Chapter 16: Problem 37
Why are ionizations of strong acids and strong bases generally not treated as equilibria?
Short Answer
Expert verified
Ionizations of strong acids and bases are complete, with no significant reverse reaction, so they don't establish equilibria.
Step by step solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Chemical Equilibrium
Chemical equilibrium is a state in a chemical reaction where the concentrations of reactants and products reach a constant balance. This happens when the rates of the forward and reverse reactions are equal. At equilibrium, chemical reactions continue to occur, but the net concentrations do not change. In other words, there is a dynamic balance, even though it might appear static from a broad perspective. Usually, this state is significant in reactions where both molecules and ions coexist in measurable amounts in the solution.
Equilibrium commonly applies to reactions involving weak acids and bases. Here, both the forward and reverse processes are noticeable. This is why, in the case of weak acids and bases, even if dissociation takes place, the formation of reactants from products (reverse reaction) is considerable. This ongoing conversion results in an equilibrium state, achieving a stable, yet dynamic, balance between reactants and products.
Equilibrium commonly applies to reactions involving weak acids and bases. Here, both the forward and reverse processes are noticeable. This is why, in the case of weak acids and bases, even if dissociation takes place, the formation of reactants from products (reverse reaction) is considerable. This ongoing conversion results in an equilibrium state, achieving a stable, yet dynamic, balance between reactants and products.
Dissociation
Dissociation is the process by which molecules, usually acids or bases, split into smaller particles such as ions when dissolved in a solvent like water. For strong acids and bases, this process results in complete dissociation. That means, when a strong acid such as hydrochloric acid (HCl) or a strong base like sodium hydroxide (NaOH) is dissolved in water, it breaks down entirely to form ions.
In the case of HCl, it dissociates fully into hydrogen ions \( H^+ \) and chloride ions \( Cl^- \). Similarly, NaOH breaks up into sodium ions \( Na^+ \) and hydroxide ions \( OH^- \). This complete dissociation explains why there are virtually no undissociated molecules left in the solution. Consequently, the concentration of ions significantly outweighs the presence of the original acid or base molecules. This total dissociation is vital for the ions' reactivity in chemical processes, particularly in strong acid and base reactions.
In the case of HCl, it dissociates fully into hydrogen ions \( H^+ \) and chloride ions \( Cl^- \). Similarly, NaOH breaks up into sodium ions \( Na^+ \) and hydroxide ions \( OH^- \). This complete dissociation explains why there are virtually no undissociated molecules left in the solution. Consequently, the concentration of ions significantly outweighs the presence of the original acid or base molecules. This total dissociation is vital for the ions' reactivity in chemical processes, particularly in strong acid and base reactions.
Ionization
Ionization is a key process in chemistry where an atom or a molecule acquires a negative or positive charge by gaining or losing electrons. This process is essential in forming ions from neutral molecules. Ionization takes place when acids and bases are dissolved in water, causing them to form ions. This process appears prominently and straightforwardly in the context of strong acids and bases.
Consider a strong acid such as sulfuric acid (\( H_2SO_4 \)), which ionizes completely in water producing hydrogen ions (\( H^+ \)) and sulfate ions (\( SO_4^{2-} \)). With weak acids and bases, partial ionization calls for equilibrium considerations, as the molecules do not convert entirely into ions, resulting in a measurable amount of undissociated molecules. However, in strong acids and bases, ionization leads almost exclusively to ion formation, leaving negligible undissociated molecules. As such, this ionization aspect significantly contributes to their high reactivity and conductivity in solutions.
Consider a strong acid such as sulfuric acid (\( H_2SO_4 \)), which ionizes completely in water producing hydrogen ions (\( H^+ \)) and sulfate ions (\( SO_4^{2-} \)). With weak acids and bases, partial ionization calls for equilibrium considerations, as the molecules do not convert entirely into ions, resulting in a measurable amount of undissociated molecules. However, in strong acids and bases, ionization leads almost exclusively to ion formation, leaving negligible undissociated molecules. As such, this ionization aspect significantly contributes to their high reactivity and conductivity in solutions.
Chemical Reactions
Chemical reactions involve the transformation of substances, where reactants convert into products through breaking and forming bonds. These reactions can be either reversible or irreversible. Understanding the nature of these reactions is crucial when discussing strong acids and bases. For strong acids and bases, the reactions are effectively irreversible in aqueous solutions.
Because strong acids and bases dissociate fully, the reaction proceeds in one predominant direction—the formation of ions. There's little to no significant reverse reaction. This is in contrast to reactions involving weak acids and bases, where the reactions can go forwards and backwards, contributing to an equilibrium state. Therefore, the nature of these chemical reactions is what sets the stage for whether or not equilibrium can be achieved. In the case of strong acids and bases, the one-sided nature of their reactions offers an excellent insight into why these substances often bypass the concept of equilibrium in solution.
Because strong acids and bases dissociate fully, the reaction proceeds in one predominant direction—the formation of ions. There's little to no significant reverse reaction. This is in contrast to reactions involving weak acids and bases, where the reactions can go forwards and backwards, contributing to an equilibrium state. Therefore, the nature of these chemical reactions is what sets the stage for whether or not equilibrium can be achieved. In the case of strong acids and bases, the one-sided nature of their reactions offers an excellent insight into why these substances often bypass the concept of equilibrium in solution.
