Multiple Choice
Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)₂.
17. Acid and Base Equilibrium
pH of Strong Acids and Bases
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Consider the titration of a 35.0 mL sample of 0.175 M HBr with 0.200 M KOH. Determine the initial pH of the HBr solution before any KOH is added.
A
2.15
B
1.25
C
0.76
D
3.00
Verified step by step guidance1
Identify that HBr is a strong acid, which means it completely dissociates in water. The concentration of HBr will be equal to the concentration of H+ ions in the solution.
Write the dissociation equation for HBr: \( \text{HBr} \rightarrow \text{H}^+ + \text{Br}^- \).
Since HBr is a strong acid, the concentration of \( \text{H}^+ \) ions is the same as the initial concentration of HBr, which is 0.175 M.
Use the formula for pH, which is \( \text{pH} = -\log[\text{H}^+] \), to find the pH of the solution.
Substitute the concentration of \( \text{H}^+ \) (0.175 M) into the pH formula to calculate the initial pH of the HBr solution.
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