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Chapter 15: Problem 11

In an aqueous solution of HF, which compound acts as a Bronsted-Lowry acid and which is the Bronsted-Lowry base?

Short Answer

Expert verified
Answer: In an aqueous solution of HF, the HF molecule acts as a Bronsted-Lowry acid and the water molecule (H2O) acts as a Bronsted-Lowry base.

Step by step solution

01

Recall the Bronsted-Lowry Theory

The Bronsted-Lowry theory defines an acid as a substance that can donate a proton (H+) and a base as a substance that can accept a proton. In an aqueous solution, it is common that water molecules act as either a Bronsted-Lowry acid or base.
02

Write the chemical equation for the HF dissociation in water

When HF is added to water, it dissociates and reacts with water molecules. The chemical equation for this process is: HF(aq) + H2O(l) 鈬� H3O+(aq) + F鈭�(aq)
03

Identify the compound that donates a proton

In the equation, HF donates a proton (H+) to a water molecule. This transfer of proton results in the formation of H3O+(aq), which is also called the hydronium ion: HF(aq) 鈫� H+ + F鈭� Thus, the HF molecule is the Bronsted-Lowry acid in this aqueous solution.
04

Identify the compound that accepts a proton

In the equation from Step 2, a water molecule (H2O) accepts a proton from HF: H2O(l) + H+ 鈫� H3O+ Thus, the water molecule (H2O) is the Bronsted-Lowry base in this aqueous solution.
05

Summarize the results

In an aqueous solution of HF, the compound that acts as a Bronsted-Lowry acid is the HF molecule, and the compound that acts as the Bronsted-Lowry base is the water molecule (H2O).

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