# 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.

###### 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:

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.

99% (445 ratings) ###### 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?

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