1. What is the molar concentration of a solution prepared by dissolving 3.00 g of K₃PO₄ in enough water to make 350. mL of solution? 

1. 0.0101 M
2. 0.0404 M
3. 0.323 M
4. 0.202 M
5. none of the above

2. 80.0 grams of K₂SO₄ is dissolved in 3.20 x 10² grams of water. Find the percent concentration by mass.

     

      A. 15.0%         B. 20.0%        C. 25.0%         D. 30.0%         E. 256%

3. Calculate the grams of alcohol, C₂H₅OH, in 440 grams of a 23.0% solution.

1. 5.23 g
2. 19.1 g
3. 23.0 g
4. 339 g
5. 101 g

4. What are the units of molality? 

1. mol solute/kg solvent
2. mol solute/L solution
3. g solvent/kg solute
4. L solvent/L solution
5. g solution/mL solution

5. Choose the pair of substances that are most likely to form a homogeneous solution.

A.    NH₃ and CH₃OH

B.     H₂O and C₁₄H₁₆

C.     C₃H₈ and C₂H₅OH

D.    LiF and C₆H₁₄

E.     all of the above

6. A Brønsted–Lowry acid is defined as a(n)...

            A. proton acceptor

            B. electron donor

            C. proton donor

            D. electron pair acceptor

            E. electron pair donor

7. Which of the following is not capable of acting like a Brønsted–Lowry base?

           

            A. H₂O(l)        B. NH₄⁺ ion    C. Cl^– ion        D. NO₃^-(aq)     E. H₂PO₄^–(aq)

8. What color change occurs when the endpoint of a titration is reached if the indicator used is phenolphthalein?

1. colorless to pink
2. clear to orange
3. pink to blue
4. purple to yellow
5. no change

9. 75.0 mL of water is added to 12.9 mL of 0.250 M KMnO₄. What is the concentration of the diluted solution?

A. 1.70 M       

B. 1.45 M       

C. 0.0581 M      

D. 0.0430 M   

E. 0.0367 M

10. Which of the following solutions is most acidic?

1. [H⁺] = 1 x 10^-3
2. [OH^-] = 1 x 10^-2
3. [OH^-] = 1 x 10^-13
4. pH = 10
5. pH = 8

11. Identify the conjugate acid base pairs in the reaction

                  H₂SO₄ + HNO₃ → H₂NO₃⁺ + HSO₄^–

         A. H₂SO₄/HSO₄^– and H₂NO₃⁺/HNO₃

         B. H₂SO₄/HNO₃ and H₂NO₃⁺/HSO₄^–

         C. HNO₃/HSO₄^– and H₂SO₄/H₂NO₃⁺

         D. HNO₃/NO₃^– and HSO₄^–/SO₄^2–

         E. HNO₃/H₂SO₄ and H₂NO₃⁺/HSO₄^–

12.  Name all the types of intermolecular forces for each molecule: (9 points)

A.    CH₃NH₂         

       H-bond, Dipole-Dipole, Induced Dipole

B.     SO₂                 

                        Dipole-Dipole, Induced Dipole

            C.   CO₂   

                  Induced Dipole

     

13.  In propane, the intermolecular interaction is weaker than that in propel alcohol.  Predict which liquid has the higher value for each of the following (propane or propel alchohol): (8 points)

A.    vapor pressure = propane                              

B.     viscosity = propel                               

C.     boiling point = propel

D.    surface tension = propel

14. A mixture of gases at 760 torr contains 45.0% nitrogen, 15.0% oxygen and 40% carbon dioxide, by volume.  What is the partial pressure of each gas in torr.  (4 points)

342 torr N₂, 114 torr O₂, 304 torr CO₂

15. Fill in the table below (6 points)

Conjugate acid	Conjugate base
HSO4-	SO42-
HCl	Cl-
H2O	OH-
HC2H5O	C2H5O-
NH4+	NH3
HNO3	NO3-

16.  What is the total heat flow if 22.2 grams of water at 82.2°C is heated to become steam at 115.9°C? The specific heat of liquid water is 4.18 J/g • °C; the specific heat of steam is 2.0 J/g•°C. The heat of vaporization of water is 2.26 kJ/g, and the boiling point of water is 100°C. (8 points)

                        52.6 kJ

17. A solution is made by dissolving 1.25 grams of NaOH, a strong base, in water to produce 2.0 liters of solution.  Calculate the following. (8 points)

a.        [H⁺] = _____6.3 x 10^-13_M______

b.       [OH^-] = ___0.016 M________

c.        pH = ____12.20_________

d.       pOH = ___1.80___________

18. A hydrochloric acid (HCl) solution is standardized by titrating against a calcium hydroxide solution (Ca(OH)₂).  23.4 mL of the base is used to neutralize 0.157 g HCl. Calculate the molarity of the base solution. (8 points)

0.0920M

19. When 15.2 mL of a 0.415 M iron(III) chloride solution are added to 25.00 mL of a 0.245 M solution of potassium phosphate, a precipitate is observed. 
1. Write the balanced molecular equation and the net ionic equation (4 points)

                                                FeCl₃(aq) + K₃PO₄(aq) → 3KCl(aq) + FePO₄(s)

                  Fe³⁺(aq) + PO₄^3-(aq) → FePO₄(s)

2. Determine the concentration of all ions in solution and calculate the mass of the precipitate formed.  (12 points)

[PO₄^3-] = 0

                        [Fe³⁺] = 0.00448 M

                        [Cl^-] = 0.471 M

                        [K⁺] = 0.457 M

                       

                        0.924g FePO₄