Problem 101 Identify whether each of the rea... [FREE SOLUTION]

Chapter 23: Problem 101

Identify whether each of the reactants in these reactions is acting as an acid or a base. (Chapter 18) a. \(HBr+H_{2} O \rightarrow H_{3} O^{+}+Br^{-}\) b. \(NH_{3}+HCOOH \rightarrow NH_{4}^{+}+HCOO^{-}\) c. \(HCO_{3}^{-}+H_{2} O \rightarrow CO_{3}^{-}+H_{3} O^{+}\)

Short Answer

Expert verified

In summary: a. In the reaction \(HBr + H_{2}O \rightarrow H_{3}O^{+} + Br^{-}\), HBr is acting as an acid and \(H_{2}O\) is acting as a base. b. In the reaction \(NH_{3}+HCOOH \rightarrow NH_{4}^{+}+HCOO^{-}\), HCOOH is acting as an acid and \(NH_{3}\) is acting as a base. c. In the reaction \(HCO_{3}^{-}+H_{2}O \rightarrow CO_{3}^{-}+H_{3}O^{+}\), \(HCO_{3}^{-}\) is acting as an acid and \(H_{2}O\) is acting as a base.

Step by step solution

Reaction a: \((\)HBr+H_{2}O \rightarrow H_{3}O^{+}+Br^{-}\()\)

In this reaction, the reactant HBr donates a proton (H鈦�) to H鈧侽, resulting in the formation of H鈧僌鈦� and Br鈦�. According to the Br酶nsted-Lowry definition, HBr acts as an acid, while H鈧侽 acts as a base.

Reaction b: \((\)NH_{3}+HCOOH \rightarrow NH_{4}^{+}+HCOO^{-}\()\)

In this reaction, the reactant HCOOH donates a proton (H鈦�) to NH鈧�, resulting in the formation of NH鈧勨伜 and HCOO鈦�. According to the Br酶nsted-Lowry definition, HCOOH acts as an acid, while NH鈧� acts as a base.

Reaction c: \((\)HCO_{3}^{-}+H_{2}O \rightarrow CO_{3}^{-}+H_{3}O^{+}\()\)

In this reaction, the reactant HCO鈧冣伝 donates a proton (H鈦�) to H鈧侽, resulting in the formation of CO鈧兟测伝 and H鈧僌鈦�. According to the Br酶nsted-Lowry definition, HCO鈧冣伝 acts as an acid, while H鈧侽 acts as a base. In summary: a. HBr is an acid, H鈧侽 is a base b. HCOOH is an acid, NH鈧� is a base c. HCO鈧冣伝 is an acid, H鈧侽 is a base

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Key Concepts

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

Proton Transfer

Proton transfer is a key process in many chemical reactions, especially in the context of acid-base chemistry. When a proton ( H鈦� ) is transferred from one molecule to another, it often results in the formation of a new substance and changes the nature of the reactants. This simple movement can determine whether a molecule behaves as an acid or a base according to the Br酶nsted-Lowry theory.

This theory defines acids as proton donors and bases as proton acceptors.

During proton transfer, the acid loses a proton.
The base gains a proton.

This interchange is crucial for the understanding of many biochemical pathways and industrial processes. It's the basic principle behind the behavior of acids and bases.

Acid-Base Reactions

Acid-base reactions involve the exchange of protons between reactants. These reactions are essential to understanding numerous natural and industrial processes. The Br酶nsted-Lowry theory provides a framework for identifying acids and bases in these reactions.

In a typical acid-base reaction:

The acid gives up a proton, becoming its conjugate base.
The base accepts the proton, becoming its conjugate acid.

For example, in the reaction NH鈧� + HCOOH 鈫� NH鈧勨伜 + HCOO鈦�, HCHO relinquishes a proton to NH鈧�. Therefore, HCOOH acts as an acid, whereas NH鈧� is the base. Understanding these dynamics helps predict the outcome of the reaction and the nature of the resulting compounds.

HBr as an Acid

Hydrobromic acid ( HBr ) is a classic example of a strong acid in Br酶nsted-Lowry theory. It effortlessly donates its proton to nearby water molecules, demonstrating its strength as an acid. This exchange is seen in the reaction: HBr + H鈧侽鈫� H鈧僌鈦� + Br鈦�.

Here, HBr serves as a proton donor, which defines it as an acid. The resulting hydronium ion ( H鈧僌鈦� ) exhibits increased acidity in water, with bromide ion ( Br鈦� ) as the resultant conjugate base. Knowing HBr's behavior is essential in understanding how strong acids fully ionize in water, impacting the pH level significantly.

HCOOH as an Acid

Formic acid ( HCOOH ) is a relatively weak acid compared to strong acids like HBr . However, it still functions as an acid by donating a proton in acid-base reactions. In the context of the reaction: HCOOH + NH鈧� 鈫� NH鈧勨伜 + HCOO鈦�, HCOOH is the acid because it donates a proton to ammonia ( NH鈧� ), forming an ammonium ion ( NH鈧勨伜 ) and the conjugate base, formate ion ( HCOO鈦� ).

This illustrates how even weak acids like HCOOH can engage in proton transfer to form new compounds, emphasizing their role in chemical processes despite their lower acidity.

HCO鈧冣伝 as an Acid

Bicarbonate ions ( HCO鈧冣伝 ) highlight an interesting aspect of acid-base chemistry. Though often considered basic, HCO鈧冣伝 can act as an acid, donating a proton to a base such as water. This behavior is seen in the reaction: HCO鈧冣伝 + H鈧侽鈫� CO鈧兟测伝 + H鈧僌鈦�.

In this case, HCO鈧冣伝 donates a proton to water, forming a carbonate ion ( CO鈧兟测伝 ) and hydronium ion ( H鈧僌鈦� ). It shows HCO鈧冣伝's dual role as both an acid and a conjugate base, which is central to many natural processes, like blood buffering. This dual capability makes it significant in maintaining pH stability in various chemical and biological systems.

91影视

Identify whether each of the reactants in these reactions is acting as an acid or a base. (Chapter 18) a. \(HBr+H_{2} O \rightarrow H_{3} O^{+}+Br^{-}\) b. \(NH_{3}+HCOOH \rightarrow NH_{4}^{+}+HCOO^{-}\) c. \(HCO_{3}^{-}+H_{2} O \rightarrow CO_{3}^{-}+H_{3} O^{+}\)

Short Answer

Step by step solution

Reaction a: \((\)HBr+H_{2}O \rightarrow H_{3}O^{+}+Br^{-}\()\)

Reaction b: \((\)NH_{3}+HCOOH \rightarrow NH_{4}^{+}+HCOO^{-}\()\)

Reaction c: \((\)HCO_{3}^{-}+H_{2}O \rightarrow CO_{3}^{-}+H_{3}O^{+}\()\)

Key Concepts

Proton Transfer

Acid-Base Reactions

HBr as an Acid

HCOOH as an Acid

HCO鈧冣伝 as an Acid

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