Week 9 Solubility & Intro electrochem

Transcription

1 Week 9 Solubility & Intro electrochem Q UEST IO N 1 2 The solubility of Ag 2CO 3 is g/l at 25 C. What is the value of Ks p at this temperature? 12 A B C D E Q UEST IO N 2 The molar solubility of PbBr 2 is M at 25 C. What is the K s p of PbBr 2 at this temperature? A M B M 9 C M 4 D M 15 E M Q UEST IO N 3 At 35 C the molar solubility of CaF 2 is mol/l. What is the K s p of CaF 2 at this temperature? 9 A B C D E Q UEST IO N What is the maximum concentration of Cd that can exist in a solution in which the S concentration is M? 27 K s p(cds) = at 25 C 2 A B C D E Q UEST IO N 5 What is K s p of Zn(OH) 2 if the ph of a saturated solution in water is 8.66? 17 A B C D E Q UEST IO N 6 5 What is the [Ag ] in a saturated solution of Ag 2SO 4 in 0.2 M Na2SO 4? (K s p of Ag 2SO 4 is ) 5 A M B M C M D M E M

2 Q UEST IO N 7 Write the equation for the equilibrium associated with the aqueous dissolution of the following salts, and the corresponding expression for K s p. a. CaF2 b. BaSO4 c. Ca 3(PO 4) 2 Q UEST IO N 8 Which of the following substances will no t be more soluble in acidic solutions? A. Al(OH) 3 B. Ca 3(PO 4) 2 C. CaF2 D. BaCO3 E. PbI2 Q UEST IO N 9 Which of the following substances will no t be more soluble in acidic solutions? A. Fe(OH) 3 B. Ca 3(PO 4) 2 C. AgCl D. CaF2 E. Ag 2CO3 Q UEST IO N 10 Which one of the following substances when added to a saturated solution of AgCl will cause it to precipitate out as a solid? A. HCl B. HNO3 C. NH3 D. H2O E. None of the above substances when added to the solution will cause a precipitation of AgCl. Q UEST IO N 11 2 Solid CaF 2 is mixed into a M solution of NaF. What will be the concentration of Ca ion in the resultant solution? 11 K s p(caf 2) = at 25 C. A M 7 B M 9 C M 4 D M 15 E M Q UEST IO N 12 Which one of the following substances will decrease the solubility of Pb(OH) 2 Pb(OH) 2 in water? when added to a saturated solution of A. NaNO3 B. H2O C. HNO3 D. NaOH E. None of the above substances will cause a decrease in solubility of Pb(OH) 2.

3 Q UEST IO N 13 2 Calculate the concentration of free Cu (aq) in 1 L of a solution that contains a total of 1 10 mol of Cu(II) ion (free ions 2 12 complexed ions) and that is 0.10 M in NH 3 at equilibrium. (K f [Cu(NH 3) 4 ] = 5 10 ) A M 5 B M 18 C M 12 D M 15 E M Q UEST IO N 14 3 What is the [Cr ] in equilibrium with Cr(OH) 4 (aq) when mol of Cr(NO 3) 3 is dissolved in a liter of solution buffered at a 29 ph of 7.3? (K f for Cr(OH) 4 (aq) is ) A M B M 8 C M 23 D M 7 E M Q UEST IO N Given that K s p for AgI = and K f for Ag(CN) 2 (aq) = , what is the equilibrium constant for the following reaction? AgI(s) 2CN (aq) Ag(CN) 2 (aq) I (aq) 4 A B C D E Q UEST IO N At ph = 7.0, a saturated solution of Fe(OH) 3 has [Fe ] = M. What is the [Fe ] in a saturated solution at ph = 9.0? 24 A M 24 B M 39 C M 18 D M 18 E M Q UEST IO N 17 2 What will happen when you gradually add KOH to an aqueous solution containing M Cu (aq) and M 2 Zn (aq)? K s p of Cu(OH) 2 = ; K s p of Zn(OH) 2 = A. Cu(OH) 2 will precipitate first. B. Z n(oh) 2 will precipitate first. C. KOH will precipitate first. D. Cu(OH) 2 and Z n(oh) 2 will precipitate at the same time. E. No precipitate will form at all. Q UEST IO N 18 Will a solid precipitate form in the following solutions? 14 a M MnCl 2 solution, ph = 8 ( K s p = for Mn(OH) 2) b L of M NaF is added to L of M Ca(NO 3) 2 (K s p = for CaF 2)

4 Q UEST IO N 19 Which of the following cations form carbonate salts that are insoluble in water? I. Na 2 II. Ca III. NH4 2 IV. Pb V. K A. I and II only B. III and IV only C. II and IV only D. II and V only E. none of them Q UEST IO N An unknown solution contains one of the following metal ions: Ba, Pb, or Ag. During testing, the metal ion reacts with a solution of sodium sulfate to form a white precipitate, but it does not react with a solution of sodium chloride. Which one of the following statements is true? A. Ag is the metal ion in the solution. 2 B. Pb is the metal ion in the solution. 2 C. Ba is the metal ion in the solution. 2 D. The solution could contain BOTH Pb and Ag because both form insoluble sulfate salts. E. There is not enough information to tell which of the three ions is in the solution. Q UEST IO N 21 Element M reacts with oxygen to from an oxide with the formula MO. When MO is dissolved in water, the resulting solution is basic. What is element M most likely to be? A. Na B. Ba C. S D. N E. Al Q UEST IO N 22 What is the oxidation state of Xe in XeO 4? A. 8 B. 6 C. 4 D. 2 E. 0 Q UEST IO N 23 Which of the following substances contains a sulfur atom that cannot act as an oxidiz ing agent? 2 A. SO4 B. SO2 C. S8 2 D. SO3 E. H2S

5 Q UEST IO N 24 Which oxide has nitrogen in the lowest oxidation state? A. N2O B. N2O3 C. NO D. NO2 E. N2O4 Q UEST IO N 25 When the redox equation below is properly balanced in acidic solution, what will the coefficients be? MnO 4 (aq) H 2 (aq) H3AsO 3(aq) Mn (aq) H3AsO 4(aq) H2O(ll) MnO 4 H 2 H3AsO 3 Mn H3AsO 4 H2O A B C D E Q UEST IO N 26 The following reaction takes place in acidic solution. balanced? What is the number of protons (H (aq)) when the equation is 2 3 Cr2O 7 (aq) I (aq) Cr (aq) IO 3 (aq) A. 2 B. 4 C. 6 D. 8 E. None of the above. Q UEST IO N 27 - The following reaction takes place in basic solution. What is the number of hydroxide ions (OH (aq)) when the equation is balanced? A. 2 B. 4 C. 6 D. 8 E. 0 CN (aq) MnO 4 (aq) CNO (aq) MnO 2(s) Q UEST IO N 28 Which of the following is NOT a disproportionation (auto- oxidation) reaction? A. 3 NO 2 H2O 2 HNO 3 NO B. Cl 2 H2O HCl HOCl C. 3 KIO 2 KI KIO3 D. 2 H2O2 2 H2O O2 E. 2 NO O2 2 NO2

6 Q UEST IO N 29 What is oxidiz ed and what is reduced in the following reactions? a. C6H12O 6(s) 6 O 2(g) 6 CO 2(g) 6 H2O(l) b. 2 H2O 2(aq) 2 H2O(l) O 2(g) c. NaI(aq) 3 HOCl(aq) NaIO 3(aq) 3 HCl(aq) d. Al(OH) 4 (aq) 4 H (aq) Al 3 (aq) 4 H2O(l) e. I2O 5(s) 5 CO(g) I 2(s) 5 CO 2(g) Q UEST IO N 30 In the following reactions, what is the oxidiz ing agent? What is the reducing agent? 2 a. Cu(s) H (aq) NO 3 (aq) NO(g) H2O(l) Cu (aq) b. Mn (aq) S2O 8 (aq) 2 H2O(l) MnO 2(s) 4 H (aq) 2 SO 4 (aq) c. 3 CuO(s) 2 NH 3(aq) N 2(g) 3 H2O(l) 3 Cu(s) Q UEST IO N a. Balance the following incomplete half reaction in acid solution. Cr2O 7 (aq) Cr (aq) b. Is this an oxidation or reduction half reaction? c. How many electrons are involved in the exchange? Q UEST IO N 32 2 a. Balance the following incomplete half reaction in basic solution.pb(oh) 4 (aq) PbO 2 (s) b. Is this an oxidation or reduction half reaction? c. How many electrons are involved in the exchange? Q UEST IO N 33 a. Balance the following incomplete half reaction in basic solution.cr(oh) 3 (aq) CrO 4 2 (aq) b. Is this an oxidation or reduction half reaction? c. How many electrons are involved in the exchange? Q UEST IO N 34 Balance the following reaction in acid solution. What is oxidiz ed? What is reduced? I 2(s) HNO 3(aq) HIO 3(aq) NO 2(g) H2O(l) Q UEST IO N 35 Balance the following reactions in basic solution. a. ClO (aq) S2O 3 2 (aq) Cl (aq) SO 4 2 (aq) b. Mn(OH) 2(s) MnO 4 (aq) MnO 4 2 (aq) Q UEST IO N 36 Balance the following reaction in acid. What is oxidiz ed? What is reduced? Cl 2 (g) H2O (l) HCl (aq) HClO (aq)