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

            A. 5.23 g         B. 19.1 g         C. 23.0 g         D. 339 g         E. 101 g

2. You are to compare the intermolecular forces in ethanol (CH₃CH₂OH) with those in ethane, C₂H₆, in which all carbons are in a continuous chain. Which of the following statements is true?

A. The principal intermolecular forces in ethanol are induced dipole forces; in

ethane, hydrogen bonds

B. Hydrogen bonding is present in ethanol, but not in ethane

C. Hydrogen bonding is present in both compounds

D. Both compounds exhibit dipole-dipole forces

E. Induced dipole forces are present in neither compound

3. 80.0 grams of potassium sulfate is dissolved in 3.20 x 10² grams of water. Find

      the percentage concentration.

     

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

4. Choose the pair of substances that are most likely to form a homogeneous solution.
1. NH₃ and CH₃OH
2. H₂O and Hg
3. C₃H₈ and C₂H₅OH
4. LiF and C₆H₁₄
5. all of the above

5. 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

6. Which of the following solutions is most acidic?

                                    A. [H⁺] = 1 x 10^–3

                                    B. [OH^-] = 1 x 10^–2

                                    C. [OH^–] = 1 x 10^–13

                                    D. pH = 12

      E. pOH = 2

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. 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^–

9.      Name the types of intermolecular forces for each molecule: (8 points)

A.    CH₃NH₂                     

                        Hydrogen bond, dipole, induced dipole

B.     SO₂                 

                        Dipole, induced dipole

            C.   CO₂   

                  induced

10.  In propane, the intermolecular attraction is less than that in propel alcohol.  Predict which liquid has the higher value for each of the following: (8 points)

A.    vapor pressure = propane                              

B.     viscosity = propel                                                       

C.     boiling point = propel

D.    surface tension = propel

11. Fill in the table below (6 points)

Conjugate acid	Conjugate base
HSO4-	SO42-
HCl	Cl-
NH4+	NH3
H2O	OH-
H3O+	H2O
C2H5OH	C2H5O-

12.  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)

                        52.5 KJ

13.  When 33.00 mL of 0.215 M iron(III) chloride are added to 25.00 mL of 0.109 M potassium phosphate, a precipitate is observed to form.  Determine the concentrations of all ions in solution and calculate the mass of the precipitate. (12 points)

[Fe³⁺] = 0.069 M

[Cl^-] = 0.362 M

            [K⁺] = 0.155 M

            [PO₄^3-] = 0

            FePO₄ = 0.412 g

14. A tank contains a mixture of 4.8 mol of N₂ gas and 2.4 mol of O₂ gas at 25.5^oC and a total pressure of 9.86 atm.  Calculate the partial pressure (in torr) of each gas in the mixture.

      (6 points)

N₂ = 5.0 x 10³ torr

O₂ = 2.5 x 10³ torr

15. A solution is prepared by dissolving 0.2162 grams of HCl in 250.0 mL of solution.  Calculate the following. (8 points)

a.        [H⁺] = 0.024 M

b.       [OH^-] = 4.17 x 10^-13

c.        pH = 1.62

d.       pOH = 12.38

16. Sodium hydroxide is commercially available at a concentration of 8.0 M. What volume of this solution must be diluted to a final volume of 1.5 L to prepare a 2.5 M solution? (6 points)

V = 0.47 L

17. A hydrochloric acid solution is standardized by titrating against calcium hydroxide

                        2 HCl(aq) + Ca(OH)₂(aq) ® CaCl₂ (aq) + 2H₂O(l)

            23.4 mL of the base is used to neutralize 0.157 g HCl. Calculate the molarity of the of the            base solution. (6 points)

      0.092 M