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anigeo
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is it necessary that all crystalline solids are hydrated or hygroscopic.
could anyone explain me the case of NACl and NA2CO3.10H2O?
could anyone explain me the case of NACl and NA2CO3.10H2O?
anigeo said:is it so that Na2CO3.10H2O crystalline and Na2CO3 not?if not what it is.
Borek said:Please elaborate, I don't understand your question.
Many substances will contain crystalline water when crystallized from water solutions, and it can be difficult to prepare their anhydrous crystals. In such cases it may mean anhydrous crystals will be very hygroscopic. It doesn't mean every crystal of every substance contains crystalline water and is hygroscopic, as is clearly shown by the quartz example.
The chemical formula for sodium chloride is NaCl, which means that it is composed of one sodium atom (Na) and one chlorine atom (Cl).
NaCl forms crystals through a process called ionic bonding. This occurs when the positively charged sodium ions (Na+) and negatively charged chloride ions (Cl-) attract and bond together in a repeating pattern, forming a crystal structure.
NaCl (sodium chloride) is a simple ionic compound, while Na2CO3.10H2O (sodium carbonate decahydrate) is a hydrated compound. This means that sodium carbonate has 10 water molecules (H2O) attached to each molecule of sodium carbonate, giving it a more complex chemical formula.
NaCl is commonly used as table salt for seasoning and preserving food. It is also used in the production of many household products such as soaps and detergents. Na2CO3.10H2O, also known as washing soda, is used in laundry detergents and water softeners.
Yes, NaCl and Na2CO3.10H2O can be separated into their individual components through different methods such as evaporation, filtration, or electrolysis. These methods take advantage of the different physical and chemical properties of the compounds to isolate them from each other.