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kindly answer thanks. K'sp is unknown
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- The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)At 25oC, Ksp for AgBr is 5.0 x 10-3 g. Calculate the solubility of AgBr in g L-1 at 25oC a) in pure water b) in the presence of 0.2mol L-1 NaBr solutionthe product of the solubility of PbSO4 at 25 ° C, is Ksp = 1.6 × 10-⁸. Calculate its solubility in pure water, in a solution of 0.1 M lead nitrate Pb (NO3) 2 and in a solution 0.001 M Na2SO4
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