Multiple Choice
A volume of 10.0 mL of a 0.600 M HNO3 solution is titrated with 0.340 M KOH. Calculate the volume of KOH required to reach the equivalence point.
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18. Aqueous Equilibrium
Titrations: Strong Acid-Strong Base
Multiple Choice
In the titration of a 35.0 mL sample of 0.175 M HBr with 0.210 M KOH, what is the pH after adding 5.0 mL of base beyond the equivalence point?
A
2.85
B
7.00
C
11.00
D
12.15
Verified step by step guidance1
Determine the moles of HBr initially present using the formula: \( \text{moles of HBr} = \text{volume (L)} \times \text{molarity (M)} \).
Calculate the moles of KOH added at the equivalence point using the formula: \( \text{moles of KOH} = \text{volume (L)} \times \text{molarity (M)} \).
Find the moles of KOH added beyond the equivalence point by calculating the moles in the additional 5.0 mL of KOH.
Determine the excess moles of KOH by subtracting the initial moles of HBr from the total moles of KOH added.
Calculate the concentration of OH\(^-\) ions in the solution using the excess moles of KOH and the total volume of the solution, then find the pOH and convert it to pH using the relation: \( \text{pH} = 14 - \text{pOH} \).
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