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A hydrated salt has a number of waters of hydration combined to each molecule of salt whereas an anhydrous salt is one that has had its waters of hydration removed. An example of a hydrated salt is nickel sulfate hexahydrate, NiSO4·6H2O. The waters of hydration can be removed by a simple heating, resulting in NiSO4(s) + 6H2O(g).
Only some salts have hydrates, not all. These salts contain in the formula water of crystallization.
'Salt' is a non-specific term in chemistry that refers to the solid crystallized state of matter that is formed when an ionically bonded compound solidifies. Anhydrous means when the salt is crystallizing, no water is captured within the crystal matrix.
Hydrated salts appear dry because they have incorporated water molecules within their crystal lattice structure. This water is not easily visible on the surface of the salt, giving the appearance of dryness. However, if the hydrated salt is heated or exposed to low humidity conditions, the water molecules can be released, causing the salt to become visibly wet.
Li+ has maximum degree of hydration and for this reason lithium salts are mostly hydrated
Anhydrous salts prepared by evaporating the water contained in a hydrated salt. However, anhydrous salts are non-electrolytes, meaning they can't pass an electric current.
When an anhydrous salt retain water in the crystalline structure.
On heating, hydrated salts lose their water of crystallization and as a result, the crystals lose their shape and colour and change to a powdery substance.
A hydrated salt has a number of waters of hydration combined to each molecule of salt whereas an anhydrous salt is one that has had its waters of hydration removed. An example of a hydrated salt is nickel sulfate hexahydrate, NiSO4·6H2O. The waters of hydration can be removed by a simple heating, resulting in NiSO4(s) + 6H2O(g).
Depends on if it is hydrated or not. If hydrated, magnesium sulfate heptahydrate, then (7.6g)/(246.47g/mole)=.0308mole. If anhydrous (7.6g)/(120.415g/mole)=0.063mole.
anhydrous is an adjective usually used to describe the properties of certain salts in that they tend to absorb water directly from sufficiently humid air.
No, only some salts change the color after dehydration.
Mg S O4 . 7 H2 O is a hydrated crystal (Epsom salt - bath salts) 246.47 g/mol (heptahydrate) Mg S O4 is an anhydrous salt 120.415 g/mol (anhydrous)
In the body salts are dissolved in water, blood etc.
The change of color after dehydration is not a general phenomenon.
The hydrated forms of these compounds are lower energy thermodynamically than the anhydrous forms. It takes heat energy to drive the water out of these salts to make them anhydrous. If left in the open, the anhydrous forms will take up water from the atmosphere and re-hydrate themselves. This process releases heat energy, so it "runs downhill" energy-wise.
Because these salts can easily absorb water and become hydrates.