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AP CHEMISTRY REVIEW:

AP CHEMISTRY REVIEW:. SOLUTIONS. How many mL o f 10.0 M HCl are needed to prepare 500. mL of 2.00 M HCl?. A. 1.00 mL B. 10.0 mL C. 20.0 mL D. 100. mL E. 200. mL ANSWER: d.

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AP CHEMISTRY REVIEW:

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  1. AP CHEMISTRY REVIEW: SOLUTIONS

  2. How many mL o f 10.0 M HCl are needed to prepare 500. mL of 2.00 M HCl? • A. 1.00 mL • B. 10.0 mL • C. 20.0 mL • D. 100. mL • E. 200. mL • ANSWER: d

  3. A solution is prepared by adding 16 g CH3OH (molar mass 32 g) to 90. g of H2O (molar mass 18.g). The mol fraction of CH3OH in this solution is closest to which of the following? • A. 0.10 • B. 0.20 • C. 0.30 • D. 0.40 • E. 0.60 • ANSWER: A

  4. Which of the following measures of concentrations changes with temperature • A. mass percentage • B. mol fraction • C. molarity • D. molality • E. parts per million by mass • Answer: C

  5. A sample of 10.0 mol of butyric acid, HC4H7O2, a weak acid, is dissolved in 1000. g of water to make a 10.0 molal solution. Which of the following would be the best method to determine the molarity of the solution. • A. Titration of the solution with a standard acid • B. measurement of the pH with a pH meter • C. determination of the freezing point of the solution • D. measurement of the total volume of the solution • E. measurement of the electrical conductivity of the solution • Answer: D

  6. The nonvolatile compound ethylene glycol, C2H6O2, forms nearly ideal solutions with water. What is the vapor pressure of a solution made from 1.00 mole of C2H6O2 and 9.00 moles of H2O if the vapor pressure of pure water at the same temperature is 25.0 mm Hg. • A. 2.50 mm Hg • B. 7.50 mm Hg • C. 12.5 mm Hg • D. 22.5 mm Hg • E. 27.5 mm Hg • Answer: d

  7. A 360. mg sample of aspirin, C9H8O4, (molar mass 180.g) is dissolved in enough water to make 200. mL of solution. What is the molarity of aspirin in a 50. mL sample of this solution • A. 0.0800 M • B. 0.0400 M • C. 0.0200 M • D. 0.0100 M • E. 0.00250 M • Answer: D

  8. The molality of glucose in a 1.0 molar glucose solution can be obtained by using which of the following? • Volume of the solution • Temperature of the solution • Solubility of glucose in water • Density of the solution ANSWER: d

  9. When 70. mL of 3.0 molar Na2CO3 is added to 30. mL of 1.0 molar NaHCO3 the resulting concentration of Na+ is • 2.0 M • 2.4 M • 4.0 M • 4.5 M • 7.0 M ANSWER: D

  10. Which of the following aqueous solutions has the highest boiling point? • 0.10 M potassium sulfate, K2SO4 • 0.10 M hydrochloric acid, HCl • 0.10 M ammonium nitrate, NH4NO3 • 0.10 M magnesium sulfate MgSO4 • 0.20 M sucrose C12H22O11 ANSWER: A

  11. what additional information is necessary to calculate the molarity of the solution? I. The density of the water II. The density of the solution III. The molar mass of sucrose • I only • II only • III only • I and III • II and III I SEEM TO HAVE LEFT OFF PART OF THE PROBLEM  ANSWER IS PROBABLY B BECAUSE YOU WOULD HAVE TO HAVE THE MOLAR MASS OF SUCROSE TO CHANGE GRAMS TO MOLES AND THE DENSITY OF THE SOLUTION TO FIND LITERS

  12. If the temperature of an aqueous solution of NaCl • is increased from 20 C to 90 C, which of the following • statements is true? • The density of the solution remains unchanged • The molarity of the solution remains unchanged • The molality of the solution remains unchanged • The mole fraction of the solute decreases • The mole fraction of the solute increases ANSWER: C

  13. 7. What is the molality of a solution of phosphoric acid, H3PO4, that contains 24.5 g of phosphoric acid (molar mass 98.0g) in 100. g of H2O • 0.245 m • 2.50 m • 4.00 m • 25.0 m • 40.0 m ANSWER: B

  14. The freezing point and electrical conductivities of three aqueous solutions are given below: Explain the relationship between the freezing point and electrical conductivity for each of the solutions above. Account for the differences in the freezing points among the three solutions. SEE FREE RESPONSE #1 ON SHEET

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