What is an Acid-Base Reaction?

An acid-base reaction is a chemical reaction that occurs between an acid and a base, which are the reactants. The products of this reaction are salt and water. An acid-base reaction is a double-replacement reaction where ions exchange their positions. This type of reaction is essential in both biochemistry and industrial chemistry ^[1,2].

General Equation

The general equation of an acid base reaction is as follows.

Acid + Base → Salt + Water

Strong Acids and Bases

A strong acid is one that readily gives off hydronium (H⁺) ions when dissolved in water (H₂O). A strong base is one that quickly gives off hydroxyl (OH^–) ions when dissolved in water. The H⁺ and OH^– combine to form H₂O. Strong acid and base react wholly and together, neutralize each other. Hence, sometimes, this reaction is called a neutralization reaction.

How to Identify the Acid and Base in a Reaction

To determine whether a substance is an acid or base, count the hydrogens before and after the reaction. If the number of hydrogens has decreased, that substance is the acid because it donates hydrogen ions. If the number of hydrogens has increased, that substance is the base since it accepts hydrogen ions.

Predicting Products of Acid-Base Reactions

In most acid-base reactions, there will always be water and the salts. For example, hydrochloric acid (HCl) reacts with sodium hydroxide (NaOH) to form sodium chloride (NaCl) salt and water (H₂O).

HCl (aq.) + NaOH (aq.) → NaCl (aq.) + H₂O (l)

Balancing Acid-Base Reactions

To balance a reaction, we must make sure that there is an equal number of atoms of a particular element on both sides of the equation. Consider the example of the reaction between phosphoric acid (H₃PO₄) and calcium hydroxide Ca(OH)₂ resulting in insoluble Ca₃(PO₄)₂ and water (H₂O).

H₃PO₄ (aq.) + Ca(OH)₂ (aq.) → Ca₃(PO₄)₂ (s/ppt.) + H₂O (l)

This equation is unbalanced. We need two phosphates (PO₄⁺) and three calcium (Ca⁺) ions on the left. So, we multiply the reactants accordingly and obtain:

2 H₃PO₄ (aq.) + 3 Ca(OH)₂ (aq.) → Ca₃(PO₄)₂ (s/ppt.) + H₂O (l)

No, we find that there are six O atoms in 3 Ca(OH)₂. So, we multiply H₂O by 6, thereby balancing both O and H.

2 H₃PO₄ (aq.) + 3 Ca(OH)₂ (aq.) → Ca₃(PO₄)₂ (s/ppt.) + 6 H₂O (l)

The chemical equation is now balanced.

Examples of Acid-Base Reaction

Most acid-base reactions take place between strong acids and bases, and hence, complete neutralization occurs. Below are some examples, along with the formula of the compounds ^[1-4].

• Sulfuric acid (H₂SO₄) and potassium hydroxide (KOH) react to form potassium sulfate (K₂SO₄) and water (H₂O).

H₂SO₄ (aq.) + 2 KOH (aq.) → K₂SO₄ (aq.) + 2 H₂O (l)

• Ammonia (NH₃) dissolves in hydrofluoric acid (HF) to form ammonium salt (NH₄^–) and fluoride (F^–).

HF (aq.) + NH₃ (aq.) → NH₄⁺ (aq.) + F^– (aq.)

• Hydrogen bromide (HBr) reacts with magnesium hydroxide (Mg(OH)₂), and the products are magnesium bromide (MgBr₂) and water (H₂O).

Mg(OH)₂ (aq.) + 2 HBr (aq.) → MgBr₂ (aq.) + 2 H₂O (l)

• Ammonia (NH₃) and hydrogen sulfate (H₂SO₄) reacts to form ammonium sulfate ((NH4)₂SO₄) salt.

H₂SO₄ (aq.) + 2 NH₃ (aq.) → (NH₄)₂SO₄ (aq.)

Acid-Base Reactions in Organic Chemistry

Acid-base reactions are also observed in organic chemistry. According to Brønsted-Lowry theory, a compound that donates a proton is an acid, and a compound that accepts a proton is a base ^[5,6].

Example

• Methanol (CH₃OH) reacts with sodium hydride (NaH), producing the sodium salt of methanol (CH₃O^–Na⁺) and hydrogen gas (H₂).

CH₃OH (aq.) + NaH (aq.) → CH₃O^–Na⁺ (aq.) + H₂ (g)

Reaction Between Weak Acid and Weak Base

When a weak acid reacts with an equivalent amount of a weak base, complete neutralization does not occur. The concentrations of the species in equilibrium with each other will depend on the equilibrium constant, K, for the reaction. The general equation can be represented as:

AH + B ⇌ A^– +BH⁺

Example

• Acetic acid (CH₃COOH) gives off proton (H⁺) atom to water (H₂O), resulting in acetate (CH₃COO^–) ion and hydronium (H₃O⁺).

CH₃COOH (aq.) + H₂O (l) ⇌ CH₃COO^– (aq.) + H₃O⁺ (aq.)

Uses of Acid-Base Reactions in Daily Life

Acid-base reactions are significant in everyday life.

• Calcium oxide (CaO) is used to neutralize acidic soil.
• Hydrochloric acid (HCl) in the stomach plays a vital role in digesting food. Antacids, which are bases, are taken to neutralize excess stomach acid, to prevent damage to the intestines.
• Alkaline calcium hydroxide (limewater) is used to absorb harmful acidic sulfur dioxide (SO₂) gas that is released from power stations and the burning of fossil fuels.

FAQs

References

1. Chem.libretexts.org
2. Pressbooks.bccampus.ca
3. Chem.libretexts.org
4. Public.asu.edu
5. Research.cm.utexas.edu
6. Leah4sci.com