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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 (NH鈧�) and water (H鈧侽) 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鈦�) in the solution. 2. Bronsted-Lowry base: It accepts a proton (H鈦�) from water, forming ammonium ion (NH鈧勨伜). 3. Lewis base: It donates a pair of electrons from the nitrogen atom to form a bond with a proton (H鈦�) from water, creating NH鈧勨伜.

Step by step solution

01

Write out the reaction between ammonia and water

Write the chemical equation representing the reaction between ammonia (NH鈧�) and water (H鈧侽) 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鈦�) 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鈦�). Therefore, ammonia meets the criteria of an Arrhenius base as it increases the concentration of OH鈦� 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鈦�) from another substance. Analyzing the reaction equation in Step 1, we see that ammonia (NH鈧�) accepts a proton (H鈦�) from water, forming the ammonium ion (NH鈧勨伜). 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鈦�) from water, it creates the ammonium ion (NH鈧勨伜). 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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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Arrhenius Base
In chemistry, the Arrhenius base definition focuses on the presence of hydroxide ions. An Arrhenius base increases the hydroxide ion concentration
  • Arrhenius bases in aqueous solutions boost hydroxide ions (OH鈦�).
  • Ammonia, when dissolved in water, results in the production of hydroxide ions.
For ammonia, the equation \[ NH_3(aq) + H_2O(l) \rightleftharpoons NH_4^+(aq) + OH^-(aq) \] illustrates the increase in the concentration of hydroxide ions.
The produced OH鈦� ions elevate the solution's basicity.
Hence, ammonia is an Arrhenius base since it increases the OH鈦� ions.
Bronsted-Lowry Base
The Bronsted-Lowry theory takes a different angle by focusing on proton transfer. Here, a base is a proton acceptor:
  • Protons are simply hydrogen atoms missing an electron, represented by H鈦�.
  • A Bronsted-Lowry base accepts these protons, forming a new substance.
For ammonia,
  • In the equation \( NH_3(aq) \), ammonia accepts the \( H^+ \) from water \( H_2O \).
  • This forms the ammonium ion \( NH_4^+ \).
These actions classify ammonia as a Bronsted-Lowry base.
Lewis Base
Under the Lewis theory, bases donate electron pairs. This widens the definition of a base even more:
  • A Lewis base is any compound that can donate an electron pair to form a bond.
  • This doesn鈥檛 involve protons directly, as in Bronsted-Lowry.
For ammonia:
  • The nitrogen atom has a lone pair of electrons.
  • When ammonia acts with water, it donates this electron pair to an \( H^+ \) ion from water.
  • It forms a bond, resulting in an \( NH_4^+ \) ion.
Thus, ammonia's ability to donate its electron pair makes it a Lewis base.

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Most popular questions from this chapter

Identify the Bronsted-Lowry acid and the Bronsted-Lowry base on the left side of each equation, and also identify the conjugate acid and conjugate base of each on the right side. (a) \(\mathrm{HBrO}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{BrO}^{-}(a q)\) (b) \(\mathrm{HSO}_{4}^{-}(a q)+\mathrm{HCO}_{3}^{-}(a q) \rightleftharpoons\) \(\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\mathrm{SO}_{4}^{2-}(a q)+\mathrm{H}_{2} \mathrm{CO}_{3}(a q)\) (c) \(\mathrm{HSO}_{3}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q) \rightleftharpoons \mathrm{H}_{2} \mathrm{SO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\)

If a solution of \(\mathrm{HF}\left(K_{a}=6.8 \times 10^{-4}\right)\) has a pH of \(3.65,\) calculate the concentration of hydrofluoric acid.

Calculate the \(\mathrm{pH}\) of each of the following strong acid solutions: \((\mathbf{a}) 8.5 \times 10^{-3} \mathrm{M} \mathrm{HBr},(\mathbf{b}) 1.52 \mathrm{g}\) of \(\mathrm{HNO}_{3}\) in 575 \(\mathrm{mL}\) of solution, \((\mathbf{c}) 5.00 \mathrm{mL}\) of 0.250 \(\mathrm{M} \mathrm{ClO}_{4}\) diluted to 50.0 \(\mathrm{mL}\) (d) a solution formed by mixing 10.0 \(\mathrm{mL}\) of 0.100 \(\mathrm{M} \mathrm{HBr}\) with 20.0 \(\mathrm{mL}\) of 0.200 \(\mathrm{M} \mathrm{HCl} .\)

Write the chemical equation and the \(K_{a}\) expression for the ionization of each of the following acids in aqueous solution. First show the reaction with \(\mathrm{H}^{+}(a q)\) as a product and then with the hydronium ion: (a) \(\mathrm{HBrO}_{2},\) (b) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{COOH} .\)

Calculate the molar concentration of \(\mathrm{OH}^{-}\) in a 0.724 \(\mathrm{M}\) solution of hypobromite ion \(\left(\mathrm{BrO}^{-} ; K_{b}=4.0 \times 10^{-6}\right) .\) What is the pH of this solution?
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