# 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. 5.94B. 8.06C. 7.75D. 8.30E. 11.61

###### FREE Expert Solution
91% (388 ratings)
###### FREE Expert 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.

91% (388 ratings)
###### Problem Details

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

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Weak Acid Strong Base Titrations concept. You can view video lessons to learn Weak Acid Strong Base Titrations. Or if you need more Weak Acid Strong Base Titrations practice, you can also practice Weak Acid Strong Base Titrations practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofCalculate the pH at the equivalence point from the titration...as high difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Sabrina took 11 minutes and 26 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

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