What will happen if a mixture of BaCl2.2h2O and KCl heated up to 150 centigrade ?

Probably the only thing that will happen at 150 C is that the water associated with BaCl2.2H2O will be driven off and you will be left with BaCl2 and KCl.

0.5 g

To determine what will happen when a mixture of BaCl2·2H2O (barium chloride dihydrate) and KCl (potassium chloride) is heated up to 150 degrees Celsius, we need to consider the properties of these compounds and their behavior under heating.

First, let's understand the individual compounds:

1. BaCl2·2H2O: This is a hydrated form of barium chloride, where two water molecules are present for each molecule of BaCl2. Heating this compound will cause the water molecules to evaporate, leaving behind anhydrous (without water) barium chloride (BaCl2).

2. KCl: This is a simple ionic compound of potassium chloride. Unlike barium chloride dihydrate, it does not contain any water molecules, so it will not undergo any physical change upon heating.

Now, considering the mixture: BaCl2·2H2O and KCl are together in the solid mixture. When heated, the temperature would be insufficient to evaporate the KCl without decomposing it or reaching high temperatures where it becomes molten (KCl has a melting point of around 770 degrees Celsius).

At 150 degrees Celsius, the BaCl2·2H2O component of the mixture would begin to lose its water molecules. This means that the water would evaporate, leaving behind anhydrous BaCl2. Simultaneously, the KCl component would remain physically unchanged.

So, heating the mixture to 150 degrees Celsius would result in the evaporation of the water molecules from the BaCl2·2H2O compound, while the KCl would remain unchanged. The end result would be a mixture of anhydrous BaCl2 and KCl.

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