Midterm 2A - Midterm II - 150 points - 11/13/2007 - Version...

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Page 1 Midterm II - 150 points - 11/13/2007 - Version A 1. Which relationship or statement best describes Δ S ° for the following reaction? K 2 SO 4 ( s ) 2K + ( aq ) + SO 4 2- ( aq ) A. Δ S ° 0 B. Δ S ° < 0 C. Δ S ° > 0 D. Δ S ° = Δ H °/ T E. More information is needed to make a reasonable prediction. 2. The formation constant for the reaction Ag + ( aq ) + 2NH 3 ( aq ) Ag(NH 3 ) 2 + ( aq ) is K f = 1.7 × 10 7 at 25°C. What is Δ G ° at this temperature? A. -1.5 kJ B. -3.5 kJ C. -18 kJ D. -23 kJ E. -41 kJ 3. A 25.0-mL sample of 0.35 M HCOOH is titrated with 0.20 M KOH. What is the pH of the solution after 25.0 mL of KOH has been added to the acid? K a = 1.77 × 10 -4 A. 4.00 B. 3.88 C. 3.63 D. 3.51 E. 3.47
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Page 2 4. An acetate buffer has a pH of 4.40. Which of the following changes will cause the pH to decrease? A. dissolving a small amount of solid sodium acetate B. adding a small amount of dilute hydrochloric acid C. adding a small amount of dilute sodium hydroxide D. dissolving a small amount of solid sodium chloride E. diluting the buffer solution with water 5. Which of the following pairs has the member with the greater molar entropy listed first? All systems are at 25°C. A. CO( g ), CO 2 ( g ) B. NaCl( s ), NaCl( aq ) C. H 2 S( g ), H 2 S( aq ) D. Li( s ), Pb( s ) E. H 2 ( g ), H 2 O( g ) 6. What is the free energy change, Δ G °, for the equilibrium between hydrogen iodide, hydrogen, and iodine at 453°C? K c = 0.020 2HI( g ) H 2 ( g ) + I 2 ( g ) A. 6.4 kJ B. 8.8 kJ C. 15 kJ D. 19 kJ E. 24 kJ 7. Which of the following is true for a system at equilibrium? A. Δ S ° sys = Δ S ° surr B. Δ S ° sys = - Δ S ° surr C. Δ S ° sys = Δ S ° surr = 0 D. Δ S ° univ > 0 E. None of these is a sufficient condition.
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Page 3 8. Calculate the solubility of zinc hydroxide, Zn(OH) 2 , in 1.00 M NaOH. K sp = 3.0 × 10 -16 for Zn(OH) 2 , K f = 3.0 × 10 15 for Zn(OH) 4 2- A. 0.60 M B. 0.52 M C. 0.37 M D. 0.32 M E. 0.24 M 9. Which, if any, of the following aqueous mixtures would be a buffer system? A. CH 3 COOH, NaH 2 PO 4 B. H 2 CO 3 , HCO 3 - C. H 2 PO 4 - , HCO 3 - D. HSO 4 - , HSO 3 - E. None of these will be a buffer solution. 10. Which of the following substances has the greatest solubility in water? A. Ba(IO 3 ) 2 , K sp = 1.5 × 10 -9 B. PbF 2 , K sp = 3.6 × 10 -8 C. SrSO 4 , K sp = 3.2 × 10 -7 D. CuCl, K sp = 1.9 × 10 -7 E. CdS, K sp = 1.0 × 10 -24 11. Which relationship or statement best describes Δ S ° for the following reaction? Pb( s ) + Cl 2 ( g ) PbCl 2 ( s ) A. Δ S ° 0 B. Δ S ° < 0 C. Δ S ° > 0 D. Δ S ° = Δ H °/ T E. More information is needed to make a reasonable prediction.
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12. A diprotic acid H 2 A has K a1 = 1 × 10 -4 and K a2 = 1 × 10 -8 . The corresponding base A 2- is titrated with aqueous HCl, both solutions being 0.1 mol L -1 . Which one of the following diagrams best represents the titration curve which will be seen? A.
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This note was uploaded on 06/07/2009 for the course CHEM 01c taught by Professor Schoeller during the Spring '09 term at UC Riverside.

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Midterm 2A - Midterm II - 150 points - 11/13/2007 - Version...

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