CHM 115 CHM115 Practice Exam 2 Answers (Grand Canyon University)

CHM 115 CHM115 Practice Exam 2 Answers (Grand Canyon University)

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CHM 115 Practice Exam 2 Answers (Grand Canyon University)

  1. How many grams of NaOH would it take to neutralize 76 ml of 1.5 M H2SO4?  
  2. The following question refers to the following system: A 1.0-liter solution contains 0.73 M HF and 0.52 M NaF. What is the pH of this solution? (Ka  for HF is 7.2  10–4)

  3. Which of the following statements correctly describe a typical titration curve for the titration of a strong acid by a strong base?

  4. A 10.5-mL sample of diprotic acid is titrated to a phenolphthalein endpoint with 20. mL of 1.0 M NaOH. What is the molarity of the acid?

  5. Choose the expression that gives the molar concentration of a HCl solution if 24.3 mL of a 0.105 M NaOH solution is required to titrate 30 mL of the acid.

  6. Calculate the pH of a solution that is 2.00 M HF, 1.00 MNaOH, and 0.439 MNaF. (Ka = 7.2 10–4)

  7. The pH of a solution containing 2.0 mole HNO2 and 2.0 mole NaNO2 in 1.0 L of solution will   notchange by:

  8. Which among the following pairs is inefficient as buffer pair?

  9. Which of the following will end up as a buffer solution when equal volumes of the two solutions are mixed?

  10. What is the pH of a solution containing 0.400 M HONH2 and 0.250 M HONH3Cl?

    (Kb for HONH2 is 1.1 x 10-8.)

  11. A 150.0 mL buffer solution containing 0.100 M hydrocyanic acid (HCN, Ka = 6.2 x 10-10) and 0.100 M sodium cyanide (NaCN) has 30.0 mL of 0.120 M NaOH added to it. What is the pH of the solution after the NaOH has been added?

  12. The Ka of acetic acid is 1.76 × 10-5. The pH of a buffer prepared by combining 50.0 mL of 1.00 M potassium acetate and 50.0 mL of 1.00 M acetic acid is __________.

  13. If 200.0 mL of 0.200 M HCl is titrated with 0.050 M NaOH. What is the pH after the addition of 100. mL of the NaOH solution?

  14. Consider a solution prepared by dissolving 0.35 mol of CH3NH3+Cl- (methylamine hydrochloride) in 1.00 L of 1.1 M CH3NH2 (methylamine). If 10 mL of 0.10 M HCl is added to this buffer solution, the pH of the solution will ________ slightly because the HCl reacts with the _________ present in the solution to produce a _______.

  15. The following titration curve shows:

  16. An initial pH of 4.0 and an equivalence point at pH = 9.1 corresponds to a titration curve for a

  17. What is the pH after 10 ml of 0.1 M KOH is added to 20 ml of 0.2 M HClO?

  18. Calculate the pH of a solution that is 1.00 M HF, 1.00 M HCl, and 1.439 MNaF. (Ka = 7.2 10–4)

  19. Calculate the pH of a solution that is 1.00 M HF, 2.00 M HCl, and 1.439 MNaF. (Ka = 7.2 10–4)

  20. For which type of titration will the pH be acidic at the equivalence point?

  21. The solubility product constant (Ksp) of Li3PO4 is 3.2 × 10-9. What is the molar solubility of Li3PO4 in water?

  22. What is the molar solubility of PbI2 (Ksp = 7.1 × 10-9) in 0.10 M Pb(NO3)2?

  23. Which of the following solid salts is more soluble in 1.0 M H+ than in pure water?

  24. Which of the following salts, each of which has a solubility product constant (Ksp) equal to 1.0 × 10-6, has the lowest molar solubility?

  25. Which of the following salts is least soluble in pure water?

  26. The solubility of which compound will not be affected by the pH of the solution?

  27. The molar solubility of MgF2 is 1.17 x 10-3 M. What is the value of Ksp for MgF2?

  28. Which of the following when dissolved in water has the highest concentration of calcium ions?

  29. For each solution indicate the effect of the change on solubility.

  30. Which of the following is the correct Ksp expression for copper (I) sulfide.

  31. The solubility product constant (Ksp) for MgF2 is 6.4 × 10-9. How many grams of MgF2 will dissolve in 150 mL of H2O at 25°C?

  32. If S° for the following reaction is -149 J/mol.  Calculate S° for Fe(s).

    2Fe(s) + 3Cl2 (g) 2FeCl3(s) 

  33. For the reaction A + B C + D, H° = +40 kJ and S° = +50 J/K. Therefore, the reaction under standard conditions is

  34. What is the value of ΔG° (in kJ/mol) for this reaction at 25°C?
  35. Which of the following reactions would have a positive value for ΔS°?

  36. Calculate ΔG0 (kJ/mol) for the reaction using the listed [ΔG0f values]:

  37. A concentration cell is constructed using two Zn electrodes with Zn2+ concentrations of 1.0 M and 1.00 10–9 M in the two half-cells. The reduction potential of Zn2+ is –0.76 V. Calculate the potential of the cell at 25°C.


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