Multiple Choice
What is the pH of a M solution of hydrobromic acid, HBr, assuming it behaves as a strong acid and water autoionization is negligible?
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17. Acid and Base Equilibrium
pH of Strong Acids and Bases
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Calculate the pH of a 25 mL of 5.45 × 10−2 M LiOH solution.
A
1.264
B
12.736
C
0.338
D
11.134
Verified step by step guidance1
Start by understanding that LiOH is a strong base, which means it dissociates completely in water. Therefore, the concentration of OH⁻ ions in the solution is equal to the concentration of LiOH.
Use the formula for pOH: \( \text{pOH} = -\log[\text{OH}^-] \). Substitute the concentration of OH⁻ ions, which is 5.45 × 10⁻² M, into this formula to find the pOH.
Recall the relationship between pH and pOH: \( \text{pH} + \text{pOH} = 14 \). Use this equation to solve for the pH once you have calculated the pOH.
Substitute the calculated pOH value into the equation \( \text{pH} = 14 - \text{pOH} \) to find the pH of the solution.
Ensure that your final pH value makes sense for a basic solution, as LiOH is a strong base. The pH should be greater than 7.
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