Exam 4 Review
Exam 4 Review Chemistry 101
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This 5 page Study Guide was uploaded by Becca LeBoeuf on Monday April 18, 2016. The Study Guide belongs to Chemistry 101 at University of Wisconsin - Oshkosh taught by George Vater Olsen in Spring 2016. Since its upload, it has received 23 views. For similar materials see General, Organic, Biological Chemistry in Chemistry at University of Wisconsin - Oshkosh.
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Date Created: 04/18/16
Exam 4 Review 1. How many liters of a 1.50 M NaOH solution can be prepared from 40.0 grams of NaOH FW = 40.0 g/mole? a. 1.33 liters. b. 3.00 liters. c. 0.133 liters. d. 0.667 liters e. 0.750 liters. f. None of the above. 2. If the dosage rate for medication is 1.75 mg/kg and you have a 0.0800% mass/volume solution of that medication, how many milliliters should you give to a 230.00 lb patient? a. 218 ml. b. 229 ml. c. 318 ml. d. 350 ml. e. None of the above. 3. If you make a solution that has 12.0 ml of water, 14.0 ml of methanol, and 10.0 ml of ethanol, which of the following statements is true? a. The solvent is water. b. The solvent is methanol. c. The solvent is ethanol. d. The solutions will not be a homogeneous mixture. e. Solution components can be separated by standard filtration. 4. If the sodium ion concentration in blood is reported as 0.14 N, how many grams of sodium ion are there in each liter of blood? a. 3.2 g. b. 6.1 x 10^3 g. c. 6.4 g. d. 1.4 x 101 g. e. 1.5 g. f. None of the above. 5. What is the number of grams of sodium nitrate FW= 85 g/mole required to prepare 75.0 ml of a 4.50% (wt/vol) solution? a. 1.25. b. 3.38. c. 4.50. d. 5.65. e. 7.76. f. None of the above. 6. Determine the concentration of an H3PO4 solution if it takes 36.5 ml of 0.120 M Ca(OH)2 to neutralize 14.3 ml of the acid. a. 0.047 M. b. 0.120 M. c. 0.20 M. d. 0.31 M. e. 0.46 M. 7. What is the molarity of a 0.20 N iron(II) chloride solution? a. 25.2 M. b. 0.80 M. c. 0.40 M. d. 0.20 M. e. 0.10 M. f. None of the above. 8. What is the volume of 6.00 M Na3PO4 necessary to prepare 24.0 ml of a 1.50 M solution of sodium ions (Na3PO4 MW = 164 g/mole)? a. 60.0 ml. b. 18.0 ml. c. 9.00 ml. d. 6.00 ml. e. 2.00 ml. 9. What is the pH of a buffer solution which is 1.0 M with respect to sodium acetate and 0.10 M with respect to acetic acid? a. 1.00. b. 2.74. c. 3.74. d. 4.74. e. 5.74. 10. Determine the concentration of an H3PO4 solution if it takes 36.5 ml of 0.120 M Ca(OH)2 to neutralize 14.3 ml of the acid. a. 0.047 M. b. 0.120 M. c. 0.20 M. d. 0.31 M. e. 0.46 M. 11. A 0.92 % m/v solution of sodium chloride FW 58.45 g/mole would have the same osmolarity as which of the following? a. 0.315 M solution of magnesium chloride. b. 0.157 M solution of magnesium sulfate. c. 0.315 M lactic acid solution. d. 0.157 M sucrose solution. e. None of the above. 12. Which of the following 0.100 M aqueous solutions would be expected to have the great boiling point? a. Acetic acid Ka = 1.8 x 10^5. b. Lactic acid Ka = 1.4 x 10^4. c. Formic acid Ka = 1.8 x 10^4. d. Propanoic acid Ka = 1.3 x 10^5. e. Hydrofluoric acid Ka = 3.5 x 10^4. 13. All of the following solution pairs would function as a buffer except for? a. HF and KF. b. HNOs and NaNO3. c. HN3 and NaN3. d. NaHCO3 and H2CO3. e. KC2H3O2 and HC2H3O2. 14. Given the KSP 3.72 x 10^19 for iron(II)sulfide, MW = 87.92, how many grams should be dissolved to make 10.0 liters of a saturated solution? a. 1.07 x 10^7. b. 5.36 x 10^7. c. 2.94 x 10^15. d. 4.82 x 10^6. e. None of the above. 15. Which one of the following 0.1 M solutions will have the lowest pH? a. Acetic acid Ka = 1.8 x 10^5. b. Lactic acid Ka = 1.4 x 10^4. c. Formic acid Ka = 1.8 x 10^4. d. Propanoic acid Ka = 1.3 x 10^5. e. Hydrofluoric acid Ka = 3.5 x 10^4. 16. All of the following will raise the pH of water when dissolved in it except for: a. AgNO3. b. NaCN. c. NH3. d. AgOH. e. NaNO2. 17. Which of the following statements is true about a buffer solution which is 1.0 M with respect to sodium acetate and 0.10 M with respect to acetic acid? a. It has the greatest buffering capacity towards added base. b. It has the greatest buffering capacity towards added acid. c. It has equal buffering capacity towards added acid or base. d. It is not a buffer system. e. None of the above. 18. The pKa of lactic acid (HC3H5O3) is 3.85. A bugger that has a lactate ion (C3H5O3 ^1) to lactic acid ration of 1 to 10 had a pH of: a. 2.00. b. 2.85. c. 3.85. d. 4.85. e. 5.85. f. None of the above. 19. 20. What is the [H+] of a 0.11 M solution of nitrous acid HNO2, Ka = 4.6 x 10^4? a. 2.36 x 10^3 M. b. 7.11 x 10^3 M. c. 4.60 x 10^4 M. d. 5.06 x 10^5 M. e. None of the above. 21. What are the respective pH and pOH of a 5.0 x 10^3 M aqueous H2SO4 solution? a. 1.30 and 12.70. b. 2.30 and 11.70. c. 2.00 and 12.00. d. 1.00 and 13.00. e. None of the above. 22. What are the respective [OH^1] and [H^1+] of a 5.0 x 10^3 M aqueous Ba(OH)2 solution? a. 5.0 x 10^2 M and 2.0 x 10^13 M. b. 5.0 x 10^3 M and 2.0 x 10^12 M. c. 1.0 x 10^2 M and 1.0 x 10^12 M. d. 1.0 x 10^1 M and 1.0 x 10^13 M. e. None of the above. 23. By Le Chatelier’s principle, for the reaction in a closed container at equilibrium: C3H8 (g) + 5 O2 (g) ← → 3 CO2 (g) + 4 H2O (l) What is the effect of increasing the pressure on the system? a. No change. b. Shift it right. c. Shift it left. d. Increase the reaction rate. e. None of the above. 24. When the following balanced redox reaction is at equilibrium, heating the reaction will cause which of the following to reestablish equilibrium: 2 NO (g) + Cl2 (g) ← → NOCl (g) 77.2 KJ. a. Shift left. b. Shift right. c. No shift. 25. For the following reaction: CH4 (g) + 2 H2S (g) ← → CS2 (g) + 4 H2 (g) The equilibrium expression would be: a. K = [CH4][H2S] / [CS2][H2]. b. K = [CS2][H2]^4 / [CH1][H2S]^2. c. K = [CS2] 4[H2]^4 / [CH4] 2[H2S]^2. d. K = [CH4] 2[H2S]^2 / [CS2][H2]^4. e. None of the above. 26. Use the following reaction equation to determine which of the following statement is true: H2CO3 + OH^1 ← → HCO3^1 + H2O a. HCO3^1 is the conjugate acid of H2CO3. b. H2O is acting as a base. c. H2O and HCO3^1 are both acting as bases. d. H2CO3 is the conjugate acid of HCO3^1. e. None of the above.
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