When calcium nitrate reacts with sulphuric acid, a chemical reaction occurs that produces calcium sulfate and nitric acid. This is a common type of double displacement reaction where the components of the two reacting compounds exchange places.
The Chemical Reaction Explained
Calcium nitrate (Ca(NO3)2) is known to be soluble in sulfuric acid (H2SO4), indicating that both are initially present in a dissolved state. Upon mixing, a reaction proceeds, leading to the formation of two new compounds.
Products of the Reaction
The specific products formed when calcium nitrate reacts with sulphuric acid are:
- Calcium Sulfate (CaSO4): This compound is typically a white solid. Unlike calcium nitrate, calcium sulfate has limited solubility in water, meaning it often precipitates out of the solution as a solid. This precipitation can serve as a driving force for the reaction to go to completion.
- Nitric Acid (HNO): A strong mineral acid that remains in solution.
Chemical Equation
The chemical equation representing this reaction is:
Ca(NO3)2 + H2SO4 → CaSO4 + 2HNO
This equation illustrates how calcium from calcium nitrate combines with the sulfate group from sulphuric acid to form calcium sulfate, while the nitrate group from calcium nitrate combines with hydrogen from sulphuric acid to form nitric acid.
Summary of Reactants and Products
To provide a clear overview of the reaction:
| Category | Chemical Formula | Common Name | Typical State | Key Characteristic |
|---|---|---|---|---|
| Reactant | Ca(NO3)2 | Calcium Nitrate | Aqueous Solution | Soluble |
| Reactant | H2SO4 | Sulphuric Acid | Aqueous Solution | Strong Acid |
| Product | CaSO4 | Calcium Sulfate | Solid/Precipitate | Low Solubility |
| Product | 2HNO | Nitric Acid | Aqueous Solution | Strong Acid |
Practical Considerations
The formation of calcium sulfate as a precipitate is a key characteristic of this reaction. In industrial or laboratory settings, this property can be utilized for various purposes, such as removing calcium ions from a solution or producing nitric acid. The efficiency of the reaction and the yield of products can be influenced by factors such as concentration, temperature, and mixing conditions.
