OH⁻ ions is equal to the concentration of NaOH, which is 0.001 M.
Calculate the pOH of the solution using the formula: \(\text{pOH} = -\log[\text{OH}^-]\).
Use the relationship between pH and pOH at 25°C: \(\text{pH} + \text{pOH} = 14\).
Rearrange the equation to find pH: \(\text{pH} = 14 - \text{pOH}\).
Substitute the pOH value into the equation to find the pH of the solution.
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