General Instructions: Read each question carefully and answer each question in the expected format, using proper English grammar. For calculation problems, show your work and include units on all answers. If you need a pencil, eraser, calculator, etc., raise your hand.

Part A. Definitions (2 points each)
 1.  pH- is the negative log of the hydrogen ion concentration
 2.   _Electrolyte_ is a substance which conducts electricity in solution
 3.  Arrhenius acid - substance that dissociates in water to give protons
 4.  Conjugate acid - the acid produced when a base accepts a proton
 5.  _Weak acid_ is an acid which in solution dissociates slightly
 6.  Dissociate - Breaking apart in solution to give ions
 7   _Red Litmus_  is a paper used to determine whether a solution is basic.
 8.  Hydronium ion - H₃O⁺, the result of a proton interacting with water
 9.   _Diprotic acid_ is a compound which donates two protons.
10.  _Bronsted-Lowry Base_  is a proton acceptor,

Part B. Concepts
1.  Describe the properties of acids and bases. (4 points)
                       Acid                       Base
    taste             sour                        bitter
    touch            none                       slippery
    litmus            blue -> red             red ->blue
    reactivity       neutralizes base       neutralizes acid

2.  List the formula of 2 strong acids and the name of 2 strong bases. (4 points)
        HCl, H₂SO₄                                                sodium hydroxide, calcium hydroxide
3.  In the following balanced equation, identify the acid, base, conjugate acid, and conjugate
base. (4 points)
                   C₆H₅OH + H₂O ---> C₆H₅O^- + H₃O⁺
                        acid        base        conjgate     conjgate
                                                        base            acid
4. Name the following acids and bases. (5 points)
                   HCl             hydrochloric acid
                   HNO₃         nitric acid
                   Mg(OH)₂     magnesium hydroxide
                   NH₃             ammonia
                   H₂CO₃         carbonic acid

5. Is an acid with a Ka of 6.8 x 10^-5 strong or weak? (2 points)
            weak
6. What is the normality of NaOH if 25.00 mL require 48.12 mL of 0.0512 N HC1 to reach equivalence? (5 points)
            0.0985 N

7. What is the pH of a solution if 3.00 mL concentrated HCl (12.1 M) is diluted to 250.00
mL? (5 points)
            0.145 M is final conc., so pH would be 0.8

8. What is the pH of a solution if 25.0 g NaOH is dissolved and diluted to 250.00 mL in
water? (5 points)
            final conc. is 2.5 M so pH is 13.6

9. Acetic acid is a weak acid. Is sodium acetate a weak or a strong conjugate base? (2
points)
            strong

10. Explain why a buffer system requires both a weak acid and the salt of a weak acid. (5
points)
            weak acid will neutralize base, salt will neutralize acid

11. What volume of 18.0 M H₂SO₄ is required to make 1.25 L of 6.0 N H₂SO₄? (5 points)
            208 mL

12. Write the total ionic equation for the reaction of phosphoric acid with potassium hydroxide. (4 points)
            3 H⁺ + PO₄^3- + 3 K⁺ + 3 OH^-  ----->  3 H₂O + 3 K⁺ + PO₄^3-

Part C. Multiple Choice (2 points each)
1. Of the following acids, the weak acid is
    a. HCl
    b. HNO₃
    c. HCN
    d. H₃PO₄ (best classified as an intermediate strength acid)

2. The most acidic solution is one of pH
    a. 11.2
    b. 4.6
    c. 7.0
    d. 3.4

3. With 3.0 M of the following acids, which would yield the most acidic solution?
    a. H₂SO₄
    b. H₃PO₄ (not a strong acid and therefore does not dissociate completely)
    c. HCN
    d. HCl

4. In the reaction NH₃ + HCl ---> NH₄⁺ + Cl^-, NH₄⁺ is
    a. a strong acid
    b. a strong conjugate acid
    c. a weak acid
    d. a weak conjugate acid

5. How many water molecules would be formed if Mg(OH)₂ reacted with HNO₃?
    a. 1
    b. 2
    c. 3
    d. 4

6. KCl is
    a. acidic
    b. basic
    c. neutral
    d. none of the above

7. A dibasic compound is
    a. NH₃
    b. KOH
    c. Ca(OH)₂
    d. 2 KOH

8. The pH of a solution containing 1 x 10^-3 M H₂SO₄ is
    a. 6
    b. -3
    c. 3
    d. 2.7 (2 protons are produced from one molecule)

9. The pH of a solution containing 1 x 10^-5 M NaOH is
    a. -5
    b. 5
    c. 7
    d. 9

10. The salt which develops in the following reaction is

11. The amount of 0.5 N HCl required to neutralize 25.00 mL 1.0 N NaOH is
    a. 12.50 mL
    b. 25.00 mL
    c. 37.50  mL
    d. 50.00  mL

12. The salt formed in the following reaction is

13. The most basic of the following solutions is
    a. milk of magnesia, pH 10.6
    b. tomatoes, pH 4.6
    c. blood, pH 7.4
    d. seawater, pH 9 2

14. How many more protons are present at pH 7.2 than 8.5?
    a. 2.3 times more
    b. 20 times more
    c. 20 times less
    d. 2 3 times less

15. If 5.00 mL 6.0 M HCl and 5.00 mL 6.0 M NaOH are mixed, the solution would be.
    a. acidic
    b. basic
    c. neutral
    d. none of the above

Part A. Definitions (2 points each)
 1. Chemistry - Study of the structure, properties and changes of matter
 2._Mass_ is the amount of matter in a substance.
 3. Matter - Anything that has mass and occupies space
 4. _Alloy_-is a solution of 2 or more metals.
 5. _Oxidation_- is a loss of electrons
 6. Supernate - The liquid remaing after a precipitate is centrifuged
 7. _Stoichiometry_- is the ratio of product to reactant.
 8. Electronegativity - The amount of pull an atom has on another atoms electrons
 9. Anion - a negatively charged ion
10. _Potential energy_- is the amount of energy stored in the bonds of molecules.
11. Accuracy - How close a measurement is to the true value
12. _Isotope_-is two atoms of the same element having different mass.
13. Dipole moment - When partial positive and parital negative regions exist on a molecule
14 _Coordinate covalent_-is a bond formed when one atom donates both electrons
15. Polyatomic ion - two or more atoms which as a unit are charged

Part B. Multiple Choice (2 points)
1. A 50.00 mL sample weighs 12.5 g. The density is
    a. 4.00 g/mL
    b. 0.25 mL/g
    c. 4.00 mL/g
    d. 0.25 g/mL

2. The oxidation state of iron in FeA1₂(PO₄)₃ is
    a. -3
    b. +3
    c. +5
    d. +9

3. A silicon-carbon bond would be expected to be
    a. ionic
    b. metallic
    c. nonpolar
    d. polar covalent

4. According to the following equation, if I begin with 16.0 g CH₄, I will get how many grams CO₂?

5. The periodic trend for atomic size.
    a. increases top to bottom, increases left to right
    b. increases top to bottom, increases right to left
    c. increases bottom to top, increases left to right
    d. increases bottom to top, increases right to left

6. The number of nitrogen atoms in Fe₂(NO₃)₃ is
    a. 2
    b. 3
     c. 6
    d. 9

7. The number of oxygen atoms in the following reaction is

8. The shape of the sulfate ion is
    a. linear
    b. triangular
    c. pyramidal
    d. tetrahedral

9. What is the volume, in liters, of l.12 mol of H₂S at 62^oC and 1.38 atm?
    a. 5.0 L
    b. 4.13 L
    c. 95.8 L
    d. 22.3 L

10. Which of the following gas samples at STP contains the greatest number of molecules?
    a. 5.0 g H₂
    b. 50 L of He
    c. 1.0 X 10²⁴ molecules of CO₂

11. A gas at 100^oC occupies 154 mL. What will the volume be at 10.0^oC, assuming no change in pressure?
    a.      15.4 mL
    b.    117 mL
    c.    203 mL
    d.  1540 mL

12. The strongest force of attraction between 2 molecules of H₂S is
    a. London force
    b. hydrogen bond
    c. dipole-dipole
    d. force of good and evil

13. The weakest force of attraction between 2 molecules of water is the gas state is
    a. hydrogen bond
    b. London force
    c. dipole-dipole
    d. the dark force

14. The compound with the highest boiling point is
    a. C₈H₁₈
    b. CH₃COOH
    c. NaBr
    d. F₂

15. Not scored

16. The reducing agent in the following reaction is
                   2 H₂S + 3 O₂ ---> 2 H₂O + 2 SO₂
    a. H₂S
    b. O₂
    c. CO₂
    d. O₂

17. The oxidized atom in the following reaction is
                   MnO₄^- + 5 Fe²⁺ + 8 H⁺ ----> Mn²⁺ + 5 Fe³⁺ + 4 H₂O
    a. Mn
    b. O
    c. Fe
    d. H

18. The number of neutrons in ⁵⁶Fe²⁺ is
    a. 30
    b. 56
    c. 24
    d. 26

19. The number of electrons in K⁺ is
    a. 39
    b. 19
    c. 20
    d. 18

20. The third period element having the Lewis dot structure E: is
    a. S
    b. Mg
    c. Ca
    d. O

21. The element having the electron configuration 1s² 2s² 2p⁵ is
    a. C
    b. N
    c. O
    d. F

22. The nitrate ion has a charge of
    a. -2
    b. -1
    c. +1
    d. +2

23. The correct Lewis dot structure of NH₃ is Answer A

24. Which of the following is an oxidation reaction?
    a. Cl₂ --- > 2 Cl^-
    b. copper (II) ions----> copper(I) ions
    c. Ag⁺ --> Ag
    d. Al ---> Al³⁺

25. Which of the following substance(s) is oxidized?

26. Which of the following correctly describes a homogenous sample?
    a. Uniform appearance and composition throughout.
    b. A mixture of diamond and graphite, which are both forms of carbon.
    c. Reacts with all natural elements.
    d. Reacts with all elements.

27. Which of the following does not describe the solid state?
    a. rigid, constant shape
    b. constant volume
    c. easily compressed
    d. particles vibrate in fixed position

28. Potassium is a(n)
    a. halogen
    b. noble gas
    c. transition element
    d. alkali metal

29. The number of inches in 25.0 cm is
    a. 25.0
    b. 615
    c. 9.84
    d. none of the above

30. The charge on a carbonate ion is
    a. -2
    b. -1
    c. +1
    d. +2

31. 1.5 L of a 3.2 M solution contains how many moles?
    a. 3.2
    b. 0.47
    c. 4.8
    d. 4.7

32. Not scored

33. The unit of amount is
    a. Liter
    b. mole
    c. meter
    d. doesn't have units

34. Identify the incorrect item in the following group
    a. SO₄^2-
    b. NH₄⁺
    c. NO₃^2-
    d. OH^-

35. The element with the highest electronegativity is
    a. Mg
    b. Cr
    c. Rn
    d. S