What is the Difference Between Hydrate and Anhydrate?
🆚 Go to Comparative Table 🆚The main difference between hydrates and anhydrates lies in the presence of water molecules in their structures.
- Hydrates are compounds containing water molecules in their structure. They are formed when ionic compounds react with water molecules, typically through exposure to air. Hydrates are often found in crystalline structures and can be stable at room temperature. Examples of hydrates include gypsum, Borax, and Epsom salt.
- Anhydrates, on the other hand, are compounds that do not contain water molecules in their structure. An anhydrate is formed when water has been removed from a hydrate, either through heating or a chemical reaction. Anhydrates can be used as drying agents or desiccants, as they can absorb water molecules from the surroundings. Examples of anhydrates include anhydrous salts and silica gel.
In summary, hydrates are compounds with water molecules in their structure, while anhydrates are compounds without water molecules in their structure. Anhydrates are often obtained by removing water from hydrates through heating or chemical reactions.
On this pageWhat is the Difference Between Hydrate and Anhydrate? Comparative Table: Hydrate vs Anhydrate
Comparative Table: Hydrate vs Anhydrate
Here is a table comparing the differences between hydrates and anhydrates:
| Feature | Hydrate | Anhydrate |
|---|---|---|
| Definition | A compound containing water molecules | A compound without water molecules |
| Water Content | Contains water molecules bound to it | Water molecules have been removed, often by heating |
| Formation | Hydrates are formed when water molecules bond to the compound's structure | Anhydrates are formed by removing water molecules from a hydrate |
| Molecular Formula | The chemical formula of a hydrate includes the water molecules | The chemical formula of an anhydrate does not include water molecules |
| Reactivity | Hydrous materials do not generally decompose at room temperature | Anhydrous materials can absorb moisture from the air and may be used as drying agents |
For example, copper sulfate can exist as a hydrate (CuSO4.5H2O) or an anhydrate (CuSO4). The hydrate form contains water molecules, while the anhydrate form does not.
Read more:
- Anhydrous vs Monohydrate
- Hydrated Salt vs Anhydrous Salt
- Hydrazine vs Hydrazine Hydrate
- Hydration vs Hydrolysis
- Solvation vs Hydration
- Hydrolysis vs Dehydration
- Hydrated vs Anhydrous Copper Sulphate
- Anhydrous vs Monohydrate Citric Acid
- Hydrolysis vs Dehydration Synthesis
- Quicklime vs Hydrated Lime
- Hydration vs Hydrogenation
- Caffeine vs Caffeine Anhydrous
- Hydroxyl vs Hydroxide
- Magnesium Dihydrate vs Magnesium Trihydrate
- Acid Anhydride vs Basic Anhydride
- Betaine HCl vs Betaine Anhydrous
- Lattice Energy vs Hydration Energy
- Hydrochloride vs Dihydrochloride
- Drying vs Dehydration