Question

Write the equation for the action of a dilute acid on a metal oxide.

Short answer

Answer: The balanced equation for the reaction between sulfuric acid and copper(II) oxide is H₂SO₄ (aq) + CuO (s) -> CuSO₄ (aq) + H₂O (l).

Step-by-step solution

Write down the general equation for the reaction of an acid with a metal oxide

Recall that the general reaction for the reaction of an acid with a metal oxide can be written as: Acid + Metal Oxide -> Salt + Water

Choose an example

We will choose a specific acid and metal oxide to write a balanced equation. Let's use sulfuric acid (H₂SO₄) and copper(II) oxide (CuO) as the reactants.

Write the equation in terms of the chosen reactants

Using the chosen reactants, write down the equation for the reaction between sulfuric acid and copper(II) oxide: H₂SO₄ (aq) + CuO (s) -> CuSO₄ (aq) + H₂O (l)

Balance the equation

Check that the equation is balanced in terms of atoms on both sides. In this case, it is already balanced: H₂SO₄ (aq) + CuO (s) -> CuSO₄ (aq) + H₂O (l) So, this balanced equation represents the reaction between a dilute acid (sulfuric acid) and a metal oxide (copper(II) oxide) to produce a salt (copper(II) sulfate) and water.

Key concepts

Balanced Chemical Equation

A balanced chemical equation is essential to accurately representing a chemical reaction. It shows how the reactants are transformed into products and specifies the number of atoms of each element involved. A reaction is balanced when the total number of each type of atom on the reactants' side is equal to the total number on the products' side.
For instance, in the given example: \( \text{H}_2\text{SO}_4 (aq) + \text{CuO} (s) \rightarrow \text{CuSO}_4 (aq) + \text{H}_2\text{O} (l) \), we must ensure that there are equal amounts of hydrogen, sulfur, oxygen, and copper atoms on both sides.
Maintaining a balanced equation is crucial because:

• It adheres to the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.
• It helps in quantitatively analyzing chemical reactions for laboratory and industrial applications.
• It ensures the correct stoichiometry, which is about the ratio between the amounts of reactants and products.

Metal Oxides

Metal oxides are compounds formed when a metal reacts with oxygen. They play a significant role in various chemical reactions, especially acid-base reactions where they usually act as bases. These do not only display fundamental chemical properties but are also widely used in industries.
Characteristics of metal oxides include:

• They are usually solid with high melting points.
• They can contain ions or covalent bonds, depending on the metal involved.
• In acid-base reactions, they react with acids to form salt and water as products.

In the context of our example reaction, copper(II) oxide is a metal oxide.

Sulfuric Acid Reactions

Sulfuric acid is a strong mineral acid, and its reactions are commonly encountered in both academic and industrial settings. It is often used in acid-base reactions, where it reacts with metal oxides to create salts and water.
Some key properties of sulfuric acid that make it remarkable are:

• It is a diprotic acid, which means it can donate two protons (hydrogen ions) per molecule in a reaction. In our equation, \( \text{H}_2\text{SO}_4 \), it donates two hydrogen ions.
• It is a highly corrosive and dense liquid, often used as a dehydrating or oxidizing agent.

When sulfuric acid reacts with copper(II) oxide, it forms copper(II) sulfate and water, illustrating a classic acid-base reaction.

Copper(II) Oxide Reactions

Copper(II) oxide, a black solid, plays a pivotal role as a reactant in the example given. It's known for readily reacting with acids, such as sulfuric acid, to form water and corresponding copper salts.
Some notable aspects of copper(II) oxide are:

• This metal oxide functions as a base, reacting with acids to form salts.
• Its reactivity serves not just in academic cases but also in industry settings, where it's employed to produce copper sulfate and other copper-based chemicals.
• The reaction with sulfuric acid specifically forms copper(II) sulfate, a compound used in agriculture and chemistry labs.

The reaction with sulfuric acid demonstrates copper(II) oxide's classic response as a basic metal oxide, ensuring water and salt as reaction products.