Problem 118 - Chemistry: An Atoms-Focused Approach

Question

Give the formulas of the acids formed in the following chemical reactions of chlorine oxides. a. \(\mathrm{ClO}+\mathrm{H}_{2} \mathrm{O} \rightarrow ?+?\) b. \(\mathrm{Cl}_{2} \mathrm{O}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{HCl}+?\) c. \(\mathrm{Cl}_{2} \mathrm{O}_{6}+\mathrm{H}_{2} \mathrm{O} \rightarrow ?+?\)

Step-by-Step Solution

Answer

A. ClO + H2O B. Cl2O + H2O C. Cl2O6 + H2O Answer: A. Hypochlorous acid (HClO) B. Hydrochloric acid (HCl) C. Chloric acid (HClO3)

Step 1: Reaction A: ClO + H2O -> ? + ?

In this reaction, ClO reacts with water (H2O). We will first balance the chemical equation: \(\mathrm{ClO} + \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{HClO} + \mathrm{OH}^{-}\) The balanced equation helps us to see that the acid formed in this reaction is HClO (hypochlorous acid).

Step 2: Reaction B: Cl2O + H2O -> HCl + ?

In this reaction, Cl2O reacts with water (H2O). The equation for B is already partially complete. We just need to balance the equation and find the other product along with HCl: \(\mathrm{Cl}_{2} \mathrm{O} + \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{2HCl} + \mathrm{O}_{2}\) In Reaction B, the acid formed is HCl (hydrochloric acid).

Step 3: Reaction C: Cl2O6 + H2O -> ? + ?

In this reaction, Cl2O6 reacts with water (H2O). To determine the formulas of the acids formed, balance the chemical equation: \(\mathrm{Cl}_{2} \mathrm{O}_{6} + \mathrm{6H}_{2} \mathrm{O} \rightarrow \mathrm{2HClO}_{3} + \mathrm{3O}_{2}\) The balanced equation shows that the acid formed in this reaction is HClO3 (chloric acid). To summarize, the acids formed in the three reactions are: a. Hypochlorous acid (HClO) b. Hydrochloric acid (HCl) c. Chloric acid (HClO3)

Key Concepts

Chemical Reactions

Understanding chemical reactions is fundamental in chemistry. It involves substances, known as reactants, being transformed into different substances, known as products. In the case of chlorine oxides reacting with water, the reactants are chlorine oxides and water, while different acids are formed as products.
These reactions illustrate how different chlorine oxides interact with water to form acids. For example, when chlorine monoxide (\(\mathrm{ClO}\)) reacts with water, hypochlorous acid (\(\mathrm{HClO}\)) is formed along with hydroxide ions. Meanwhile, other reactions involving different chlorine oxides like \(\mathrm{Cl}_{2} \mathrm{O}\) and \(\mathrm{Cl}_{2} \mathrm{O}_{6}\) result in the formation of hydrochloric acid and chloric acid, respectively. These reactions are essential for studying the properties and behaviors of acids and bases.

Acid Formation

Acid formation in chemical reactions, especially those involving chlorine oxides, is a fascinating process. A common feature in these reactions is the reaction of chlorine oxides with water, leading to the formation of an acid. The acid's type depends on the specific chlorine oxide involved.

• For instance, when chlorine monoxide (\(\mathrm{ClO}\)) reacts with water, the resultant product is hypochlorous acid (\(\mathrm{HClO}\)), a weak acid.
• If dichlorine monoxide (\(\mathrm{Cl}_{2} \mathrm{O}\)) interacts with water, it produces hydrochloric acid (\(\mathrm{HCl}\)) which is a strong acid.
• Lastly, the reaction between dichlorine hexoxide (\(\mathrm{Cl}_{2} \mathrm{O}_{6}\)) and water forms chloric acid (\(\mathrm{HClO}_{3}\)), a moderately strong acid.

The variation in the strength and type of acids formed highlights the versatility and reactivity of chlorine oxides. Understanding these reactions is essential for appreciating the chemical properties and potential applications of acids.

Balancing Equations

Balancing chemical equations is a crucial skill in chemistry. It ensures that the laws of conservation of mass and charge are satisfied. In the context of the reactions between chlorine oxides and water, balancing the equations helps to accurately represent the formation of products.
To balance a chemical equation:

• Count and compare the number of atoms of each element in the reactants and products.
• Adjust coefficients to ensure that the same number of each type of atom appears on both sides.
• Check to confirm that all atoms and charges balance out evenly.

For example, in the reaction of \(\mathrm{Cl}_{2} \mathrm{O} + \mathrm{H}_{2} \mathrm{O}\rightarrow 2\mathrm{HCl} + \mathrm{O}_{2}\), you must ensure that two hydrogen, two chlorine, and a proper amount of oxygen atoms are present on both sides. Balancing equations not only helps in predicting the products accurately but also minimizes errors in laboratory experiments and theoretical calculations.