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solubility rules for alkaline earth metals

For example, barium has more activity than strontium or calcium. The alkaline earth metals are soluble. Because BeO and MgO are much more inert than the other group 2 oxides, they are used as refractory materials in applications involving high temperatures and mechanical stress. Solubility of sulphates and carbonates of alkaline earth metals decreases as the atomic number of the metal increases down the group because the size of the cation increases down the group. This question illustrates it well. All alkali metals sulfide and alkaline earth metals sulfides are soluble in water and form colourless aqueous solutions. Actually I have to tell you it ranges from “not very” to “almost completely insoluble”. Hydroxides of the lighter alkaline earth metals are insoluble in water, but their solubility increases as the atomic number of the metal increases. Solubility of sulfates generally decrease as you go down a group. There are solubility rules to follow when prdicting the solubility of a salt.see below. Most of the precipitation reactions that we will deal with involve aqueous salt solutions. Solubilities of the halides, nitrates, carbonates, sulfates, and some perchlorates of all the alkali metals and alkaline earth metals in methanol at room temperature have been determined. so your answer becomes BaSO4

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