Question: The solubility of the ionic compound M2X3 having a molar
The solubility of the ionic compound M2X3, having a molar mass of 288 g/ mol, is 3.60 × 10-7 g/ L. Calculate the Ksp of the compound.
Answer to relevant QuestionsFor each of the following pairs of solids, determine which solid has the smallest molar solubility. a. CaF2(s), Ksp = 4.0 × 10-11 or BaF2(s), Ksp = 2.4 × 10-5 b. Ca3(PO4) 2(s), Ksp = 1.3 × 10-32 or FePO4(s), Ksp = 1.0 × ...Explain the following phenomenon: a. Using the Ksp for Cu(OH)2 (1.6 × 10-19) and the overall formation constant for Cu(NH3)42+ (1.0 × 1013), calculate a value for the equilibrium constant for the reaction Cu(OH)2(s) + 4NH3(aq) ⇌ Cu(NH3) 42+(aq) + ...The equilibrium constant for the following reaction is 1.0 × 10-3: Consider the titration of 100.0 mL of 0.10 M phosphoric acid with 0.10 M NaOH. a. Determine the pH at the third half- equivalence point by assuming it is a “special point” (see Fig.). b. Calculate the pH at the third ...
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