Yes, copper hydroxide readily reacts with sulphuric acid in a classic neutralization reaction. This chemical interaction is fundamental in inorganic chemistry, producing a salt and water.
The Reaction Explained
The interaction between copper hydroxide, an alkaline base, and sulphuric acid, a strong acid, is a perfect example of an acid-base neutralization. During this process, the sulphuric acid neutralizes the copper hydroxide, resulting in the formation of copper sulfate (a salt) and water. This reaction is often exothermic, meaning it releases heat.
Chemical Equation
The balanced chemical equation for the reaction is:
$\text{Cu(OH)}_2\text{(s)} + \text{H}_2\text{SO}_4\text{(aq)} \rightarrow \text{CuSO}_4\text{(aq)} + 2\text{H}_2\text{O(l)}$
Where:
- $\text{Cu(OH)}_2$: Copper(II) Hydroxide (solid)
- $\text{H}_2\text{SO}_4$: Sulphuric Acid (aqueous solution)
- $\text{CuSO}_4$: Copper(II) Sulfate (aqueous solution)
- $\text{H}_2\text{O}$: Water (liquid)
Understanding the Reactants and Products
To better understand this reaction, let's examine the key components:
- Copper(II) Hydroxide ($\text{Cu(OH)}_2$): This is a light blue, gelatinous solid that is sparingly soluble in water. It acts as a base due to the presence of hydroxide ($\text{OH}^-$) ions. Learn more about Copper(II) Hydroxide.
- Sulphuric Acid ($\text{H}_2\text{SO}_4$): A strong, highly corrosive mineral acid. It is a diprotic acid, meaning it can donate two protons ($\text{H}^+$) per molecule, making it a powerful neutralizing agent. Find out more about Sulphuric Acid.
- Copper(II) Sulfate ($\text{CuSO}_4$): The salt formed during the reaction. It is typically encountered as a bright blue crystalline solid (pentahydrate form, $\text{CuSO}_4 \cdot 5\text{H}_2\text{O}$) and is highly soluble in water. It has various applications, from agriculture to electroplating. Explore Copper(II) Sulfate uses.
- Water ($\text{H}_2\text{O}$): The other product of the neutralization, formed from the combination of $\text{H}^+$ ions from the acid and $\text{OH}^-$ ions from the base.
Key Aspects of the Reaction
This neutralization reaction demonstrates several important chemical principles:
- Acid-Base Chemistry: It perfectly illustrates Brønsted-Lowry acid-base theory, where $\text{H}_2\text{SO}_4$ donates protons and $\text{Cu(OH)}_2$ accepts them.
- Salt Formation: The reaction produces a salt (copper sulfate) and water, which is characteristic of neutralization reactions between an acid and a metal hydroxide.
- Solubility Changes: The solid, sparingly soluble copper hydroxide transforms into the highly soluble copper sulfate in an aqueous solution.
Why This Reaction Matters
Understanding the reaction between copper hydroxide and sulphuric acid has practical implications across various fields.
Practical Applications
- Synthesis of Copper Salts: This reaction is a straightforward method for preparing copper(II) sulfate from copper hydroxide. Copper sulfate is widely used:
- As a fungicide and herbicide in agriculture.
- In the textile industry as a mordant.
- For electroplating and metal finishing.
- In school laboratories for demonstrating chemical principles.
- Waste Treatment: While not a primary method for treating copper waste due to the toxicity of copper ions, understanding such reactions is crucial in processes where metal hydroxides might be neutralized or dissolved.
- Chemical Manufacturing: It can be part of a larger process in chemical manufacturing where specific copper compounds are required.
Summary of Reaction Components
| Component | Chemical Formula | Role | State | Key Property |
|---|---|---|---|---|
| Copper Hydroxide | $\text{Cu(OH)}_2$ | Base (Reactant) | Solid | Alkaline, sparingly soluble, light blue |
| Sulphuric Acid | $\text{H}_2\text{SO}_4$ | Acid (Reactant) | Aq. | Strong acid, highly corrosive |
| Copper Sulfate | $\text{CuSO}_4$ | Salt (Product) | Aq. | Soluble, typically blue crystals, various uses |
| Water | $\text{H}_2\text{O}$ | Water (Product) | Liquid | Neutral, universal solvent |
This reaction highlights a fundamental chemical principle where an acid and a base combine to form a salt and water, playing a role in both industrial applications and educational chemistry.
