Barium hydroxide is used in analytical chemistry to titrate weak acids, particularly organic acids. It forms clear aqueous solutions that are free from carbonate, unlike those of the alkali hydroxides, since barium carbonate is insoluble in water.
Calculate the molar solubility of barium fluoride, BaF2, in water at 25oC. The Ksp at 25oC is 1.0 x 10-6. Since "x" represents the molarity of the Ba+2 ion, and we get one mole of barium ions for each mole of barium fluoride that dissolves.
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