Chemistry Practice Problems Weak Acid Strong Base Titrations Practice Problems Solution: Calculate the pH at the equivalence point from the...

🤓 Based on our data, we think this question is relevant for Professor Eichler's class at UCR.

Solution: Calculate the pH at the equivalence point from the titration of 80.00 mL of 0.140 M hydrofluoric acid, HF, with 160.00 mL of 0.0700 M NaOH. Ka of HF is 3.5 x 10-4.A. 5.94B. 8.06C. 7.75D. 8.30E. 11.61

Problem

Calculate the pH at the equivalence point from the titration of 80.00 mL of 0.140 M hydrofluoric acid, HF, with 160.00 mL of 0.0700 M NaOH. Ka of HF is 3.5 x 10-4.

A. 5.94

B. 8.06

C. 7.75

D. 8.30

E. 11.61

Solution

We are being asked to calculate the pH at the equivalence point in the titration hydrofluoric acid (HF) with NaOH.


We will calculate the pH of the solution at the equivalence point using the following steps:

Step 1. Write the chemical equation for the reaction between HF and NaOH.
Step 2. Calculate the initial amounts of HF and NaOH in moles before the reaction happens.
Step 3. Construct an ICF Chart.
Step 4. Calculate the new concentration of the species left in the solution.
Step 5. Calculate pH.


Step 1. Write the chemical equation for the reaction between HF and NaOH.

Solution BlurView Complete Written Solution