Hydration and Crystallization of Salts
Chemistry ⇒ Acids, Bases, and Salts
Hydration and Crystallization of Salts starts at 9 and continues till grade 12.
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See sample questions for grade 9
A sample of hydrated magnesium sulfate (MgSO4·7H2O) weighs 12.0 g. After heating, the residue weighs 5.9 g. Calculate the mass of water lost.
A student heats 5 g of hydrated copper(II) sulfate (CuSO4·5H2O) and obtains 3.2 g of anhydrous copper(II) sulfate. How much water was lost during heating?
Describe how you would obtain pure crystals of copper(II) sulfate from its solution.
Describe the process of crystallization.
Describe what happens when hydrated copper(II) sulfate is exposed to air for a long time.
Explain the difference between a hydrated and an anhydrous salt.
Explain why hydrated salts are important in chemical analysis.
Explain why hydrated salts often have bright colors, while their anhydrous forms are usually white or pale.
Explain why some salts are deliquescent.
What happens to the color of copper(II) sulfate when it is heated and loses its water of crystallization?
What is meant by the term 'anhydrous'?
What is meant by the term 'efflorescence' in relation to hydrated salts?
What is meant by the term 'hydrated salt'?
What is the chemical formula for washing soda?
What is the main difference between efflorescent and deliquescent salts?
What is the role of water of crystallization in the structure of a salt?
What is the significance of the dot (·) in the formula of a hydrated salt, such as CuSO4·5H2O?
What is water of crystallization?
