List the sulfates of the Group 2 A metals in order of increasing solubility in water. Explain the trend. (Hint: You need to consult a chemistry handbook.)

Short Answer

Expert verified
In general, the solubility of Group 2A sulfates decreases from BeSO₄ to BaSO₄ as the ion size increases from Be to Ba. This is due to a decrease in hydration energy and relatively constant lattice energy as we move down the group.

Step by step solution

01

Retrieving Solubility Data

Consult a reliable chemistry handbook or a related resource and find the solubility of the sulfates of Group 2 A metals. Group 2 A metals include Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), and Barium (Ba). So, find the solubilities of BeSO₄, MgSO₄, CaSO₄, SrSO₄, and BaSO₄, and list them down.
02

Organizing Solubility Data

Organize this data in increasing order of solubility. That means starting with the metal sulfate having the least solubility and ending with the one having the greatest solubility.
03

Explaining the Trend

The solubility trends in water for Group 2 A metal sulfates typically reflect the hydration energy and the lattice energy of the sulfates. As we move down the group, the size of the cation increases, which decreases the effective charge density, thus, the hydration energy decreases. But, the lattice energy changes less significantly. So, the solubility decreases on moving down the group in Group 2 A elements.

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