chapter16practice

chapter16practice - Final Examination Spring 2011.

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Unformatted text preview: Final Examination Spring 2011. Name___________________________________ R.Lopez de la Vega Bubble in the form number in the section entitled Grade or Educ in the scantron. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which is the net ionic equation for the neutralization of a weak acid with a strong base? A) H3O+(aq) + OH-(aq) ⇌ 2 H2O(l) B) HF(aq) + OH-(aq) ⇌ H2O(l) + F-(aq) 1) C) HF(aq) + NaOH(aq) ⇌ H2O(l) + NaF(aq) D) HCl(aq) + NaOH(aq) ⇌ H2O(l) + NaCl(aq) 2) Which is the net ionic equation for the neutralization reaction of a strong acid with a weak base? A) HCl(aq) + NaOH(aq) ⇌ H2O(l) + NaCl(aq) B) H3O+(aq) + OH-(aq) ⇌ 2 H2O(l) C) H3O+(aq) + NH3(aq) ⇌ NH4+(aq) + H2O(l) 2) D) HCl(aq) + NH3(aq) ⇌ NH4Cl(aq) 3) What is the hydronium ion concentration in a solution prepared by mixing 50.00 mL of 0.10 M HCN with 50.00 mL of 0.050 M NaCN? Assume that the volumes of the solutions are additive and that Ka = 4.9 × 10-10 for HCN. C) 2.4 × 10-10 M A) 4.9 × 10-10 M B) 7.0 × 10-6 M D) 9.8 × 10-10 M 3) 4) What is the common ion in a solution prepared by mixing 0.10 M NaCH 3CO 2 with 0.10 M CH3CO 2H? A) H3O+ B) H2O C) CH3CO 2H D) CH3CO 2- 4) 5) What is the pH of the resulting solution if 30.00 mL of 0.10 M acetic acid is added to 10.00 mL of 0.10 M NaOH? Assume that the volumes of the solutions are additive. Ka = 1.8 × 10-5 for CH3CO 2H. A) 5.05 B) 8.95 C) 4.44 D) 9.56 5) 6) Formic acid (HCO2H, Ka = 1.8 × 10-4) is the principal component in the venom of stinging ants. What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 29.80 mL of 0.0567 M NaOH to reach the equivalence point? A) 0.0567 M B) 0.0476 M C) 0.0676 M D) 0.0134 M 6) 7) What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 30.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive. Ka = 1.8 × 10-5 for CH3CO 2H. A) 8.72 B) 7.00 C) 5.28 D) 10.02 7) 1 8) What is not a correct expression for the weak acid HA? A) pKa = logKa B) Ka = [H3O+][A-]/[HA] C) pKa = pH - log{[A -]/[HA]} D) pKa = 14 - p Kb 8) 9) Which of the following titrations result in a basic solution at the equivalence point? A) HOCl titrated with NaOH B) HI titrated with NaCH3CO 2 C) HBr titrated with KOH D) Pb(NO3)2 titrated with NaI 9) 10) A buffer solution is prepared by dissolving 27.22 g of KH2PO4 and 3.37 g of KOH in enough water to make 0.100 L of solution. What is the pH of the H2PO4-/HPO42- buffer if the Ka2 = 6.2 × 10-8? A) 6.84 B) 7.84 C) 7.21 10) D) 7.00 11) Sodium hypochlorite, NaOCl, is the active ingredient in household bleach. What is the concentration of hypochorite ion if 20.00 mL of bleach requires 28.30 mL of 0.500 M HCl to reach the equivalence point? A) 0.708 M B) 0.208 M C) 0.353 M D) 1.21 M 11) 12) What is the solubility product constant, Ksp, for the slightly soluble salt Fe(OH)2? The equation of interest is Fe(OH) 2(s) + H2O(l) ⇌ Fe2+(aq) + 2 OH-(aq). 12) A) Ksp = 1/{[Fe2+][OH-]2} B) Ksp = {[Fe2+][OH-]2}/[Fe(OH)2] C) Ksp = [Fe2+][OH-]2 D) Ksp = {[Fe2+][OH-]2}/{[Fe(OH)2][H 2O]} 13) Calculate the solubility (in g/L) of silver carbonate in water at 25°C if the Ksp for Ag2CO 3 is 8.4 × 10-12. A) 8.0 × 10-4 g/L B) 5.6 × 10-2 g/L C) 4.4 × 10-2 g/L D) 3.5 × 10-2 g/L 13) 14) What is the most soluble salt of the following set? A) Sn(OH)2 with Ksp = 1.6 × 10-19 B) Fe(OH) 3 with Ksp = 2.6 × 10-39 C) Al(OH)3 with Ksp = 1.9 × 10-33 D) AgCN with Ksp = 6.0 × 10-17 14) 15) Calculate the molar solubility of thallium chloride in 0.30 M NaCl at 25°C. Ksp for TlCl is 1.7 × 10-4. A) 1.3 × 10-2 M B) 5.1 × 10-5 M C) 7.1 × 10-3 M D) 5.7 × 10-4 M 15) 16) 0.10 M potassium chromate is slowly added to a solution containing 0.20 M AgNO 3 and 0.20 M Ba(NO 3)2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? Ksp for 16) Ag2CrO4 and BaCrO 4 are 1.1 × 10-12 and 1.2 × 10-10, respectively. A) 3.2 × 10-4 M B) 4.3 × 10-2 M C) 6.5 × 10-5 M 2 D) 1.3 × 10-4 M 17) Precipitation of an ionic compound will occur upon mixing of desired reagents if the initial ion product is ________. A) equal to the Ksp B) greater than the Ksp C) equal to the pKsp D) less than the Ksp 17) Use the graphs below to answer the following questions. 18) What is the characteristic pH-titration curve for the titration of a weak acid by a strong base? A) A B) B C) C D) D 18) 19) What is the characteristic pH-titrant curve for the titration of a strong base by a strong acid? A) A B) B C) C D) D 19) The following plot shows two titration curves, each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. 20) Which point a-d represents the equivalence point for the titration of a strong acid? A) point a B) point b C) point c D) point d 20) 21) Which point a-d represents the equivalence point for the titration of a weak acid? A) point a B) point b C) point c D) point d 21) 22) At which point a-d is the pKa of the acid equal to the pH? A) point a B) point b C) point c 22) 3 D) point d 23) Which points a-d represent the half-equivalence point and the equivalence point, respectively, for the titration of a weak acid? A) points a and b B) points b and d C) points c and d D) points a and c 23) 24) Which point a-d represents a buffer region? A) point a B) point b 24) C) point c D) point d Use the graphs below to answer the following questions. 25) What is the characteristic pH-titrant curve for the titration of a strong acid by a strong base? A) A B) B C) C D) D 25) 26) What is the hydronium ion concentration in a solution prepared by mixing 50.00 mL of 0.10 M HCN with 50.00 mL of 0.010 M NaCN? Assume that the volumes of the solutions are additive and that Ka = 4.9 × 10-10 for HCN. A) 7.0 × 10-6 M B) 4.9 × 10-9 M 26) C) 4.9 × 10-10 M D) 4.9 × 10-11 M 27) What volume of 0.500 M HNO 3 is needed to titrate 60.00 mL of 0.500 M Ca(OH)2 to the equivalence point? A) 30.0 mL B) 60.0 mL C) 7.50 mL D) 120. mL 27) 28) What is the [CH3CO 2-]/[CH3CO 2H] ratio necessary to make a buffer solution with a pH of 4. 34? Ka = 1.8 × 10-5 for CH 3CO 2H. 28) A) 0.91:1 B) 2.5:1 C) 1.09:1 D) 0.39:1 29) Formic acid (HCO2H, Ka = 1.8 × 10-4) is the principal component in the venom of stinging ants. What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 49.80 mL of 0.0567 M NaOH to reach the equivalence point? A) 0.0567 M B) 0.0134 M C) 0.113 M D) 0.0285 M 29) 30) 0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO3 and 0.50 M Ba(NO 3)2. What is the Ag+ concentration whenBaCrO4 just starts to precipitate? The Ksp 30) for Ag2CrO4 and BaCrO 4 are 1.1 × 10-12 and 1.2 × 10-10, respectively. A) 6.5 × 10-5 M B) 1.1 × 10-2 M C) 3.2 × 10-4 M 4 D) 1.3 × 10-4 M Answer Key Testname: UNTITLED1 1) B 2) C 3) D 4) D 5) C 6) C 7) A 8) A 9) A 10) A 11) A 12) C 13) D 14) A 15) D 16) B 17) B 18) A 19) C 20) D 21) C 22) A 23) D 24) A 25) B 26) B 27) D 28) D 29) C 30) B 5 ...
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This note was uploaded on 12/17/2011 for the course CHM 1046 taught by Professor Staff during the Fall '08 term at FIU.

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