Question

The same net ionic process takes place when any strong acid reacts with any strong base. Write the equation for that process.

Short answer

The net ionic equation for the reaction between any strong acid and any strong base is: \( H^+ (aq) + OH^- (aq) \rightarrow H_2O (l) \)

Step-by-step solution

Identify the ions present in strong acids and strong bases

Strong acids dissociate completely in water to produce hydrogen ions (H+), while strong bases dissociate completely in water to produce hydroxide ions (OH-).

Write the molecular equation for the reaction between a strong acid and a strong base

A strong acid (HA) will react with a strong base (BOH) to produce water (H₂O) and a salt (BA) as products. The molecular equation for the reaction can be represented as: \( HA (aq) + BOH (aq) \rightarrow H_2O (l) + BA (aq) \) Here, "aq" indicates that the species are dissolved in water and "l" indicates that water is a liquid.

Write the total ionic equation

As strong acids and strong bases completely dissociate in water, we can rewrite the molecular equation as a total ionic equation, showing all the ions present in the solution: \( H^+ (aq) + A^- (aq) + B^+ (aq) + OH^- (aq) \rightarrow H_2O (l) + B^+ (aq) + A^- (aq) \)

Write the net ionic equation

In the net ionic equation, we only show the species that are transformed in the reaction. In this case, the hydrogen ions (H+) react with the hydroxide ions (OH-) to produce water (H₂O). The spectator ions (A⁻ and B⁺) do not participate in the reaction and can be removed from the equation. The net ionic equation is: \( H^+ (aq) + OH^- (aq) \rightarrow H_2O (l) \) This equation represents the net ionic process that occurs when any strong acid reacts with any strong base.

Key concepts

Strong Acids

Strong acids are fascinating and quite reactive substances in chemistry. Their defining feature is the ability to completely dissociate in water. What this means is that when you have a strong acid, such as hydrochloric acid (HCl), it will break down entirely into its constituent ions when dissolved in water.
This results in a large concentration of hydrogen ions (H⁺), making the solution strongly acidic. Some common examples are:

• Hydrochloric acid (HCl)
• Sulfuric acid (H₂SO₄)
• Nitric acid (HNO₃)

Because strong acids dissociate completely, none of the original acid molecules are left in the solution. This complete dissociation is why they are referred to as 'strong' acids. These acids play crucial roles in many chemical reactions, often acting as a catalyst or a primary reactant in ionic reactions.

Strong Bases

Strong bases are similar to strong acids in that they dissociate completely in water. However, instead of producing hydrogen ions like strong acids, they produce hydroxide ions (OH⁻), which make the solution basic. As a result, solutions of strong bases have a high pH.
Examples of strong bases include:

• Sodium hydroxide (NaOH)
• Potassium hydroxide (KOH)
• Calcium hydroxide (Ca(OH)₂)

The high concentration of hydroxide ions in solutions of strong bases allows them to effectively neutralize acids. This is why when a strong base reacts with a strong acid, they produce water, a much less reactive compound.

Ionic Reactions

Ionic reactions, such as the reaction between a strong acid and a strong base, involve the exchange of ions in an aqueous solution. These reactions are particularly important in chemistry because they are widespread and often involve highly reactive participants.
The beauty of ionic reactions lies in their simplicity and elegance. When we look at the ionic reaction between a strong acid (HA) and a strong base (BOH), we can focus on the ions involved. Upon dissociation, the acid provides hydrogen ions (H⁺) and the base provides hydroxide ions (OH⁻).
During the reaction, these two ions combine to form water (H₂O), simplifying the net ionic equation to:
\[ H^+ (aq) + OH^- (aq) \rightarrow H_2O (l) \]
By considering only the ions that undergo transformation, we arrive at the net ionic equation that captures the essence of the reaction. Such equations are helpful to students and chemists as they strip the reaction down to its core, showing the exact exchanges taking place.