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Chapter 10: Problem 6

Identify the conjugate acid鈥揵ase pairings in the reactions below: $$ \begin{array}{|l|l|l|l|l|} \hline \text { Reaction } & \text { Acid } & \text { Base } & \text { Conjugate Acid } & \text { Conjugate Base } \\ \hline \mathrm{H}_2 \mathrm{CO}_3+\mathrm{H}_2 \mathrm{O} \rightleftharpoons \mathrm{HCO}_3{ }^{-}+\mathrm{H}_3 \mathrm{O} & & & & \\ \hline \begin{array}{l} \mathrm{H}_2 \mathrm{PO}_4{ }^{-}+\mathrm{H}_2 \mathrm{O} \rightleftharpoons \mathrm{H}_3 \mathrm{PO}_4+ \\ \mathrm{OH}^{-} \end{array} & & & & \\ \hline \end{array} $$

Short Answer

Expert verified
In the first reaction, H鈧侰O鈧�/HCO鈧冣伝 and H鈧侽/H鈧僌鈦� are the conjugate acid-base pairs. In the second reaction, H鈧侾O鈧勨伝/H鈧働O鈧� and H鈧侽/OH鈦� are the pairs.

Step by step solution

01

Identify Reactants and Products

Write down the reactants and products for each reaction and identify the acid and base pairs.
02

Determine Proton Transfers

Look at which species donate protons (H鈦�) and which species accept protons. This will help to identify the acid-base pairs.
03

Identify Conjugate Acid-Base Pairs

For each acid that donates a proton, identify the corresponding conjugate base. For each base that accepts a proton, identify the corresponding conjugate acid.
04

Fill in the Table

Complete the table with the identified acids, bases, and their conjugates.

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Key Concepts

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

Acid-Base Reactions
In chemistry, acid-base reactions are fundamental processes. They form the basis of various chemical phenomena. You will often encounter these reactions both in academic settings and in real-life applications. An acid-base reaction usually involves the transfer of protons (H鈦�) between reactants. This process can be observed in a variety of reactions, such as the neutralization of acids by bases.

To identify acid-base reactions:
  • Start by noting the reactants and products.
  • Identify which species donate protons and which accept them.
  • Recognize the acids and bases in the equation.
Recognizing these key elements will help you zoom in on the core components of acid-base reactions, making it easier to understand the overall process.
Proton Transfer
Proton transfer is a critical part of acid-base reactions. This is the process where a proton (H鈦�) moves from one molecule to another. To understand this better, let's consider the nature of proton donors and acceptors.

  • An acid is a proton donor. It gives away an H鈦� ion in the reaction.
  • A base is a proton acceptor. It receives an H鈦� ion.
Proton transfer is evident in the following reaction: ewline ewline \text{\(H_2CO_3 + H_2O \rightleftharpoons HCO_3^{-} + H_3O^+\)}
In this case, H鈧侰O鈧� donates a proton to H鈧侽, resulting in HCO鈧冣伝 and H鈧僌鈦� as products. Identifying proton transfers helps to pinpoint which substances serve as acids and which serve as bases in a given reaction.
Conjugate Acids
Conjugate acids are the species formed when a base accepts a proton (H鈦�). Essentially, when a molecule or ion gains a proton, it becomes a conjugate acid. Understanding conjugate acids is essential for correctly identifying acid-base pairs.

For instance, consider the reaction: ewline ewline \text{\(H_2PO_4^{-} + H_2O \rightleftharpoons H_3PO_4 + OH^-\)}
In this reaction, H鈧侾O鈧勨伝 accepts a proton from H鈧侽 to form H鈧働O鈧�. Here, H鈧働O鈧� is the conjugate acid because it is formed when the base (H鈧侾O鈧勨伝) gains a proton. Always remember:
  • A conjugate acid has one more proton than its corresponding base.
This concept is critical in understanding the acid-base equilibrium in reactions.
Conjugate Bases
Conjugate bases are the species formed when an acid donates a proton (H鈦�). When an acid loses a proton, the remaining species is known as its conjugate base.

For example, examining the reaction: ewline ewline \text{\(H_2CO_3 + H_2O \rightleftharpoons HCO_3^{-} + H_3O^+\)}
Here, H鈧侰O鈧� donates a proton to H鈧侽 and becomes HCO鈧冣伝. Thus, HCO鈧冣伝 is the conjugate base of the acid H鈧侰O鈧�. Key points to remember include:
  • A conjugate base has one less proton than its corresponding acid.
  • It often carries a negative charge as a result of losing a proton.
Recognizing conjugate bases helps in the identification of acid-base pairs and understanding the dynamics of proton transfer during chemical reactions.

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Most popular questions from this chapter

What is the purpose of a buffer solution?

Identify which reactants are amphoteric species in the following reactions. For those species, determine if the compound is also amphiprotic. $$ \begin{array}{|l|l|l|} \hline \multicolumn{1}{|c|}{\text { Reaction }} & \text { Amphoteric Reactant } & \text { Amphiprotic? ( } \mathrm{Y} \text { or } \mathrm{N}) \\ \hline \mathrm{HCO}_3{ }^{-}+\mathrm{HBr} \rightleftharpoons \mathrm{H}_2 \mathrm{CO}_3+\mathrm{Br}^{-} & & \\ \hline \begin{array}{l} 3 \mathrm{HCl}+\mathrm{Al}(\mathrm{OH})_3 \rightleftharpoons \mathrm{AlCl}_3+3 \\\ \mathrm{H}_2 \mathrm{O} \end{array} & & \\ \hline 2 \mathrm{HBr}+\mathrm{ZnO} \rightleftharpoons \mathrm{ZnBr}_2+\mathrm{H}_2 \mathrm{O} & & \\ \hline \end{array} $$

What are the \(\mathrm{pH}\) and \(\mathrm{pOH}\) of a solution containing \(5 \mathrm{~mL}\) of \(5 \mathrm{M}\) benzoic acid \(\left(K_{\mathrm{a}}=\right.\) \(6.3 \times 10^{-5}\) ) and \(100 \mathrm{~mL}\) of \(0.005 \mathrm{M}\) benzoate solution?

In which part of the \(\mathrm{pH}\) range (acidic, basic, or neutral) will the equivalence points fall for each of the following titrations? \- Strong acid + weak base: \- Strong base + weak acid: \- Strong acid + strong base: \- Weak acid + weak base:

Utilizing Arrhenius acid naming trends, predict the acid formula and name for the following anions: $$ \begin{array}{|c|c|c|} \hline \text { Anion } & \text { Acid Formula } & \text { Acid Name } \\ \hline \mathrm{MnO}_4{ }^{-} & & \\ \hline \text { Titanate }\left(\mathrm{TiO}_3{ }^{2-}\right) & & \\ \hline \mathrm{I}^{-} & & \\ \hline \mathrm{IO}_4{ }^{-} & & \\ \hline \end{array} $$
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