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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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Most popular questions from this chapter

The awful odor of dead fish is due mostly to trimethylamine, \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N},\) one of three compounds related to ammonia in which methyl groups replace one, two, or all three of the \(\mathrm{H}\) atoms in ammonia. a. The \(K_{\mathrm{b}}\) of trimethylamine \(\left[\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N}\right]\) is \(6.5 \times\) \(10^{-5}\) at \(25^{\circ} \mathrm{C} .\) Calculate the \(\mathrm{pH}\) of \(3.00 \times 10^{-4} M\) trimethylamine. b. The \(K_{\mathrm{b}}\) of methylamine \(\left[\left(\mathrm{CH}_{3}\right) \mathrm{NH}_{2}\right]\) is \(4.4 \times 10^{-4}\) at \(25^{\circ} \mathrm{C} .\) Calculate the \(\mathrm{pH}\) of \(2.88 \times 10^{-3} \mathrm{M}\) methylamine. "c. The \(K_{\mathrm{b}}\) of dimethylamine \(\left[\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH}\right]\) is \(5.9 \times 10^{-4}\) at \(25^{\circ} \mathrm{C} .\) What concentration of dimethylamine is needed for the solution to have the same \(\mathrm{pH}\) as the solution in part b?

The \(K_{\mathrm{b}}\) of aminoethanol, \(\mathrm{HOCH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2},\) is \(3.1 \times 10^{-5}\) a. Is aminoethanol a stronger or weaker base than ethylamine, \(\mathrm{p} K_{\mathrm{b}}=3.36 ?\) b. Calculate the \(\mathrm{pH}\) of \(1.67 \times 10^{-2} \mathrm{M}\) aminoethanol. c. Calculate the [OH \(\left.^{-}\right]\) concentration of \(4.25 \times 10^{-4} M\) aminoethanol.

Are all Arrhenius bases also Bronsted-Lowry bases? Are \(15.9=\) all Bronsted-Lowry bases also Arrhenius bases? If yes, explain why. If not, give a specific example to demonstrate the difference.

What is the pH of \(5.00 \times 10^{-4} \mathrm{MH}_{2} \mathrm{SO}_{4} ?\)

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