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(a) If the molar solubility of BaF2 at 25 °C is 0.00358 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found tha

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s= solubility = mol Batz - BaataF Kop= [B2) Caps = [] [23] Ksp= 4503 24 * Co.00358) 3 . ksp = 1183 x 157 Solusility product oSn= koer 8.05x1035 st- hos = 108 1oge) = log (0.0166 x 1D25 = -10793-35 logs= -36.732 dio -36.732 . 10 4 = S -90183 solusity

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