Multiple Choice
Which of the following compounds will form an aqueous solution with a pH higher than 7?
17. Acid and Base Equilibrium
Acids Introduction
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A 850.0 mL sample of 0.20 M HF is titrated with 0.10 M NaOH. Determine the pH of the solution after the addition of 850.0 mL of NaOH. The Ka of HF is 6.8 x 10^-4.
A
pH = 8.20
B
pH = 7.00
C
pH = 3.45
D
pH = 5.00
Verified step by step guidance1
Calculate the initial moles of HF using the formula: \( \text{moles of HF} = \text{volume (L)} \times \text{molarity (M)} \).
Calculate the moles of NaOH added using the formula: \( \text{moles of NaOH} = \text{volume (L)} \times \text{molarity (M)} \).
Determine the limiting reactant by comparing the moles of HF and NaOH. Since they react in a 1:1 ratio, the smaller number of moles will be the limiting reactant.
Calculate the moles of HF remaining and the moles of F\(^-\) produced after the reaction. Use the stoichiometry of the reaction: \( \text{HF} + \text{NaOH} \rightarrow \text{NaF} + \text{H}_2\text{O} \).
Use the Henderson-Hasselbalch equation to find the pH: \( \text{pH} = \text{pK}_a + \log \left( \frac{[\text{F}^-]}{[\text{HF}]} \right) \), where \( \text{pK}_a = -\log(\text{K}_a) \).
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