Question

Write ionization equations and ionization constant expressions for these acids and bases. (a) \(\mathrm{CH}_{3} \mathrm{COOH}\) (b) \(\mathrm{HCN}\) (c) \(\mathrm{SO}_{3}^{2-}\) (d) \(\mathrm{PO}_{4}^{3-}\) (e) \(\mathrm{NH}_{4}^{+}\) (f) \(\mathrm{H}_{2} \mathrm{SO}_{4}\)

Short answer

Ionization steps written for each substance. Constants: (a) \( K_a \), (b) \( K_a \), (c) \( K_b \), (d) \( K_b \), (e) \( K_a \), (f) \( K_{a2} \).

Step-by-step solution

Analyzing Acetic Acid Ionization

Identify the ionization process for acetic acid \( \text{CH}_3\text{COOH} \). It ionizes as:\[ \text{CH}_3\text{COOH} \rightleftharpoons \text{CH}_3\text{COO}^- + \text{H}^+ \]The ionization constant expression (\( K_a \)) is:\[ K_a = \frac{[\text{CH}_3\text{COO}^-][\text{H}^+]}{[\text{CH}_3\text{COOH}]} \]

Analyzing Hydrocyanic Acid Ionization

Identify the ionization process for hydrocyanic acid \( \text{HCN} \). It ionizes as:\[ \text{HCN} \rightleftharpoons \text{H}^+ + \text{CN}^- \]The ionization constant expression (\( K_a \)) is:\[ K_a = \frac{[\text{H}^+][\text{CN}^-]}{[\text{HCN}]} \]

Analyzing Sulfite Ionization

Identify the ionization process for sulfite ion \( \text{SO}_3^{2-} \). It ionizes as it accepts protons:\[ \text{SO}_3^{2-} + \text{H}_2\text{O} \rightleftharpoons \text{HSO}_3^- + \text{OH}^- \]The ionization constant expression (\( K_b \)) is:\[ K_b = \frac{[\text{HSO}_3^-][\text{OH}^-]}{[\text{SO}_3^{2-}]} \]

Analyzing Phosphate Ionization

Identify the ionization process for phosphate ion \( \text{PO}_4^{3-} \). It can accept protons:\[ \text{PO}_4^{3-} + \text{H}_2\text{O} \rightleftharpoons \text{HPO}_4^{2-} + \text{OH}^- \]The ionization constant expression (\( K_b \)) is:\[ K_b = \frac{[\text{HPO}_4^{2-}][\text{OH}^-]}{[\text{PO}_4^{3-}]} \]

Analyzing Ammonium Ion Ionization

Identify the ionization process for ammonium ion \( \text{NH}_4^+ \). It ionizes by:\[ \text{NH}_4^+ \rightleftharpoons \text{NH}_3 + \text{H}^+ \]The ionization constant expression (\( K_a \)) is:\[ K_a = \frac{[\text{NH}_3][\text{H}^+]}{[\text{NH}_4^+]} \]

Analyzing Sulfuric Acid Ionization

Identify the ionization process for sulfuric acid \( \text{H}_2\text{SO}_4 \). It ionizes in two steps:First ionization:\[ \text{H}_2\text{SO}_4 \rightarrow \text{HSO}_4^- + \text{H}^+ \]Second ionization (in weaker form): \[ \text{HSO}_4^- \rightleftharpoons \text{SO}_4^{2-} + \text{H}^+ \]The ionization constant expression for the second ionization (\( K_{a2} \)) is:\[ K_{a2} = \frac{[\text{SO}_4^{2-}][\text{H}^+]}{[\text{HSO}_4^-]} \]

Key concepts

Acid-Base Chemistry

Acid-base chemistry is a fundamental part of understanding chemical reactions because it involves the transfer of protons (H⁺ ions) between substances.
Acids are defined as substances that donate protons, while bases accept protons.
In water, acids increase the concentration of H⁺ ions, leading the solution to become acidic, whereas bases increase the concentration of OH⁻ ions, which makes the solution basic.

• Common examples: Hydrochloric acid (HCl) is a strong acid, while sodium hydroxide (NaOH) is a strong base.
• Indicators: Litmus paper or phenolphthalein are often used to identify acidic or basic solutions visually.

The process of acids and bases interacting in a solution often reaches a state of equilibrium where the rate of the forward reaction equals the rate of the reverse reaction.

Ionization Constants

Ionization constants are pivotal in acid-base chemistry because they quantify the strength of an acid or base in solution.
The equilibrium constant, known as the acid dissociation constant (Ka) for acids, helps predict the extent of ionization.
For bases, the analogous constant is the base dissociation constant (Kb).

• Acid Example: Acetic acid ( \( ext{CH}_3 ext{COOH} \)) has a specified Ka, showing how much it ionizes in water.
• Base Example: Ammonia ( \( ext{NH}_3 \)) has a known Kb value, indicating its basic nature and ionization level.

Understanding ionization constants allows chemists to predict - and calculate - the pH of solutions, determine the position of equilibrium, and estimate the degree of ionization.

Chemical Equilibrium

In chemical reactions, equilibrium refers to the condition where the forward and reverse reaction rates are equal, resulting in no net change in the concentrations of reactants and products.
This is crucial in acid-base reactions, particularly for weak acids and bases that do not fully ionize in solution.

• Dynamic Nature: Even though the concentrations remain constant, the reactions continue to occur at a molecular level.
• Le Chatelier's Principle: If an equilibrium system is subjected to a change in conditions, the system will adjust itself to partially counteract the change.

By understanding equilibrium, students can better grasp how solutions behave when concentrations, temperatures, or pressures are altered.

Proton Transfer

Proton transfer is the fundamental process in acid-base reactions where a proton (H⁺) is transferred from an acid to a base.
It forms the crux of the Bronsted-Lowry acid-base theory.

• An acid donates a proton to become its conjugate base.
• A base accepts a proton to form its conjugate acid.

For example, when acetic acid ( \( ext{CH}_3 ext{COOH} \)) donates a proton, it forms acetate ( \( ext{CH}_3 ext{COO}^- \)). Understanding this concept is key to interpreting many chemical reactions, buffer solutions, and determining reaction directions.

Acid Ionization

Acid ionization describes how acids release protons into a solution, creating H⁺ ions and their corresponding anions, which is essential for determining an acid's strength.
For instance, strong acids like sulfuric acid ( \( ext{H}_2 ext{SO}_4 \)) ionize completely in solution, liberating numerous H⁺ ions compared to weak acids like acetic acid, which only partially ionize.

• The ionization process affects the conductivity of the solution.
• The extent of ionization can be quantified using the acid dissociation constant ( \( K_a \)).

By grasping how acids ionize, students can predict their behavior in reactions, understand concentration effects, and relate it to pH levels in solution.

Base Ionization

Base ionization is the process by which a base accepts protons in a solution, typically resulting in the formation of hydroxide ions (OH⁻).
This reaction is an indicator of a base's strength.

• Bases like ammonia ( \( ext{NH}_3 \)) interact with water to produce ammonia ions ( \( ext{NH}_4^+ \)) and hydroxide ions leading to a basic solution.
• The extent of base ionization is described by the equilibrium constant known as \( K_b \).

Understanding base ionization helps students predict the consequent pH of solutions and the neutralization potential when these solutions interact with acids.