Question

When chloric acid reacts with water, it reacts as a strong acid. Write an equation for this reaction.

Short answer

The equation for the reaction of chloric acid with water is \[\text{HClO}_3 (aq) + \text{H}_2\text{O} (l) \rightarrow \text{H}_3\text{O}^+ (aq) + \text{ClO}_3^- (aq)\].

Step-by-step solution

Identify the reactants

The first step in writing a reaction equation is to identify the reactants. In this case, the reactants are chloric acid (HClO3) and water (H2O).

Determine the products

Chloric acid is a strong acid and will completely dissociate in water to form hydronium ions (H3O+) and chlorate ions (ClO3-).

Write the balanced chemical equation

Now, write the chemical equation with the reactants on the left and the products on the right, ensuring the equation is balanced. For chloric acid reacting with water, the balanced equation is: \[\text{HClO}_3 (aq) + \text{H}_2\text{O} (l) \rightarrow \text{H}_3\text{O}^+ (aq) + \text{ClO}_3^- (aq)\]. This shows that each mole of chloric acid yields one mole of hydronium ions and one mole of chlorate ions when dissolved in water.

Key concepts

Understanding Acid-Base Reactions

When exploring the fascinating world of chemistry, one fundamental concept is the acid-base reaction. These reactions are processes in which an acid and a base interact, typically resulting in the formation of water and a salt. Most notably, an important subclass of these reactions is when acids donate protons (H+) to water, forming hydronium ions (H3O+).

This transfer of protons is the cornerstone of a common phenomenon we notice in aqueous solutions, such as the chloric acid and water reaction from the textbook exercise. Acid-base reactions are not limited to only strong acids and bases; they also include weak acids and bases that only partially dissociate in solution. Understanding how these reactions occur allows students to predict the products and write balanced chemical equations effectively.

The Nature of Chloric Acid

Chloric acid, with the chemical formula HClO3, is an example of an oxyacid where incorporation of oxygen into its structure affects its acidic strength. As mentioned in the exercise, chloric acid is a strong acid, which implies that it completely dissociates in water to release all of its hydrogen ions.

Being a strong acid makes chloric acid a considerable player in acid-base chemistry. When it reacts with water, it contributes significantly to the acidity of the solution by forming hydronium ions (H3O+), which then can partake in further chemical reactions. In the broader context, strong acids like chloric acid are commonly used in various chemical processes, including the purification of substances and in the manufacturing of fertilizers.

Dissociation of Acids in Water

Dissociation is the general process where molecules or ionic compounds separate or split into smaller particles such as atoms, ions, or radicals, usually in a reversible manner. When it comes to acids, dissociation refers specifically to the release of hydrogen ions (H+) into the solution.

In the context of our textbook example, chloric acid (HClO3) dissociates completely in water to form hydronium ions (H3O+) and chlorate ions (ClO3-). The complete dissociation characterizes chloric acid as a strong acid. We use the arrow in the chemical equation to show the directionality of the reaction, pointing towards the products, indicating complete dissociation. It's crucial for students to understand this concept to predict the behavior of acids in solution.

Balancing Chemical Equations

The skill of balancing chemical equations is a fundamental part of understanding chemical reactions. It requires that the number of atoms of each element is the same on both sides of the equation, reflecting the law of conservation of mass.

In our exercise example, the balanced equation for the reaction of chloric acid with water is presented as: \[\text{HClO}_3 (aq) + \text{H}_2\text{O} (l) \rightarrow \text{H}_3\text{O}^+ (aq) + \text{ClO}_3^- (aq)\].Here, we ensure that the number of each type of atom on the reactant side equals the number on the product side. For instance, there's one chlorine (Cl), three oxygens (O), and four hydrogens (H) in both reactants and products. Mastering balancing will enable students to write correct chemical formulas and understand reaction stoichiometry, which is crucial for quantitative aspects of chemistry.