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Chapter 15: Problem 10

Is the conjugate base of a strong acid always a spectator ion? Explain.

Short Answer

Expert verified
Yes, the conjugate base of a strong acid is usually a spectator ion as it remains unchanged in reactions.

Step by step solution

01

Understand the Concept of a Strong Acid

Strong acids are acids that completely dissociate in water. This means they release all of their hydrogen ions into the solution and leave behind their conjugate bases. Examples of strong acids include hydrochloric acid (HCl), sulfuric acid (H鈧係O鈧�), and nitric acid (HNO鈧�).
02

Identify the Conjugate Base

When a strong acid donates a proton (H鈦�), the remaining part of the acid that is left is known as the conjugate base. For instance, when HCl dissociates into H鈦� and Cl鈦�, the chloride ion (Cl鈦�) is the conjugate base of hydrochloric acid.
03

Examine the Role of the Conjugate Base

Conjugate bases of strong acids in aqueous solutions typically do not participate significantly in chemical reactions. Since strong acids completely dissociate in solution, their conjugate bases are often very weak bases and do not readily gain hydrogen ions, participating minimally in the equilibrium of acid-base reactions.
04

Define a Spectator Ion

A spectator ion is an ion that exists in the same form on both the reactant and product sides of a chemical equation. They do not participate in the actual chemical reaction but are present to maintain charge balance.
05

Connect Conjugate Bases to Spectator Ions

Since the conjugate base of a strong acid is weak and does not participate in further reactions, they often fulfill the role of spectator ions in solution. For example, the Cl鈦� ion from HCl dissociation remains unchanged in a chemical equation and balances the charge, acting as a spectator ion.

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Key Concepts

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

Strong Acid
To understand strong acids, it is essential to know that these acids fully dissociate in water. Dissociation means they release all of their hydrogen ions ( H鈦� ) into the solution. This characteristic makes them potent acid contributors. Examples of strong acids include hydrochloric acid ( HCl ), sulfuric acid ( H鈧係O鈧� ), and nitric acid ( HNO鈧� ). When strong acids dissociate, they are left with their conjugate bases.
  • Complete Dissociation: Strong acids fully separate into ions in aqueous solutions.
  • Examples: Hydrochloric acid, sulfuric acid, nitric acid.
  • Strong Acid Behavior: Their behavior contrasts with weak acids, which only partially dissociate.
Recognizing how strong acids dissociate helps grasp why their conjugate bases have specific roles in chemical reactions.
Spectator Ion
Spectator ions are intriguing because they seem indifferent to the ongoing chemical reactions. They remain unchanged and appear on both sides of the chemical equation. Spectator ions play a vital role by maintaining the charge balance during reactions, even though they do not actually participate. They are important for understanding the full context of a reaction.
  • Unchanged Role: Present in both reactants and products.
  • Charge Balance: Crucial in keeping the ionic balance intact.
  • Example: Chloride ions ( Cl鈦� ) typically act as spectators in reactions involving strong acids.
This characteristic of spectator ions helps differentiate them from other participants in chemical equations.
Dissociation
Dissociation is a fundamental concept, especially when discussing acids such as strong acids. Dissociation refers to the process where a compound splits into separate ions. For strong acids, this occurs entirely in water, meaning the acid releases all its hydrogen ions. This action results in distinct ions, which are essentially the building blocks for understanding acid-base chemistry.
  • Complete for Strong Acids: Strong acids dissociate completely.
  • Conjugate Base Formation: The leftover part after releasing H鈦� becomes the conjugate base.
  • Illustrative Example: When HCl ionizes, it yields H鈦� and Cl鈦� ions.
Comprehensive understanding of dissociation is crucial for predicting the behavior of acids in solutions.
Chemical Reaction
Chemical reactions involve the transformation of reactants into products. In acid-base reactions, dissociation plays a pivotal role. While reactants undergo changes, spectator ions ensure the charge balance by staying constant throughout the reaction. This means even if they don't participate directly, they ensure the reaction's completion without imbalance.
  • Transformation Process: Involves reactants turning into products.
  • Role of Spectator Ions: Keep charge balanced without participating in the reaction.
  • Importance of Reaction Dynamics: Understanding who participates and who spectates helps in grasping the reaction mechanism.
Recognizing the underlying dynamics of chemical reactions helps in fully understanding acid-base interactions.

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Most popular questions from this chapter

Determine the hydrogen ion or hydroxide ion concentration in each of the following solutions, as appropriate. (a) a solution in which \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=4.5 \times 10^{-4} M\) (b) a solution in which \(\left[\mathrm{OH}^{-}\right]=8.33 \times 10^{-5} \mathrm{M}\)

Define \(\mathrm{pH}\) and explain why \(\mathrm{pH},\) rather than molarity, is used as a concentration measure of \(\mathrm{H}_{3} \mathrm{O}^{+}\).

In acidic solvents, such as concentrated acetic acid, some of the acids considered strong (in water) behave as weak acids. Explain why \(\mathrm{HCl}\) behaves as a weak acid and \(\mathrm{HClO}_{4}\) behaves as a strong acid in acetic acid solvent.

A solution is made by dissolving \(15.0 \mathrm{~g}\) sodium hydroxide in approximately \(450 \mathrm{~mL}\) water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to \(500.0 \mathrm{~mL}\) of solution. (a) Calculate the \(\mathrm{pH}\) and \(\mathrm{pOH}\) in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly \(450 \mathrm{~g}\) and the temperature of the water increased by \(8.865^{\circ} \mathrm{C}\), how much heat was given off by the dissolution of \(15.0 \mathrm{~g}\) of solute? Assume the specific heat of the solution is \(4.184 \mathrm{~J} / \mathrm{g} \cdot \mathrm{K}\). What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, \(\left.\Delta H_{\mathrm{sol}}\right) ?\)

State whether each of the following reactions is an acidbase reaction, according to the definitions of Arrhenius, Br酶nsted-Lowry, and Lewis. (a) \(\mathrm{HCl}(\mathrm{aq})+\mathrm{NH}_{3}(\mathrm{aq}) \rightarrow \mathrm{NH}_{4} \mathrm{Cl}(\mathrm{aq})\) (b) \(\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{NaOH}(\mathrm{s}) \rightarrow \mathrm{NaHSO}_{3}(\mathrm{~s})\)
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