Q&A Hero

Q: For which of the following reactions is Sº at 25ºC closest to zero?A) N2(g) + O2(g) → 2NO(g)B) H2(g) + I2(s) → 2HI(g)C) CH3CHO(g) + 5/2O2(g) → 2CO2(g) + 2H2O(g)D) 2NO(g) + O2(g) → 2NO2(g)E) C2H4(g) + Br2(l) → C2H4Br2(l)

Q: The following reaction represents a step in the separation of which analytical group of cations?Cu2+(aq) + S2-(aq) → CuS(s)A) Analytical Group IB) Analytical Group IIIC) Analytical Group VD) Analytical Group IVE) Analytical Group II

Q: Consider a solution containing the following cations: Na+, Hg2+, Mn2+, Al3+and Ag+. Treatment of the solution with dilute, HCl followed by saturation with H2S, results in formation of precipitate(s). Which ions still remain in solution (did not precipitate)? A) Na+, Hg2+, Al3+ B) Na+only C) Ag+ and Hg2+ D) Ag+only E) Na+, Al3+, and Mn2+

Q: In the sulfide scheme for qualitative analysis, the cations of Analytical Group IV are precipitated as phosphates or carbonates. Analytical Group IV consists of A) alkaline earth elements. B) the halogens. C) alkali metals. D) transition metals having +2 ions. E) none of these

Q: What is the effect of substituting soluble metal salts such as NaCl and K2CO3for HCl or (NH4)2CO3in the qualitative analysis scheme for separating the five Analytical Groups? A) You can no longer tell if your original sample contained Na+or K+. B) There is no effect on the analysis since Na+and K+do not form a precipitate. C) The NaCl and K2CO3are not pure, analytical grade materials. D) Potassium ion forms a precipitate with sulfide ion. E) Na+and K+react violently with acids such as H2S, producing highly flammable and potentially explosive hydrogen gas.

Q: In the qualitative analysis scheme for metal ions, how are the Analytical Group III cations separated from the cations of Analytical Groups IV and V? A) by addition of H2S in acidic solution, forming insoluble metal sulfides B) by addition of (NH4)2CO3or (NH4)3PO4, forming insoluble metal carbonates or phosphates C) by addition of H2SO4, forming insoluble metal sulfates D) by addition of HCl, forming insoluble metal chlorides E) by addition of H2S in basic solution, forming insoluble metal sulfides or hydroxides

Q: Which of the following statements concerning the separation of metal ions into Analytical Groups I-V is/are correct? 1) The substitution of dilute Zn(Cl)2for dilute HCl in step one, the precipitation of the Analytical Group I metal ions as chloride salts, will have no effect on the rest of the analysis. 2) Group I ions cannot be precipitated using this scheme. 3) In the filtration stages, the filtrate is the solid material that is removed from the mixture by filtration. A) 1 only B) 2 only C) 3 only D) 1 and 2 E) 1, 2, and 3

Q: Which of the following statements concerning the separation of metal ions into Analytical Groups I-V is/are correct? 1) Only the least soluble sulfides will precipitate in an acidic solution of H2S. 2) K+and Na+are precipitated in the last step of the separation scheme. 3) The formation of a precipitate with the addition of dilute HCl(aq) indicates the original solution contains all of the ions of Analytical Group I (the ions which precipitate as chlorides). A) 1 only B) 2 only C) 3 only D) 1 and 2 E) 1, 2, and 3

Q: What is the molar solubility of zinc hydroxide at pH 12.40? For Zn(OH)2, Ksp=2.1x10-16; for Zn(OH)42-, Kf=2.8x1015.A) 9.4 x10-26MB) 1.5 x10-2MC) 3.7 x10-4MD) 3.7 x10-6ME) 1.4 x10-8M

Q: What is the molar solubility of nickel(II) sulfide in 0.053M KCN? For NiS, Ksp=3.0x10-19; for Ni(CN)42-, Kf=1.0x1031.A) 5.5 x10-10MB) 5.3 x10-2MC) 1.5 x10-19MD) 1.3 x10-2ME) 2.2 x10-5M

Q: Given the following equilibrium constants,AgIO3 Ksp = Ag(NH3)2+ Kf = determine Kc for the dissolution of the sparingly soluble salt AgIO3 in aqueous ammonia (shown below).AgIO3(s) + 2NH3(aq) Ag(NH3)2+(aq) + IO3-(aq)A) B) C) D) 1.9E)

Q: Given the two equilibria below,Ag(NH3)2+(aq) Ag+(aq) + 2NH3(aq); Kd = 5.9 x10-8AgCN(s) Ag+(aq) + CN-(aq); Ksp= what is Kc for the following equilibrium?AgCN(s) + 2NH3(aq) Ag(NH3)2+(aq) + CN-(aq)A) B) C) D) E)

Q: What will happen if 50.0 mL of 0.022 M Na2S2O3, 50.0mL of 0.010M AgNO3, and 50.0mL of 0.097M KCl are mixed together? For AgCl, Ksp=1.8x10-10; for Ag(S2O3)23-, Kf=2.9x1013.A) A precipitate of Ag2S2O3 will form.B) A precipitate of KNO3 will form.C) No precipitate will form because silver(I) ion exists predominantly as Ag+.D) No precipitate will form because silver(I) ion exists predominantly in the complex Ag(S2O3)23-.E) A precipitate of AgCl will form.

Q: The figure below represents the results of adding NH3 to a saturated solution of an ionic compound. Which of the following could the ionic compound be?A) AgCl or CaF2B) CaF2C) Mg(OH)2D) AgClE) SrCO3

Q: Which sparingly soluble salt will exhibit the highest solubility at low pH's?A) PbS (Ksp= 2.5 x10-27)B) MnS (Ksp= 2.5 x10-10)C) HgS (Ksp= 1.6 x10-52)D) NiS (Ksp= 3 x10-9)E) ZnS (Ksp= 1.1 x10-21)

Q: Which of the following insoluble salts will dissolve upon reaction with excess ammonia? A) BaSO4 B) CaCO3 C) PbSO4 D) HgS E) AgCl

Q: What is the concentration of Cd2+in a 0.010 M Cd(NO3)2 solution that is also 1.0M NH3? For Cd(NH3)42+,Kf=1.0x107.A) 3.2 x10-5MB) 1.0 x10-9MC) 1.2 x10-9MD) 3.2 x10-4ME) 1.0 x10-2M

Q: Suppose sodium hydroxide is added to a 0.0016 M solution of zinc nitrate such that the pH of the solution is 13.42. What is the equilibrium concentration of Zn2+?Zn2+(aq) + 4OH-(aq) Zn(OH)42-(aq); Kf= 2.8 x1015A) 2.2 x10-18MB) 1.6 x10-3MC) 6.6 x10-2MD) 1.2 x10-16ME) 2.2 x10-18M

Q: An aqueous solution of Ag(CN)2-is made by combining 0.0100 moles AgNO3 with 1.00 mole NaCN and diluting to 1.000 L. What is the molar concentration of Ag+in the solution?Ag+(aq) + 2CN-(aq) Ag(CN)2-(aq); Kf= 5.6 x1018A) 1.9 x10-21MB) 5.3 x1020MC) 5.8 x1016MD) 1.7 x10-17ME) 0.010 M

Q: What is the molar equilibrium concentration of uncomplexed Ag+(aq) in a solution composed of 1.1 mol Ag(CN)2-dissolved in 1.00 L of 0.47 M NaCN. Kf for Ag(CN)2-is .A) MB) MC) MD) ME) M

Q: Cyanide ion forms very stable complex ions with a variety of metal ions. What is the molar equilibrium concentration of uncomplexed Cu2+(aq) in a solution that initially contains 1.3mol of Cu(CN)2- per liter of solution . Kf for Cu(CN)2- is .A) MB) MC) MD) ME) M

Q: Calculate the molar concentration of uncomplexed Zn2+(aq) in a solution that contains 0.22mol of Zn(NH3)42+ per liter and 0.3109M NH3at equilibrium. Kf for Zn(NH3)42+is .A) MB) MC) MD) ME) M

Q: Which of the following statements concerning amphoteric hydroxides is/are correct?1) The amphoteric hydroxide of aluminum(III) is commercially used to separate aluminum(III) oxide from impurities in the aluminum ore bauxite.2) Amphoteric hydroxides form soluble complex ions at high pH's.3) The amphoteric hydroxide, Zn(OH)2, can be precipitated by increasing the pH of a solution containing Zn2+(aq) or lowering the pH of a solution containing Zn(OH)42-.A) 1 onlyB) 2 onlyC) 3 onlyD) 1 and 2E) 1, 2, and 3

Q: Which of the following is not likely to form a complex ion with Al3+?A) NH4+B) NH3C) OH-­D) H2OE) CH3NH2

Q: What is the value of the dissociation constant, Kd, for the complex ion Cd(NH3)42+? For Cd(NH3)42+, Kf=1.0x107.A) 1.0 x10-7B) 2.5 x106C) 1.0 x107D) 5.6 x101E) 1.0 x10-7

Q: Suppose hydrogen sulfide is added to a solution that is 0.0010 Min Fe2+, Cd2+, Co2+, and Mn2+ such that the concentration of H2S is 0.10 M. When the pH of the solution is adjusted to 3, a precipitate forms. What is the composition of the precipitate?H2S(aq) + 2H2O(l) 2H3O+(aq) + S2-(aq); Kc= 1.1 x10"20 SaltKspFeS6.0 x10-18CdS8.0 x10-27CoS4.0 x10-21MnS2.5 x10-10A) CdS onlyB) CdS, CoS, FeS, and MnSC) CdS, CoS, and FeSD) CdS and FeSE) CdS and CoS

Q: Suppose hydrogen sulfide is added to a solution that is 0.10 M in Cu2+, Pb2+, and Ni2+such that the concentration of H2S is 0.10 M. When the pH of the solution is adjusted to 1.00, a precipitate forms. What is the composition of the precipitate?H2S(aq) + 2H2O(l) 2H3O+(aq) + S2-(aq); Kc= 1.1 x10-20SaltKspCuS6.0 x10-36PbS2.5 x10-27NiS3.0 x10-19A) CuS onlyB) PbS and NiSC) CuS and PbSD) NiS onlyE) CuS, PbS, and NiS

Q: What is the best way to ensure complete precipitation of SnS from a saturated H2S solution? A) Add a strong acid. B) Add a weak acid. C) Add a strong base. D) Add a weak base. E) Add more H2S.

Q: The figure below represents the results of adding a strong acid to a saturated solution of an ionic compound. Which of the following could be the ionic compound? A) AgClO4 B) AgF C) AgI D) AgCl E) AgBr

Q: In which of the following solutions would CaC2O4have the highest molar solubility?A) 0.01 M Na2C2O4B) 0.01 M NaClC) 0.01 M HClD) 0.01 M Ca(NO3)2E) 0.01 M NaHC2O4

Q: Which of the following substances will increase the molar solubility of nickel(II) phosphate in a saturated solution? A) AgCl B) HNO3 C) KOH D) AlPO4 E) Na3PO4

Q: For which of the following salts would the addition of nitric acid increase its solubility?A) AgIB) AgNO3C) AgClD) Ag2SO4E) AgBr

Q: You have two salts, AgX and AgY, with very similar Ksp values. You know that Ka for HX is much greater than Ka for HY. Which statement will be true?A) AgX and AgY are less soluble in acidic solution than in pure water.B) AgX is more soluble in acidic solution.C) AgX and AgY are equally soluble in acidic solution.D) AgY is more soluble in acidic solution.E) none of these

Q: The best explanation for the dissolution of ZnS in dilute HCl is that A) the zinc ion is amphoteric. B) the sulfide ion concentration is decreased by the formation of H2S. C) the solubility product of ZnCl2is less than that of ZnS. D) the zinc ion concentration is decreased by the formation of a chloro complex. E) the sulfide ion concentration is decreased by oxidation to sulfur.

Q: A solution contains 0.018 mol each of I-, Br-, and Cl-. When the solution is mixed with 200mL of 0.24M AgNO3, how much AgCl(s) precipitates out?Ksp AgI = 1.5 x10-16Ksp AgBr = 5.0 x10-13Ksp AgCl = 1.6 x10-10A) 5.0 gB) 3.3 gC) 2.6 gD) 0.0 gE) 1.7 g

Q: Silver nitrate (AgNO3) is slowly added to a solution containing 0.100 M Br-and 0.050 M FeCN64- until a precipitate just forms. What is the molar concentration of Ag+just as the precipitate forms? AgBr Ksp= 5.0 x10-13and Ag4FeCN6 Ksp= 8.5 x10-45.A) 2.0 x10-11M Ag+B) 5.0 x10-12M Ag+C) 1.0 x10-11M Ag+D) 3.3 x10-12M Ag+E) 1.7 x10-43M Ag+

Q: Solid KCN is added to a solution composed of 0.10 M Ag+and 0.10 M Zn2+just until a precipitate forms. What is the composition of this initial precipitate? AgCN Ksp= 2.2 x10-16and Zn(CN)2Ksp= 3 x10-16.A) The precipitate is pure AgCN(s).B) The precipitateis pure Zn(CN)2(s).C) The precipitate is a mixture of AgCN(s) and Zn(CN)2(s).D) The precipitate is a mixture of KCN(s) and AgCN(s).E) The precipitate is a mixture of KCN(s) and Zn(CN)2(s).

Q: Sodium chloride is added slowly to a solution that is 0.010 M in Cu+, Ag+, and Au+. The Kspvalues for the chloride salts are 1.9x10-7, 1.6x10-10, and 2.0x10-13, respectively. Which compound will precipitate first?A) AuCl(s)B) All will precipitate at the same time.C) It cannot be determined.D) AgCl(s)E) CuCl(s)

Q: For which pair of cations would the addition of dilute hydrobromic acid precipitate one but not the other? A) Ag+and Ca2+ B) Hg22+and Ag+ C) Ba2+and Na+ D) Ca2+and Ba2+ E) Pb2+and Ag+

Q: Which of the following solutions should be added to a solution containing both copper(II) ions and silver(I) ions in order to precipitate only one of the ions?A) HCl(aq)B) H2S(aq)C) HNO3(aq)D) H2S(aq) + HCl(aq)E) H2S(aq) + HNO3(aq)

Q: What is the maximum concentration of carbonate ions that will precipitate BaCO3 but not MgCO3 from a solution that is M each in Mg2+ and Ba2+? For MgCO3, Ksp=1.0x10-5and for BaCO3, Ksp=2.6x10-9.A) MB) MC) MD) ME) 2.6 x10-14M

Q: A solution is 0.010 M in each of Pb(NO3)2, Mn(NO3)2, and Zn(NO3)2. Solid NaOH is added until the pH of the solution is 8.50. Which of the following statements is true?SaltKspPb(OH)21.4 x10-20Mn(OH)22.0 x10-13Zn(OH)22.1 x10-16A) Only Mn(OH)2will precipitate.B) All three hydroxides will precipitate.C) Only Pb(OH)2will precipitate.D) No precipitate will form.E) Only Zn(OH)2and Pb(OH)2will precipitate.

Q: What is the maximum volume of 4.9 x10-5M K2CrO4that, added to 17.0 mL of a solution that is 8.6x10-5M Ba(NO3)2and 5.4x10-6M Pb(NO3)2, will precipitate PbCrO4 but not BaCrO4? For PbCrO4, Ksp=1.8x10-14, and for BaCrO4, Ksp=1.2x10-10.A) 17 mLB) 0.51 mLC) 0.48 mLD) 0.0012 mLE) 7.7 mL

Q: What is the minimum mass of Na2CO3 that must be added to 24.6 mL of a 9.5x10-4M AgNO3 solution in order for precipitation to occur? For Ag2CO3, Ksp=8.6x10-12.A) 2.5 x10-3gB) 3.1 x10-4gC) 1.2 x10-3gD) 2.4 x10-8gE) 2.5 x10-5g

Q: If 270 mL of 1 x10-8M Al(NO3)3 is mixed with 270 mL of 1x10-8M NaOH, what will occur? For Al(OH)3, Ksp=4.6x10-33.A) Aluminum hydroxide will precipitate.B) Sodium hydroxide will precipitate.C) Aluminum nitrate will precipitate.D) Sodium nitrate will precipitate.E) No precipitate will form.

Q: If 315 mL of 1 x10-4M Ca(NO3)2 is mixed with 315 mL of 1x10-4 M NaF, what will occur? For CaF2, Ksp=3.4x10-11.A) No precipitate will form.B) Sodium nitrate will precipitate.C) Calcium nitrate will precipitate.D) Calcium fluoride will precipitate.E) Sodium fluoride will precipitate.

Q: If 270 mL of 1 x10-7M AgNO3is mixed with 270 mL of 1x10-8M NaI, what will occur? For AgI, Ksp=8.3x10-17.A) Sodium nitrate will precipitate.B) Silver(I) nitrate will precipitate.C) Sodium iodide will precipitate.D) Silver(I) iodide will precipitate.E) No precipitate will form.

Q: Suppose 50.00 mL of a 1 x10-5M solution of lead(II) nitrate is mixed with 50.00mL of a 1x10-6 solution of sodium phosphate. Which of the following statements is true? For lead(II) phosphate, Ksp=1x10-44.A) A precipitate forms because Qc< Ksp.B) No precipitate forms because Qc> Ksp.C) A precipitate forms because Qc> Ksp.D) No precipitate forms because Qc= Ksp.E) No precipitate forms because Qc< Ksp.

Q: If 500 mL of 1.4 x10-6M AgNO3is mixed with 500 mL of 1.4x10-6M NaBr, what will occur? For AgBr, Ksp=5x10-13.A) Silver(I) bromide will precipitate.B) The concentration of Ag+will be 1.4 x10-6M.C) 7.0 x10-7mol of AgBr will form.D) No precipitation will occur.E) Sodium bromide will precipitate.

Q: What is the maximum hydroxide-ion concentration that a 0.027 M MgCl2solution could have without causing the precipitation of Mg(OH)2? For Mg(OH)2, Ksp=1.8x10-11.A) 4.2 x10-6B) 1.7 x10-4C) 1.2 x10-8D) 6.7 x10-9E) 2.6 x10-5

Q: What is the minimum concentration of Cu2+ required to begin precipitating Cu(OH)2(s) in a solution of pH 10.77? For Cu(OH)2, Ksp=2.6x10-19.A) 2.9 x10-4MB) 1.5 x10-8MC) 4.4 x10-16MD) 7.5 x10-13ME) 2.2 x10-21M

Q: A 4.0 x10-4 M solution of MnSO4 is gradually made more basic by adding NaOH. At what pH will manganese(II) hydroxide begin to precipitate? For Mn(OH)2, Ksp=2.0x10-13.A) 4.70B) 9.57C) 4.65D) 9.35E) 9.30

Q: What will happen if 0.1 mol of solid silver(I) nitrate is added to 1.0 L of a saturated solution of silver(I) chromate? For Ag2CrO4, Ksp=2.4x10-12.A) The AgNO3will settle to the bottom without dissolving.B) The concentration of CrO42-will increase.C) Some Ag2CrO4will precipitate.D) Nothing will happen.E) The concentration of Ag+in solution will not change.

Q: What is the maximum Sr2+concentration possible in a solution that has a M sulfide-ion concentration without precipitating strontium sulfate? For SrSO4, Ksp=2.5x10-7.A) MB) MC) MD) ME) M

Q: To 1.0 L of water, 3.0 x10-6mol of Pb(NO3)2, 4.0 x10-6mol of K2CrO4, and 1.0 mol of NaCl are added. What will happen?SaltKspPbCrO41.8 x10-14PbCl21.6 x10-5A) A precipitate of KCl will form.B) A precipitate of PbCrO4 will form.C) A precipitate of PbCl2 will form.D) No precipitate will form.E) Both a precipitate of PbCl2 and a precipitate of PbCrO4 will form.

Q: Suppose 50.00 mL of 2.0 x10-6M Fe(NO3)3 is added to 50.00 mL of 2.0 x10-4M KIO3. Which of the following statements is true? For Fe(IO3)3, Ksp=1.0x10-14.A) A precipitate forms because Qc> Ksp.B) A precipitate forms because Qc< Ksp.C) No precipitate forms because Qc< Ksp.D) No precipitate forms because Qc= Ksp.E) No precipitate forms because Qc> Ksp.

Q: Which of the following will apply to a saturated solution of an ionic compound? A) Qc< Ksp B) Qc> Ksp C) Qc= Ksp D) Ksp= 1 E) Qc= 1

Q: For which of the following will precipitation be expected? A) Qc< Ksp B) Qc= 1 C) Qc= Ksp D) Qc> Ksp E) Ksp= 1

Q: Which Figures I-IV represent(s) the result of mixing aqueous solutions of NaOH and CuCl2in which the ion product Qc> Ksp for the insoluble product? (C = cation, A = anion)A) only IIB) both I and IIC) only IVD) only IE) only III

Q: Which of Figures I-IV represent(s) the result of mixing aqueous solutions of Na2S and NiCl2in which the ion product Qc> Ksp for the insoluble product? (C = cation, A = anion)A) both I and IIB) only IC) only IID) only IIIE) only IV

Q: How many moles of CaF2 will dissolve in 3.0 L of 0.051 M NaF solution? (Ksp for CaF2=4.0x10-11)A) 2.6 x10-10B) 1.5 x10-8C) 4.6 x10-8D) 5.1 x10-9E) none of these

Q: Which of the following, when added to a saturated solution of AgCl, will cause a decrease in the molar concentration of Ag+ relative to the original solution?1) HCl(g)2) AgCl(s)3) MgCl2(s)A) 1 onlyB) 2 onlyC) 3 onlyD) 1 and 3E) 1, 2, and 3

Q: The solubility of La(IO3)3in a 0.62 M KIO3solution is 1.0 x10-7mol/L. Calculate Ksp for La(IO3)3.A) 6.2 x10-8B) 2.4 x10-22C) 2.4 x10-1D) 2.4 x10-8E) none of these

Q: Ksp for PbF2 is 4.0 x10-8. If a 0.034 M NaF solution is saturated with PbF2, what is [Pb2+] in solution?A) 4.6 x10-11MB) 1.4 x10-9MC) 1.2 x10-6MD) 1.0 x10-3ME) 3.5 x10-5M

Q: What is the molar solubility of MgF2 in a 0.45 MNaF solution? For MgF2, Ksp=8.4x10-8.A) 1.0 x10-7 MB) 1.4 x10-4 MC) 1.9 x10-7 MD) 7.1 x10-4 ME) 4.1 x10-7 M

Q: What is the molar solubility of MgF2in a 0.40 MMg(NO3)2solution? For MgF2, Ksp=8.4x10-8.A) 8.0 x10-8MB) 2.3 x10-4MC) 2.0 x10-8MD) 4.6 x10-4ME) 3.2 x10-3M

Q: What is the concentration of silver(I) ion in a saturated solution of silver(I) carbonate containing 0.0030 M Na2CO3? For Ag2CO3, Ksp=8.6x10-12.A) 6.0 x10-4MB) 2.0 x10-9MC) 8.0 x10-9MD) 5.4 x10-5ME) 8.0 x10-4M

Q: The figure below represents the result of adding which of the following aqueous solutions to a filtered, saturated solution of AgCl? A) only NaCl(aq) B) only HNO3(aq) C) HCl(aq) or NaCl(aq) D) only HCl(aq) E) HCl(aq) or HNO3(aq)

Q: In which of these solutions would silver(I) carbonate have the lowest molar solubility? For silver(I) carbonate, Ksp=8.5x10-12.A) 0.03 M H2CO3B) 0.1 M AgNO3C) 0.01 M AgNO3D) 0.1 M Na2CO3E) pure water

Q: In which of the following solutions would silver(I) phosphate, Ag3PO4, be least soluble?A) 0.10 MNa3PO4B) 0.10 MAgNO3C) 0.10 MNa2HPO4D) 0.10 MHNO3E) 0.10 MNaH2PO4

Q: The insoluble salts AV, B2W, C2X3, DY2, and EZ3, which were formed from the metal ions A+, B+, C3+, D2+, and E3+and the nonmetals V1-, W2-, X2-, Y1", and Z1-, all have the same Ksp value. Which salt has the highest molar solubility?A) AVB) EZ3C) DY2D) B2WE) C2X3

Q: Rank the following salts in order of increasing molar solubility.SaltKspAgSCN1.0 x10-12Ag2CrO41.1 x10-12Ag3PO41.0 x10-16A) AgSCN < Ag2CrO4< Ag3PO4B) AgSCN < Ag3PO4< Ag2CrO4C) Ag3PO4< Ag2CrO4< AgSCND) Ag3PO4< AgSCN < Ag2CrO4E) Ag2CrO4< AgSCN < Ag3PO4

Q: What is the pH of a saturated solution of Ni(OH)2? For Ni(OH)2, Ksp=2.0x10-15.A) 4.80B) 8.90C) 5.10D) 9.20E) 7.00

Q: What is the hydroxide-ion concentration of a saturated solution of Ni(OH)2? For Ni(OH)2, Ksp=2.0x10-15.A) 2.8 x10-3MB) 7.9 x10-6MC) 1.0 x10-7MD) 2.7 x10-2ME) 1.6 x10-5M

Q: Which salt has the lowest molar solubility in pure water? Salt Ksp Cd(OH)2 5.3 x10-15 Fe(OH)2 8.0 x10-16 PbCrO4 1.8 x10-14 CdCO3 6.2 x10-12 Mn(OH)2 2.0 x10-13 A) PbCrO4B) Fe(OH)2C) CdCO3D) Cd(OH)2E) Mn(OH)2

Q: Which salt has the highest molar solubility in pure water? Salt Ksp Cd(OH)2 5.3 x10-15 Fe(OH)2 8.0 x10-16 PbCrO4 1.8 x10-14 CdCO3 6.2 x10-12 Mn(OH)2 2.0 x10-13 A) CdCO3B) Cd(OH)2C) Mn(OH)2D) PbCrO4E) Fe(OH)2

Q: Which of the following salts has the highest molar solubility in water?A) CaCO3(Ksp= 3.8 x10-9)B) Ni(OH)2(Ksp= 2.0 x10-15)C) Fe(OH)2(Ksp= 8 x10-16)D) AgBr (Ksp= 5.0 x10-13)E) PbI2(Ksp= 6.5 x10-9)

Q: Which of the following salts has the lowest molar solubility in water?A) Ni(OH)2(Ksp= 2.0 x10-15)B) Fe(OH)2(Ksp= 8 x10-16)C) PbI2(Ksp= 6.5 x10-9)D) SrCO3(Ksp= 9.3 x10-10)E) AgBr (Ksp= 5.0 x10-13)

Q: Pure water is saturated with slightly soluble calcium fluoride, CaF2. Which of the following is true concerning the equilibrium concentration of Ca2+?A) B) [Ca2+] = [F"]C) D) E) [Ca2+] = Ksp

Q: What is the solubility (in g/L) of calcium fluoride at 25ºC? The solubility product constant for calcium fluoride is 3.4x10-11at 25ºC.A) 0.00046 g/LB) 2.7 x10-9g/LC) 0.016 g/LD) 1.3 x10-9g/LE) 0.094 g/L