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Chemistry 103B Exam 2 answer key 2
Course: CHEM 103B, Spring 2007School: Arizona
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Chemistry 103B Exam 2 Answer Key Form B 1. (2) Which acid/<a href="/keyword/conjugate-base/" >conjugate base</a> pair would be best for making a buffer solution with pH = 3.00? (a) H3PO4/H2PO4(b) HCO3-/CO32(c) H2CO3/HCO3(d) HCN/CN(e) CH3OH/CH3O- Essentially from the d2l practice test. 2. (2) Lead(II) iodide, PbI2(s), has Ksp = 7.9e-9. What is the concentration of...
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Chemistry 103B Exam 2 Answer Key Form B 1. (2) Which acid/<a href="/keyword/conjugate-base/" >conjugate base</a> pair would be best for making a buffer solution with pH = 3.00? (a) H3PO4/H2PO4(b) HCO3-/CO32(c) H2CO3/HCO3(d) HCN/CN(e) CH3OH/CH3O- Essentially from the d2l practice test. 2. (2) Lead(II) iodide, PbI2(s), has Ksp = 7.9e-9. What is the concentration of iodide ion, I (aq), in a saturated solution of PbI2 ? (a) 1.3e-3 M (b) 2.5e-3 M (c) 2.0e-3 M (d) 6.3e-5 M (e) 1.3e-4 M From the study outline: " Computation of the equilibrium concentrations of ions in a saturated solution of an ionic compound." 3. (2) A water solution has a pH of 0.00. This means: (a) The solution is neutral. (b) the hydrogen ion concentration is 1.00 mol/L (c) There is no hydronium ion present. (d) There is no hydroxide ion present. (e) The hydrogen ion concentration is 0.00 mol/L. Definition of pH 4. (2) What is [H3O+] of a buffer solution that consistes of 0.10 M HF(aq) and 0.95 M NaF(aq)? (a) 6.8e-3 M (b) 7.6e-5 M (c) 7.2e-4 M (d) 1.5e-12 M (e) 1.3e-10 M From the study outline: "Be able to calculate the pH or hydrogen ion concentration of a buffer solution given the equilibrium concentrations of the weak acid, its <a href="/keyword/conjugate-base/" >conjugate base</a> and the appropriate Ka." 5. (2) Which of the 0.10 mol/L solutions will have a pH greater than 13.00? (a) KCH3(aq) (b) KH(aq) (c) KCH3O(aq) (d) KOH(aq) (e) Ca(OH)2(aq) From the study outline: "Be able to explain why a 0.10 mol/L solution of sulfuric acid has a lower pH than a 0.10 mol/L solution of hydrochloric acid." same principle here. 6. (2) Choose the strongest acid. (b) (c) (d) (e) (a) From the study outline: "Understand how the strength of an oxyacid depends upon molecular structure." 7. (2) ) A diprotic acid H2A has Ka1 = 4.0e-6 and Ka2 = 6.0e-10. In a 0.50 mol/L solution of this acid, what is [A2-]? (a) 6.0e-10 M (b) 4.0e-6 M (c) 6.3e-4 M (d) 4.5e-3 M (e) 1.4e-3 M From the study outline: "Be able to find the equilibrium concentrations of all species in a solution of a diprotic acid." 8. (2) A diprotic acid H2A has Ka1 = 4.0e-6 and Ka2 = 6.0e-10. In a 0.50 mol/L solution of this acid, what is [H3O+]? (a) 4.5e-3 M (b) 1.00 M (c) 0.50 M (d) 6.3e-4 M (e) 1.4e-3 M 9. (2) A phosphate buffer (H2PO4-/HPO42-) has a pH of 8.3. Which of the following will cause the pH to increase? (a) Adding a small amount of phosphoric acid (H3PO4) (b) Dissolving a (c) Adding a small amount small amount of NaH2PO4. of dilute hydrochloric acid. (d) Making the buffer more concentrated by removing some water by evaporation. (e) Adding a small amount of Na2HPO4. From the d2l practice test. 10. (2) Which of the 0.10 mol/L solutions will have a pH less than 1.00? (a) H2SO4(aq) (b) HCl(aq) (c) HF(aq) (d) HNO3(aq) (e) HNO3(aq) From the study outline: Be able to explain why a 0.10 mol/L solution of sulfuric acid has a lower pH than a 0.10 mol/L solution of hydrochloric acid. 11. (2) <a href="/keyword/potassium-hydroxide/" >potassium hydroxide</a> (KOH) is an ionic compound and a strong base. A water solution of KOH has a pH of 12.83. Find the mol/L concentration of potassium ion in this solution (a) 1.0e-7 M (b) 1.17 M (c) 0.068 M (d) 1.5e-13 M (e) 12.83 M From the study outline: "Know that ionic compounds (metal-nonmetal) are always 100% ionized (dissociated into ions) in solution." 12. (2) <a href="/keyword/potassium-hydroxide/" >potassium hydroxide</a> (KOH) is an ionic compound and a strong base. A water solution of KOH has a pH of 12.83. Find the mol/L concentration of hydroxide ion this solution (a) 1.5e-13 M (b) 3.7e-12 M (c) 1.17 M (d) 12.83 M (e) 0.068 M 13. (2) <a href="/keyword/potassium-hydroxide/" >potassium hydroxide</a> (KOH) is an ionic compound and a strong base. A water solution of KOH has a pH of 12.83. Find the mol/L concentration of hydronium ion in this solution (a) 1.5e-13 M (b) 0.068 M (c) 1.17 M (d) 3.7e-12 M (e) none of these 14. (2) A solution is prepared by dissolving 0.10 mol of potassium acetate (KCH3CO2) in 1.0 L of pure water. Which statement about the solution is correct? (a) The pH is greater than 7.0 (b) The pH is less than 7.0 (c) The solution is neutral. (d) The concentrations of potassium ion and acetate ion are identical. (e) The concentration of acetate ion will be greater than the concentration of potassium ion. From the d2l practice exam. 15. (2) Which acid has the strongest <a href="/keyword/conjugate-base/" >conjugate base</a> ? (a) HCl (b) HF (c) HCN (d) HCH3CO2 (e) HOCl The strongest base will be the conjugate of the weakest acid. From the study outline: "Understand and be able to explain the meaning of all regions of the acid-<a href="/keyword/conjugate-base/" >conjugate base</a> table shown in lecture and on problem set 4 and 5." 16. (2) This question involves interpretation of the acid-base table attached to this exam. Which substance is a weaker proton donor than water? (a) HNO3 (b) HOCl (c) H2S (d) H2 (e) HCO3- From the study outline: "Understand and be able to explain the meaning of all regions of the acid-<a href="/keyword/conjugate-base/" >conjugate base</a> table shown in lecture and on problem set 4 and 5." 17. (2) Choose the weakest proton donor. (a) (b) (c) (d) (e) From the study outline: "Predicting the qualitative strength of an acid by examination of its structural formula." 18. (2) This question involves interpretation of the acid-base table attached to this exam. Which substance is a weaker proton acceptor than water? (a) CN(b) H(c) Cl(d) OCl(e) CO32- From the study outline: "Understand and be able to explain the meaning of all regions of the acid-<a href="/keyword/conjugate-base/" >conjugate base</a> table shown in lecture and on problem set 4 and 5." 19. (2) What is the value of Kb for the <a href="/keyword/conjugate-base/" >conjugate base</a> of formic acid (HCO2H). Ka = 2.1 x 10-4 (a) 4.8e-11 (b) 2.1e-4 (c) 6.9e-6 (d) 2.1e-18 (e) -2.1e-4 From the study outline: "Be able to calculate Kb for the <a href="/keyword/conjugate-base/" >conjugate base</a> of a weak acid given the Ka value of the acid." The next five questions involve a strong acid HClO3(aq). 20. (2) What is the pH of a 0.20 mol/L solution of HClO 3? (a) 0.30 (b) 0.70 (c) -0.20 (d) 0.080 (e) -0.69 Since it is a strong acid, it is 100% dissociated. The concentration of hydrogen ion is 0.20 mol/L. From the study outline: "Calculation of the equilibrium concentrations of all solution species in problems involving strong acids or bases. This includes finding pH." 21. (2) What is the pH of a 0.20 mol/L solution of KClO 3(aq)? (a) 0.69 (b) 0.30 (c) -0.20 (d) -0.69 (e) 7.00 ClO3- is the <a href="/keyword/conjugate-base/" >conjugate base</a> of a strong acid, and therefore not a base. The solution is neutral. The potassium ion is just a "spectator ion." From the study outline: "Know that ionic compounds (metal-nonmetal) are always 100% ionized (dissociated into ions) in solution." And "Calculation of the equilibrium concentrations of all solution species in problems involving strong acids or bases. This includes finding pH." 22. (2) What is [OH-] of a 0.20 mol/L solution of KClO3(aq)? (a) 7.0e-1 M (b) 1.0e-14 M (c) 0.69 M (d) 1.0e-7 M (e) 0.20 M 23. (2) What is the pOH of a 0.20 mol/L solution of HClO 3(aq)? (a) 7.00 (b) 13.30 (c) 0.20 (d) 0.70 (e) none of these 24. (2) What is the pOH of a 0.20 mol/L solution of KClO 3(aq)? (a) 13.30 (b) 7.00 (c) 14.00 (d) 0.00 (e) 0.20 25. (2) What is [H3O+] for a solution that has pOH = 5.640? (a) 8.360 M (b) 2.34e-4 M (c) 2.29e-6 M (d) 4.37e-9 M (e) 4.27e-11 M Definitions of pOH and pH.
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