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Group IV, The Carbonate Group PRELAB NAME: 1. How is the Ba separated from Ca?? 2. What test is used to confirm the presence
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Answer #1

1. Ba2+ can be separated from Ca2+ by the concept of fluorides solubility. They differ in the Solubility of the fluorides, BaF2 and CaF2. Ex. When fluoride ions are subjected to add to the 0.1M Ba2+ and Ca2+ solution the precipitation of CaF2, will from immediately.

2. Test used to confirm the presence of calcium.

Confirmation is done by dissolving the precipitate obtained from the group analysis, in the concentrated Hydrochloric acid and flame test. If Calcium is present Calcium Oxalate precipitate is obtained from neutral and alkaline solutions, indicating the presence of Ca2+, whereas Ba2+ and Sr2+ are absent. While testing the acidity of the solution with litmus paper Caclium shows Brick red color in medium and fleeting.

3. Presence of Ba2+ and Ca2+ will affect the test of Mg2+. While reaction with Sodium suphate Magnesium sulphate is soluble. But if Ba2+ present it won't get soluble. And for Calcium sulphate it is hardly soluble, but there won't be any precipitate formation during this experiment.

4. MgCO3 is more soluble. The reason is radius of ion increases down the group in periodic table. Dissociation of anion(CO3-) and Cation(Mg2+/Ba2+) takes place When MgCO3 or BaCO3 reacts with water. O2- anion form from the dissociation of water molecule gets accomplish with the cations (Mg2+/Ba2+). As the radius of ion increases down the group in the table, Mg2+ is smaller in size, so the association with O2- is effortless. The Size of Ba2+ has larger radius than O2-.So it is not possible. This proves that MgCO3 is more soluble. This concept is also for CaCO3.

By taking hydration energy into consideration, Solubility will be more when hydration energy is higher. According to the down any group hydration energy decreases, so that the solubility of BaCO3 and CaCO3 will also be lower than MgCO3

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