Multiple Choice
The pH of a M solution of (assume complete dissociation at 25 °C) is closest to:
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17. Acid and Base Equilibrium
pH of Strong Acids and Bases
Multiple Choice
At 25 °C, what is the pH of a M aqueous solution of sodium hydroxide, , assuming it dissociates completely?
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Verified step by step guidance1
Identify that sodium hydroxide (NaOH) is a strong base and dissociates completely in water, so the concentration of OH⁻ ions is equal to the initial concentration of NaOH, which is 1.00 × 10⁻¹ M.
Calculate the pOH of the solution using the formula: \(\text{pOH} = -\log[\text{OH}^-]\), where \([\text{OH}^-]\) is the hydroxide ion concentration.
Use the relationship between pH and pOH at 25 °C, which is: \(\text{pH} + \text{pOH} = 14.00\).
Rearrange the equation to solve for pH: \(\text{pH} = 14.00 - \text{pOH}\).
Substitute the calculated pOH value into the equation to find the pH of the solution.
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