Multiple Choice
Consider the titration of 575.00 mL of HCl with a pH of 1.34. How much 0.0300 M NaOH (in mL) needs to be added to reach the equivalence point?
18. Aqueous Equilibrium
Titrations: Strong Acid-Strong Base
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Determine the pH at the equivalence point for a titration of 50 mL of 0.1 M KOH with 0.1 M HClO4.
A
pH = 7
B
pH = 9
C
pH = 5
D
pH = 3
Verified step by step guidance1
Identify the type of titration: This is a strong base (KOH) titrated with a strong acid (HClO4). In such titrations, the pH at the equivalence point is determined by the neutralization of the base and acid.
Calculate the moles of KOH: Use the formula \( \text{moles} = \text{concentration} \times \text{volume} \). For KOH, \( \text{moles} = 0.1 \text{ M} \times 0.050 \text{ L} \).
Determine the moles of HClO4 needed: Since the reaction is a 1:1 stoichiometry, the moles of HClO4 required to reach the equivalence point are equal to the moles of KOH calculated in the previous step.
Calculate the total volume at the equivalence point: Add the initial volume of KOH (50 mL) to the volume of HClO4 added to reach the equivalence point. Since the concentrations are equal, the volume of HClO4 added will also be 50 mL, making the total volume 100 mL or 0.1 L.
Determine the pH at the equivalence point: For a strong acid-strong base titration, the solution at the equivalence point is neutral, meaning the pH is 7. This is because the resulting solution is composed of water and the salt KClO4, which does not affect the pH.
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