Problem: You are asked to prepare a pH = 3.00 buffer solution starting from 1.25 L of a 1.00 M solution of hydrofluoric acid (HF) and an excess of sodium fluoride (NaF).How many grams of sodium fluoride should be added to prepare the buffer solution? Neglect the small volume change that occurs when the sodium fluoride is added.

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

FREE Expert Solution

We are asked how many grams of sodium fluoride should be added to prepare the buffer solution with a pH = 3.00 with 1.25 L of a 1.00 M solution of hydrofluoric acid (HF) and an excess of sodium fluoride (NaF).


Since the solution is a buffer, we can use the Henderson-Hasselbalch Equation to calculate the gram of NaF needed to have a pH of 3.00 with 1.25 L 1.00M solution of HF:


pH =pKa + log conjugate baseweak acid


In the solution, identify the weak acid and the conjugate base. 

Recall from the Bronsted-Lowry definition that an acid is a proton (H+) donor and the base is a proton (H+) acceptor.

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Problem Details

You are asked to prepare a pH = 3.00 buffer solution starting from 1.25 L of a 1.00 M solution of hydrofluoric acid (HF) and an excess of sodium fluoride (NaF).

How many grams of sodium fluoride should be added to prepare the buffer solution? Neglect the small volume change that occurs when the sodium fluoride is added.

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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 Buffer concept. You can view video lessons to learn Buffer. Or if you need more Buffer practice, you can also practice Buffer practice problems.

What professor is this problem relevant for?

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