Multiple Choice
What is the pH of a 2.8 M solution of HClO_4, assuming complete dissociation?
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17. Acid and Base Equilibrium
pH of Strong Acids and Bases
Multiple Choice
The pH of a M solution of (assume complete dissociation at 25 °C) is closest to:
A
B
C
D
Verified step by step guidance1
Recognize that calcium hydroxide, Ca(OH)₂, is a strong base and dissociates completely in water according to the equation: \(\text{Ca(OH)}_2 \rightarrow \text{Ca}^{2+} + 2\text{OH}^-\).
Calculate the hydroxide ion concentration, \([\text{OH}^-]\), by multiplying the initial concentration of Ca(OH)₂ by 2, since each formula unit produces 2 hydroxide ions: \([\text{OH}^-] = 2 \times 0.0040\,M\).
Use the hydroxide ion concentration to find the pOH of the solution using the formula: \(\text{pOH} = -\log [\text{OH}^-]\).
Calculate the pH from the pOH using the relationship at 25 °C: \(\text{pH} = 14 - \text{pOH}\).
Compare the calculated pH value to the given options to determine which is closest to the correct pH.
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