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Chapter 16: Problem 93

Ammonia, \(\mathrm{NH}_{3},\) acts as an Arrhenius base, a Bronsted-Lowry base, and a Lewis base, in aqueous solution. Write out the reaction \(\mathrm{NH}_{3}\) undergoes with water and explain what properties of ammonia correspond to each of the three definitions of "base."

Short Answer

Expert verified
The reaction between ammonia (NH₃) and water (H₂O) is given by: \[ NH_3(aq) + H_2O(l) \rightleftharpoons NH_4^+(aq) + OH^-(aq) \] Ammonia fits all three base definitions: 1. Arrhenius base: It increases the concentration of hydroxide ions (OH⁻) in the solution. 2. Bronsted-Lowry base: It accepts a proton (H⁺) from water, forming ammonium ion (NH₄⁺). 3. Lewis base: It donates a pair of electrons from the nitrogen atom to form a bond with a proton (H⁺) from water, creating NH₄⁺.

Step by step solution

01

Write out the reaction between ammonia and water

Write the chemical equation representing the reaction between ammonia (NH₃) and water (H₂O) as follows: \[ NH_3(aq) + H_2O(l) \rightleftharpoons NH_4^+(aq) + OH^-(aq) \]
02

Explain how ammonia acts as an Arrhenius base

According to the Arrhenius definition, a base is a substance that increases the concentration of hydroxide ions (OH⁻) in an aqueous solution. From the reaction equation in Step 1, we can see that when ammonia reacts with water, one of the products is a hydroxide ion (OH⁻). Therefore, ammonia meets the criteria of an Arrhenius base as it increases the concentration of OH⁻ ions in the solution.
03

Explain how ammonia acts as a Bronsted-Lowry base

A Bronsted-Lowry base is a substance that can accept a proton (H⁺) from another substance. Analyzing the reaction equation in Step 1, we see that ammonia (NH₃) accepts a proton (H⁺) from water, forming the ammonium ion (NH₄⁺). Therefore, ammonia fulfills the Bronsted-Lowry definition of a base, as it accepts a proton from another substance (water, in this case).
04

Explain how ammonia acts as a Lewis base

A Lewis base is a substance that can donate a pair of electrons to form a bond with another substance. In the reaction between ammonia and water, the nitrogen atom in ammonia has a lone pair of electrons. When the nitrogen atom donates this lone pair of electrons to form a bond with a proton (H⁺) from water, it creates the ammonium ion (NH₄⁺). This ability to donate a pair of electrons to form a bond with another substance (proton in this case) makes ammonia a Lewis base.

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Most popular questions from this chapter

Butyric acid is responsible for the foul smell of rancid butter. The \(\mathrm{pK}_{a}\) of butyric acid is 4.84 (a) Calculate the pK \(_{b}\) for the butyrate ion. (b) Calculate the pH of a 0.050 \(M\) solution of butyric acid. (c) Calculate the pH of a 0.050\(M\) solution of sodium butyrate.

Calculate the concentration of an aqueous solution of NaOH that has a pH of 11.50.

Predict which member of each pair produces the more acidic aqueous solution: (a) \(\mathrm{K}^{+}\) or \(\mathrm{Cu}^{2+},(\mathbf{b}) \mathrm{Fe}^{2+}\) or \(\mathrm{Fe}^{3+}\) , (c) \(\mathrm{Al}^{3+}\) or \(\mathrm{Ga}^{3+}\) .

(a) Which of the following is the stronger Bronsted-Lowry acid, \(\mathrm{HClO}_{3}\) or \(\mathrm{HClO}_{2} ?\) (b) Which is the stronger Bronsted-Lowry base, \(\mathrm{HS}^{-}\) or \(\mathrm{HSO}_{4}^{-}\) ?

Pyridinium bromide \(\left(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NHBr}\right)\) is a strong electrolyte that dissociates completely into \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NH}^{+}\) and \(\mathrm{Br}^{-} .\) An aqueous solution of pyridinium bromide has a pH of \(2.95 .\) (a) Write out the reaction that leads to this acidic pH. (b) Using Appendix D, calculate the \(K_{a}\) for pyridinium bromide. (c) A solution of pyridinium bromide has a pH of 2.95 . What is the concentration of the pyridinium cation atequilibrium, in units of molarity?
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