Question

Write the balanced formula equation for the acid–base reactions that occur when the following are mixed. a. potassium hydroxide (aqueous) and nitric acid b. barium hydroxide (aqueous) and hydrochloric acid c. perchloric acid \(\left[\mathrm{HClO}_{4}(a q)\right]\) and solid iron(III) hydroxide d. solid silver hydroxide and hydrobromic acid e. aqueous strontium hydroxide and hydroiodic acid

Short answer

a. \(KOH (aq) + HNO_3 (aq) \rightarrow H_2O (l) + KNO_3 (aq)\) b. \(Ba(OH)_2 (aq) + 2 HCl (aq) \rightarrow 2 H_2O (l) + BaCl_2 (aq)\) c. \(3 HClO_4 (aq) + Fe(OH)_3 (s) \rightarrow 3 H_2O (l) + Fe(ClO_4)_3 (aq)\) d. \(AgOH (s) + HBr (aq) \rightarrow H_2O (l) + AgBr (s)\) e. \(Sr(OH)_2 (aq) + 2 HI (aq) \rightarrow 2 H_2O (l) + SrI_2 (aq)\)

Step-by-step solution

Write the chemical formulas

The chemical formulas for the given compounds are: - Potassium Hydroxide (KOH) - Nitric Acid (HNO₃)

Determine the products

In this acid-base reaction, the products are water (H₂O) and potassium nitrate (KNO₃).

Balance the equation

The balanced equation for this reaction is: KOH (aq) + HNO₃ (aq) -> H₂O (l) + KNO₃ (aq) b. Barium hydroxide (aqueous) and hydrochloric acid

Write the chemical formulas

The chemical formulas for the given compounds are: - Barium Hydroxide (Ba(OH)₂) - Hydrochloric Acid (HCl)

Determine the products

In this acid-base reaction, the products are water (H₂O) and barium chloride (BaCl₂).

Balance the equation

The balanced equation for this reaction is: Ba(OH)₂ (aq) + 2 HCl (aq) -> 2 H₂O (l) + BaCl₂ (aq) c. Perchloric acid [HClO₄(aq)] and solid iron(III) hydroxide

Write the chemical formulas

The chemical formulas for the given compounds are: - Perchloric Acid (HClO₄) - Iron(III) Hydroxide (Fe(OH)₃)

Determine the products

In this acid-base reaction, the products are water (H₂O) and iron(III) perchlorate (Fe(ClO₄)₃).

Balance the equation

The balanced equation for this reaction is: 3 HClO₄ (aq) + Fe(OH)₃ (s) -> 3 H₂O (l) + Fe(ClO₄)₃ (aq) d. Solid silver hydroxide and hydrobromic acid

Write the chemical formulas

The chemical formulas for the given compounds are: - Silver Hydroxide (AgOH) - Hydrobromic Acid (HBr)

Determine the products

In this acid-base reaction, the products are water (H₂O) and silver bromide (AgBr).

Balance the equation

The balanced equation for this reaction is: AgOH (s) + HBr (aq) -> H₂O (l) + AgBr (s) e. Aqueous strontium hydroxide and hydroiodic acid

Write the chemical formulas

The chemical formulas for the given compounds are: - Strontium Hydroxide (Sr(OH)₂) - Hydroiodic Acid (HI)

Determine the products

In this acid-base reaction, the products are water (H₂O) and strontium iodide (SrI₂).

Balance the equation

The balanced equation for this reaction is: Sr(OH)₂ (aq) + 2 HI (aq) -> 2 H₂O (l) + SrI₂ (aq)

Key concepts

Chemical Equations

Chemical equations are representations of chemical reactions, showing the reactants and products with their respective chemical formulas. These equations provide a clear view of what happens during a chemical reaction. In the context of acid-base reactions, chemical equations help to visualize how acids and bases neutralize each other to form water and a salt. For example, when potassium hydroxide (KOH) reacts with nitric acid (HNO₃), they form water (H₂O) and potassium nitrate (KNO₃).
Writing chemical equations involves listing the chemical formulas of the reactants on the left side and the products on the right side, separated by an arrow indicating the direction of the reaction. It is essential to represent each substance accurately to ensure clarity.

• Reactants are the starting substances that undergo change in the reaction.
• Products are the substances produced as a result of the reaction.

Understanding chemical equations is foundational for predicting the outcome of chemical reactions and for learning how different substances interact at a molecular level.

Balancing Equations

Balancing chemical equations is a crucial skill in chemistry to ensure that the law of conservation of mass is obeyed. This law states that mass cannot be created or destroyed in a chemical reaction, meaning that the mass of the reactants must equal the mass of the products. Each element must have the same number of atoms on both sides of the equation.
To balance equations, we adjust coefficients—numbers placed before the chemical formulas—rather than altering the formulas themselves. For instance, in the reaction between barium hydroxide and hydrochloric acid:

1. Start by writing the unbalanced equation: Ba(OH)₂ + HCl -> H₂O + BaCl₂.
2. Identify the elements that are not balanced; here, H and Cl need attention.
3. Balance the hydrogen and chlorine atoms by adding a coefficient of 2 in front of HCl and H₂O: Ba(OH)₂ + 2 HCl -> 2 H₂O + BaCl₂. Now each side of the equation has 2 H and 2 Cl atoms.

Balancing equations require practice but grows easier as you become more familiar with the process. Always double-check to confirm that each element is balanced.

Acid-Base Chemistry

Acid-base chemistry is the study of the reactions between acids and bases, which are integral to many chemical processes. Acids are substances that release hydrogen ions (H⁺) in solution, while bases produce hydroxide ions (OH⁻). The interaction between an acid and a base is known as a neutralization reaction, leading to the formation of water and a salt.
Neutralization reactions are a key concept in acid-base chemistry. When an acid and a base react, the H⁺ from the acid combines with the OH⁻ from the base to form water (H₂O), a neutral molecule.

• Example: In the reaction between aqueous strontium hydroxide and hydroiodic acid, the products are water and strontium iodide: Sr(OH)₂ (aq) + 2 HI (aq) -> 2 H₂O (l) + SrI₂ (aq).
• Similarly, when solid silver hydroxide reacts with hydrobromic acid, we get water and silver bromide as products: AgOH (s) + HBr (aq) -> H₂O (l) + AgBr (s).

These reactions are predictable: acids neutralize bases to produce water and salt, making acid-base chemistry essential for understanding reactions in various natural and industrial processes.