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Chapter 14: Problem 101

$$ \begin{aligned} &\text { Complete the following table: (14.2) } \\ &\begin{array}{ll} \text { Acid } & \text { Conjugate Base } \\ \text { HI } & \\ & \mathrm{Cl}^{-} \\ \mathrm{NH}_{4}^{+} & \\ & \mathrm{HS}^{-} \end{array} \end{aligned} $$

Short Answer

Expert verified
HI -> I鈦�, Cl鈦� <- HCl, NH鈧勨伜 -> NH鈧�, HS鈦� <- H鈧係.

Step by step solution

01

- Identify the conjugate base for HI

To find the conjugate base of an acid, remove one proton (H鈦�) from the acid. For HI, the conjugate base is I鈦�.
02

- Identify the acid for Cl鈦�

The conjugate base Cl鈦� comes from the dissociation of HCl. Thus, the acid form is HCl.
03

- Identify the conjugate base for NH鈧勨伜

Remove one proton (H鈦�) from NH鈧勨伜 to form its conjugate base, which is NH鈧�.
04

- Identify the acid for HS鈦�

The conjugate base HS鈦� can be derived from the dissociation of H鈧係. Therefore, the acid form is H鈧係.

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Key Concepts

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

acid-base chemistry
Acid-base chemistry focuses on the interactions between acids and bases. It's a core topic in chemistry that helps us understand many chemical reactions.
Acids are substances that can donate protons (H鈦� ions), while bases are substances that can accept protons.
The Bronsted-Lowry theory is often used to explain acid-base reactions.
According to this theory:
  • An acid donates a proton, resulting in the formation of its conjugate base.
  • A base accepts a proton, resulting in the formation of its conjugate acid.

This means acids and bases always come in pairs known as conjugate acid-base pairs. Understanding these pairs is crucial for predicting the outcomes of many chemical reactions.
For example, when hydrochloric acid (HCl) donates a proton, it forms its conjugate base, the chloride ion (Cl鈦�).
conjugate base identification
Identifying the conjugate base of an acid is a straightforward process that involves removing a proton from the acid.
Let's look at some examples to illustrate this concept:
  • HI (hydroiodic acid) loses a proton to form I鈦� (iodide). So, the conjugate base of HI is I鈦�.
  • HCl (hydrochloric acid) loses a proton to form Cl鈦� (chloride). So, the conjugate base of HCl is Cl鈦�.
  • NH鈧勨伜 (ammonium) loses a proton to form NH鈧� (ammonia). So, the conjugate base of NH鈧勨伜 is NH鈧�.

In each case, identifying the conjugate base is just a matter of removing one proton (H鈦�) from the acid.
This concept is crucial when working with acid-base reactions, as it helps predict how acids and bases will behave in a chemical reaction.
proton transfer
Proton transfer is the process by which a proton (H鈦� ion) moves from one molecule or ion to another.
This is the fundamental mechanism behind acid-base reactions.
When an acid donates a proton, this proton is accepted by a base.
The strength of acids and bases depends on their ability to donate or accept protons.
  • Strong acids easily donate protons and have weak conjugate bases.
  • Weak acids do not donate protons as readily and have stronger conjugate bases.
  • Strong bases readily accept protons and are formed from weak acids.

For example, in the reaction between HCl and water, HCl donates a proton to water, forming H鈧僌鈦� (hydronium) and Cl鈦� (chloride).
The transfer of protons is what drives the acid-base reaction, and understanding this transfer process is key to mastering acid-base chemistry.

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Most popular questions from this chapter

A solution with a pH of 3 is 10 times more acidic than a solution with \(\mathrm{pH} 4\). Explain.

Complete and balance each of the following: (14.7) a. \(\mathrm{HCl}(a q)+\mathrm{LiOH}(s) \longrightarrow\) b. \(\mathrm{MgCO}_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow\)

Calculate the volume, in milliliters, of a \(0.215 \mathrm{M} \mathrm{NaOH}\) solution that will completely neutralize each of the following: (14.8) a. \(3.80 \mathrm{~mL}\) of a \(1.25 \mathrm{M} \mathrm{HNO}_{3}\) solution b. \(8.50 \mathrm{~mL}\) of a \(0.825 \mathrm{M} \mathrm{H}_{3} \mathrm{PO}_{4}\) solution

State whether each of the following solutions is acidic, basic, or neutral: a. blood plasma, \(\mathrm{pH} 7.38\) b. vinegar, \(\mathrm{pH} 2.8\) c. drain cleaner, \(\mathrm{pOH} 2.8\) d. coffee, \(\mathrm{pH} 5.52\) e. tomatoes, \(\mathrm{pH} 4.2\) f. chocolate cake, \(\mathrm{pH} 7.6\)

In an acidic solution, how does the concentration of \(\mathrm{H}_{3} \mathrm{O}^{+}\) compare to the concentration of \(\mathrm{OH}^{-}\) ?
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