What is the molar solubility of PbIO 3 2 in 005M NaIO 3 K sp 26 x 10 13 A 10 x

What is the molar solubility of pbio 3 2 in 005m naio

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29. What is the molar solubility of Pb(IO3)2in 0.05M NaIO3? (Ksp= 2.6 x 10¯13) (A) 1.0 x 10¯10(B) 5.2 x 10¯12(C) 6.4 x 10¯5(D) 2.0 x 10¯930. Addition of NH3solution to AgCl(s) will cause (A) no perceptible change. (B) AgCl to dissolve and form the soluble complex [Ag(NH3)2]+(C) AgCl to dissolve and form Ag+, (NH4)+, and Cl¯ (D) AgCl to dissolve and form the soluble complex [Ag2(NH3)]2+31. For the gas phase reaction A2<===> 2A, Keq= 1 x 105at 1000 °C. Two moles of A2are injected into a 5.0-L container at 1000 °C and allowed to reach equilibrium. What is the molar concentration of A2at equilibrium? 32. What is the oxidation number of Pt in K[PtNH3Cl5]? 33. Which element is used during steel production to oxidize impurities such as carbon and silicon?
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34. Which aqueous cation is notparamagnetic? (A) Sc3+(B) Ti3+(C) V3+(D) Cr3+35. Two-half cells are prepared and connected by a salt bridge and a wire. Both have Zn metal electrodes immersed in a solution of ZnCl2. The concentration of Zn2+is not equal in the two cells. In this complete cell, 36. Standard Reduction Potentials at 25 °C Half-Cell Reaction E° (volts) Cu2+(aq) + 2e¯ ---> Cu(s) +0.34 2H+(aq) + 2e¯ ---> H20.00 Cr3+(aq) + 3e¯ ---> Cr(s) -0.74 What is the equilibrium constant for the spontaneous reaction between the Cu/Cu2+and Cr/Cr3+half-cells at 25 °C? 37. What volume of 0.200 M KMnO4solution is required to oxidize 25.0 mL of 0.400 M FeSO4in acidic solution? (A) 2.00 mL (B) 10.0 mL (C) 25.0 mL (D) 50.0 mL 38. Calculate the number of hours an electroplating apparatus would have to operate at a current
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of 3.00 A to plate 25.0 g of chromium from a 0.500 M CrCl3solution. 39. A compound used to etch (or dissolve) glass and silicate compounds is 40. How many bonds and of what type are present in acteylene? 41. The equilibrium constant for the reaction Zn + Sn2+<===> Zn2++ Sn is very large . Which of the following sets gives the correct relative strengths of the oxidizing and reducing agents in this reaction? Oxidizing Agents Reducing Agents (A) Zn > Sn and Sn2+> Zn2+(B) Zn < Sn and Sn2+< Zn2+(C) Sn2+> Zn2+and Zn > Sn (D) Sn2+< Zn2+and Zn < Sn
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