Write balanced equations for the following reactions: (a)...

Write balanced equations for the following reactions:
(a) sulfur dioxide with water, (b) lithium oxide in water, $(\mathbf{c})$ zinc oxide with dilute hydrochloric acid,
(d) arsenic trioxide with aqueous potassium hydroxide.

Key Concepts

Amphoteric Behavior

Some oxides, such as arsenic trioxide, are amphoteric, meaning they can react with both acids and bases. In reactions with bases, such amphoteric compounds form salts that reflect their dual acidic and basic character. This property is important for understanding the diverse reactivity of compounds like arsenic trioxide in different chemical environments.

Reactions of Oxides with Water

Many non-metal and metal oxides react with water to form acidic or basic solutions. In these reactions, non-metal oxides typically form acids (as in the case of sulfur dioxide forming sulfurous acid), while metal oxides can form bases (like lithium oxide forming lithium hydroxide), illustrating the different properties and behaviors of oxides in aqueous environments.

Acid-Base Reactions

Acid-base reactions refer to processes where acids and bases interact to yield salts and water, often involving the transfer of protons. These reactions are vital in inorganic chemistry and help explain how oxides react with water or acids to form hydroxides or chloride salts, respectively.

Balancing Chemical Equations

This concept involves adjusting the coefficients of reactants and products in a chemical reaction so that the number of atoms for each element is the same on both sides of the equation. It is grounded in the law of conservation of mass and is essential for accurately representing the chemical processes at the molecular level.

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