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Chapter 15: Problem 89

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.

Short Answer

Expert verified
Answer: All Arrhenius bases are Bronsted-Lowry bases, but not all Bronsted-Lowry bases are Arrhenius bases.

Step by step solution

01

Define an Arrhenius base

An Arrhenius base is a substance that increases the concentration of hydroxide ions (OH-) in aqueous solution when dissolved.
02

Define a Bronsted-Lowry base

A Bronsted-Lowry base is a substance that can accept a proton (H+) from another substance in a chemical reaction.
03

Compare Arrhenius bases to Bronsted-Lowry bases

All Arrhenius bases are Bronsted-Lowry bases because they increase the concentration of OH- ions in solution by accepting a proton (H+) from water to form hydroxide ions. Since the process of accepting a proton is a defining characteristic of a Bronsted-Lowry base, all Arrhenius bases satisfy this requirement.
04

Compare Bronsted-Lowry bases to Arrhenius bases

Not all Bronsted-Lowry bases are Arrhenius bases. Bronsted-Lowry bases encompass a wider variety of substances, since their definition only requires the ability to accept a proton. An Arrhenius base, on the other hand, specifically increases the concentration of hydroxide ions in the solution. Thus, some Bronsted-Lowry bases do not meet the criteria for being an Arrhenius base.
05

Provide an example of a Bronsted-Lowry base not being an Arrhenius base

An example of a Bronsted-Lowry base that is not an Arrhenius base is ammonia (NH3). When ammonia is added to water, it accepts a proton (H+) from water forming the ammonium ion (NH4+) and a hydroxide ion (OH-). The chemical reaction can be represented as: NH3 + H2O -> NH4+ + OH- In this case, ammonia is a Bronsted-Lowry base because it accepts a proton from water. However, it is not an Arrhenius base because it does not directly introduce hydroxide ions into the solution (rather, these are a product of its reaction with water).

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Key Concepts

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

Arrhenius Bases
Arrhenius bases are defined by their ability to increase the concentration of hydroxide ions (OH鈦�) in water.
This happens when they dissolve in water and separate into ions.
For example:
  • Sodium hydroxide (NaOH) dissolves in water to give hydroxide ions and sodium ions.
  • Potassium hydroxide (KOH) does the same, adding OH鈦� ions to the solution.
This definition is limited to cases where the substance actually releases OH鈦� ions directly into the aqueous solution.
Therefore, Arrhenius bases typically contain hydroxide in their formula.
It's important to note that this results in a basic or alkaline solution with a pH greater than 7.
Additionally, the Arrhenius definition mainly applies to aqueous solutions.
Bronsted-Lowry Bases
The concept of Bronsted-Lowry bases broadens the scope of bases beyond the Arrhenius definition.
According to Bronsted-Lowry theory, a base is any substance capable of accepting a proton (H鈦�) from another substance.
This definition doesn't require the direct release of OH鈦� ions.
Some examples include:
  • Ammonia (NH鈧�), which accepts protons from water to form ammonium (NH鈧勨伜) and OH鈦�.
  • Acetate ion (CH鈧僀OO鈦�), which can accept a proton to form acetic acid (CH鈧僀OOH).
This theory allows for a greater variety of substances to be classified as bases.
It includes not only aqueous solutions but also reactions in non-aqueous environments.
Ammonia NH3 as a Base
Ammonia (NH鈧�) is a classic example of a Bronsted-Lowry base that does not fit the Arrhenius definition.
When ammonia is added to water, it accepts a proton from water to form ammonium ions (NH鈧勨伜) and releases hydroxide ions (OH鈦�):\[\text{NH}_3 + \text{H}_2\text{O} \rightarrow \text{NH}_4^+ + \text{OH}^-\]This reaction allows ammonia to act as a base by increasing the concentration of OH鈦� ions, but not in the direct manner of an Arrhenius base.
Here are some key points about ammonia's behavior:
  • Ammonia's ability to accept protons makes it an excellent Bronsted-Lowry base.
  • Its indirect production of OH鈦� ions through interaction with water distinguishes it from most Arrhenius bases.
  • Due to its gaseous state at room temperature, it can enter into reactions easily in aqueous and gaseous forms.
These characteristics make ammonia a versatile base in various chemical reactions.

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Most popular questions from this chapter

Identify the acids and bases in the following reactions: a. \(\mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \rightarrow \mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(\ell)\) b. \(\mathrm{MgCO}_{3}(s)+2 \mathrm{HCl}(a q) \rightarrow\) \(\mathrm{MgCl}_{2}(a q)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(\ell)\) c. \(2 \mathrm{NH}_{3}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(a q)\)

Calculate the \(\mathrm{pH}\) and \(\mathrm{pOH}\) of the following solutions: a. stomach acid in which \([\mathrm{HCl}]=0.155 \mathrm{M}\) b. \(0.00500 M \mathrm{HNO}_{3}\) c. a 2: 1 mixture of \(0.0125 M \mathrm{HCl}\) and \(0.0125 M \mathrm{NaOH}\) d. a 3: 1 mixture of \(0.0125 M \mathrm{H}_{2} \mathrm{SO}_{4}\) and \(0.0125 \mathrm{MKOH}\)

Neutralizing the Smell of Fish Trimethylamine, \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N}\) \(\left(K_{\mathrm{b}}=6.5 \times 10^{-5} \text {at } 25^{\circ} \mathrm{C}\right),\) contributes to the "fishy" odor of not-so-fresh seafood. Some people squeeze fresh lemon juice (which contains a high concentration of citric acid) on cooked fish to reduce the fishy odor. Why is this practice effective?

For each of the molecular equations, write net ionic equations and identify the Bronsted-Lowry acids and bases: a. \(2 \mathrm{HNO}_{3}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \rightarrow\) \(2 \mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) b. \(\mathrm{Na}_{2} \mathrm{CO}_{3}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow\) \(\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(\ell)\) c. \(\mathrm{CH}_{3} \mathrm{NH}_{2}(a q)+\mathrm{HBr}(a q) \rightarrow\left(\mathrm{CH}_{3} \mathrm{NH}_{3}\right) \mathrm{Br}(a q)\) d. \(2 \mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(s) \rightarrow\) \(\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2} \mathrm{Mg}(a q)+2 \mathrm{H}_{2} \mathrm{O}(\ell)\) e. \(\mathrm{CaO}(s)+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{Ca}(\mathrm{OH})_{2}(s)\) f. \(\operatorname{LiH}(s)+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \operatorname{LiOH}(a q)+\mathrm{H}_{2}(g)\) g. \(\mathrm{Ba}(\mathrm{OH})_{2}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{BaSO}_{4}(s)+2 \mathrm{H}_{2} \mathrm{O}(\ell)\) h. \(\mathrm{NaSH}(a q)+\mathrm{HNO}_{3}(a q) \rightarrow \mathrm{NaNO}_{3}(a q)+\mathrm{H}_{2} \mathrm{S}(g)\)

Calculate the \(\mathrm{pH}\) and \(\mathrm{pOH}\) of the solutions with the following hydronium ion or hydroxide ion concentrations. Indicate which solutions are acidic, basic, or neutral. a. \(\left[\mathrm{OH}^{-}\right]=8.2 \times 10^{-11} \mathrm{M}\) b. \(\left[\mathrm{OH}^{-}\right]=7.7 \times 10^{-6} \mathrm{M}\) c. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=3.2 \times 10^{-4} \mathrm{M}\) d. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.0 \times 10^{-7} \mathrm{M}\)
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