Unit 13 Homework by pengxuebo

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									Pre-AP Chemistry Unit 13 HW Packet                      Name ______________________________________

             WKS 13.1 – Conjugates Using Brönsted-Lowry’s Definition (2 pages)
Give the conjugate acid of the following bases:
BASE                  CONJUGATE ACID               BASE              CONJUGATE ACID

   H2O                                                ClO─


  acetate                                            H2PO4 ─


   NH3                                               HSO4─


hydroxide                                              A─

                                                   Methylamine
  CO32-
                                                    (CH3NH2)

Give the acid of the following conjugate bases:
         ACID                CONJUGATE BASE                ACID            CONJUGATE BASE

                                       water                                          OH─

                                                                                  bromide ion
                                      ammonia


                                       SO42-                                           O2-

                                                                                    CH3NH2
                                       HCO3-

                                                                                    C2H3O2-
                                     cyanide ion

Give the base of the following conjugate acids:
         BASE                 CONJUGATE ACID               BASE            CONJUGATE ACID

                                        HCN                                        hydronium


                                       HCO3─                                        CH3NH3+


                                     ammonium                                         H2O


                                        HF                                           HSO3─

                                     HC2H3O2                                           HA

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Pre-AP Chemistry Unit 13 HW Packet                                           Name ______________________________________
             WKS 13.1 – Conjugates Using Brönsted-Lowry’s Definition (continued)
Give the conjugate base of the following acids:
    ACID                  CONJUGATE BASE                                ACID                CONJUGATE BASE

    HC2H3O2                                                                H2SO4


      HBr                                                                oxalic acid

                                                                           H3PO4
hydrochloric acid


      NH4+                                                                 H2CO3

                                                                    hydrosulfuric acid
      HCN


Identify the acid (A), base (B), conjugate acid (CA), and conjugate base (CB) in the following reactions:



       (1)    NH3 (g) +      H3O+ (aq)           NH4+ (aq)     +        H2O (l)




       (2)    CH3COOH (l)        +       NH2-            CH3COO- (aq)        +    NH3 (g)




       (3)    NH2 -(g) +     H2O (l)           NH3 (g)     +     OH-(aq)




       (4)    HClO4 (aq)     +       H2O (l)         H3O+ (aq)      +      ClO4- (aq)




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Pre-AP Chemistry Unit 13 HW Packet                                     Name ______________________________________
                                     WKS 13.2 – Naming Acids (1 page)
Name the following acids. (They may not all exist, but use your rules to propose a name!)
 Formula                       Acid Name                      Formula                       Acid Name

   H2Te                                                         H2S

   H2SO2                                                       HNO2

   HBrO3                                                        HIO

   HNO3                                                        H3PO3

    HCl                                                          HF

   H3PO2                                                       HBrO2

   HIO2                                                        H2SO3

   HClO3                                                        H2Se

   H2SO4                                                         HI

    HBr                                                        HClO4


Write the formula for the following acids.
      Name                           Formula                       Name                        Formula
   Nitrous acid                                                 Acetic acid

Hydrobromic acid                                             Hypochlorous acid

   Chloric acid                                              Permanganic acid

Hydrofluoric acid                                            Hydrochloric acid

Hydrotelluric acid                                          Hyposulfurous acid

 Hypoiodous acid                                                 Iodic acid

  Carbonic acid                                                Bromous acid

Phosphorous acid                                              Perchloric acid

Hydrosulfuric acid                                           Hydroselenic acid




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Pre-AP Chemistry Unit 13 HW Packet                                         Name ______________________________________

                          WKS 13.3 – pH / pOH Calculations, Part 1 (1 page)
Show all work and circle your answers!

1.     (a) If the hydrogen ion concentration of a solution is 1.30 x 10-4 M, what is the pH of the solution? (pH = 3.89)


       (b) What is the pOH of this same solution? (pOH = 10.11)


       (c) What is the hydroxide concentration of the solution? [7.69 x 10-11]


2.     (a) If the hydroxide ion concentration of a solution is 2.8 x 10-6 M, is it an acidic or a basic solution?
                (pH = 8.45, basic)

       (b) What is the pH of this solution? (pH = 8.45)


       (c)   What is the hydrogen ion concentration of this solution? [3.61 x 10-9]


       (d)   What is the pOH of this solution?       (pOH = 5.65)


3.     (a)   If the pH of a solution is 4.67, what is the hydroxide ion concentration? [4.68 x 10-10]


       (b)   What is the pOH of this solution?       (pOH = 9.33)


       (c)    What is the hydrogen ion concentration?      [2.14 x 10-5]


       (d)    Is this an acidic or basic solution?   (acidic)


4.     (a)    If the pOH of a solution is 3.6, what is the pH? (pH = 10.40)


       (b)   What is the hydrogen ion concentration of this solution?       [3.98 x 10-11]


       (c)   What is the hydroxide ion concentration of this solution?      [2.51 x 10-4]


       (d)   Does this solution have a higher hydrogen ion or hydroxide ion concentration? (hydroxide)


5. Which would have a more basic pH—a solution whose hydrogen ion concentration is 3.4 x 10-8 M or a solution whose
   hydroxide ion concentration is 2.6 x 10-5 M? (2.6 x 10-5 M)




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Pre-AP Chemistry Unit 13 HW Packet                             Name ______________________________________

                          WKS 13.4 – pH / pOH Calculations, Part 2 (1 page)
Calculate all of the unknown variables in the table.
                                                                                        Acidic,Basic, or
                  [H+]                    pH             [OH-]                pOH
                                                                                           Neutral
1             2.30 x 10-4                 3.63         4.35 x 10-11            10.4           Acidic

2                                         7.9

3                                                      1.05 x 10-3

4             3.66 x 10-3

5                                                                              11.5

6                                          12

7                                                       5.5 x 10-7

8             7.77 x 10-11

9                                                                              13.0

10                                        7.0

11            9.33 x 10-6

12                                                     1.11 x 10-2

13                                                                             2.55

14                                        0.55

15            9.05 x 10-14




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Pre-AP Chemistry Unit 13 HW Packet                                       Name ______________________________________
                        WKS 13.5 – Strong Acid & Base Calculations (2 pages)
Show all work and circle your answers!
1. What is the pH of 0.80 M hydrobromic acid? (pH = 0.097)




2. If the pH of a sulfuric acid solution is known to be 3.25, what is the molar concentration of the acid solution?
   (2.8 x 10-4 M)




3.       (a) If the pH of a barium hydroxide solution is known to be 12.50, what is the hydroxide ion concentration?
             (3.16 x 10-2 M)




        (b)   What is the barium ion concentration?    (1.58 x 10-2 M)


        (c)   What is the molar concentration of the base solution?      (1.58 x 10-2 M)


4.      (a) What is the hydroxide ion concentration of a 0.166 M calcium hydroxide solution? (0.33 M)




        (b) What is the hydrogen ion concentration of the solution? (3.03 x 10-14)


        (c) What is the pH of the solution?      (pH = 13.52)


        (d) What is the Ca+2 ion concentration in this solution?   (0.166 M)


5. If the pH of a cesium hydroxide solution is known to be 9.75, what is the molar concentration of the base solution?
   (5.62 x 10-5 M)



6. If the pH of a hydroiodic acid solution is known to be 3.21, what is the molar concentration of the acid solution?
   (6.17 x 10-4)



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Pre-AP Chemistry Unit 13 HW Packet                                     Name ______________________________________
                      WKS 13.5 – Strong Acid & Base Calculations (continued)
Show all work and circle your answers!
7. (a) A solution was prepared using 28.3 g of potassium hydroxide and then diluting to a final volume of 2.0000L.
       What is the molarity of the base solution? (0.252 M)




        (b) What is the pH of the solution? (13.40)




8. (a) A strong monoprotic acid was prepared by diluting 1.35 mL of a concentrated, 12.0 M solution to a final volume
       of 0.250 L. Calculate the final molarity of the solution. HINT: Think about dilution from last unit! (0.0648 M)




        (b) What is the molar concentration of the hydrogen ion?    (0.0648 M)




        (c) What is the pH of the solution? (1.19)



        (d) What color would phenolphthalein be in this solution?


9. Which would have a higher pH—a 0.035 M potassium hydroxide solution or a 0.018 M calcium hydroxide solution?
   Explain. (Ca(OH)2)




10. Which would have the more acidic pH-a 0.0025 M strontium hydroxide solution or a solution whose hydrogen ion
    concentration is 1.44 x 10-13? (.0025 M Sr(OH)2)




11. If the barium ion concentration of a barium hydroxide solution is known to be 0.25 M , what is the pH of the solution?
    (pH = 13.70)




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Pre-AP Chemistry Unit 13 HW Packet                                      Name ______________________________________

             WKS 13.6 – Titration Calculations & Neutralization Reactions (1 page)
Solve the following titration problems. Be sure to show your work!
1.   What is the molarity of a solution of barium hydroxide if 50.0 mL are titrated to an endpoint by 15.0 mL of a solution
     of hydrobromic acid that is 0.00300 M? (4.5 x 10-4 M Ba(OH)2)



2.   What is the concentration of a strontium hydroxide solution if 20.0 mL of it is neutralized by 25.0 mL of a 0.0500 M
     hydrochloric acid solution? (0.0313 M)



3.   What is the molarity of a potassium hydroxide solution if 35.0 mL of it are neutralized by 15.0 mL of 0.765 M
     sulfuric acid? (0.656 M)



4.   If 25.0 mL of vinegar solution (acetic acid) is neutralized 15.0 mL of 0.500 M NaOH, what is the molarity of the
     vinegar? (0.300 M)



5.   How many mL of 0.0200 M lithium hydroxide will neutralize 15.0 mL of 0.400 sulfuric acid? (600 mL)




6.   What volume of 0.196 M cesium hydroxide is required to neutralize 27.3 mL of 0.413 M hydrobromic acid? (57.5
     mL)



Write the balanced neutralization reactions for the following:
7.   Cesium Hydroxide and Sulfuric Acid




8.   Calcium Hydroxide and Hydrobromic Acid




9.   Sodium Hydroxide and Perchloric Acid




10. Lithium Hydroxide and Hydroselenic Acid




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Pre-AP Chemistry Unit 13 HW Packet                                    Name ______________________________________

                      WKS 13.7 – A Little Bit of Everything Review! (2 pages)
   1. Put the following in order of most acidic to most basic.
      a. pH 3.6
      b. [H+] = 1.25 x10-7
      c. pOH = 13.2
      d. [OH-] = 5.89 x10-2

   2. Fill out the following chart with regards to acids and bases:
                                                             ACIDS                             BASES

           Usually have in the formula:


            Arrhenius’ definition says:


         Bronsted-Lowry’s definition says:


                Has a pH range of:

          Will turn this color with litmus
                       paper:

               Will turn this color in
                phenolphthalein:

        Will do this when put with a metal:
        (include identity of gas, if formed)

   3. Fill out the following chart with regards to strong vs. weak acids and bases:
                                                    Strong Acids and Bases               Weak Acids and Bases

            To what % do they ionize?

          Are they a strong conductor or a
                 poor conductor?

        Would their pH be closer or farther
            away from 7 (neutral)?

         Which arrow do we show in their
              ionization reaction?

   4. Write a reaction using phosphoric acid and ammonia as reactants. Identify each reactant and product as being an
      acid, base, conjugate acid, or conjugate base. (Use Bronsted-Lowry’s definition to help you!)




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Pre-AP Chemistry Unit 13 HW Packet                                    Name ______________________________________
                    WKS 13.7 – A Little Bit of Everything Review! (continued)
   5. What is the difference between strength and concentration (in regards to acids and bases)?



   6. What is the pH of a 0.32 M solution of calcium hydroxide? (13.81)




   7. If the pH of a cesium hydroxide solution is known to be 9.75, what is the molar concentration of the original base
      solution? (5.62 x 10-5 M)




   8. What is the [OH-] of a sulfuric acid solution with a pH of 1.34? What is the original concentration of the acid?
      (2.19 x 10-13 M, 2.29 x 10-2 M)




   9. How many grams of strontium hydroxide must be dissolved to make a 8.78 L solution with a pH of 12.12? What
      is the hydroxide ion concentration? What is the strontium ion concentration? (7.02 g, 0.0132 M, 6.59 x 10-3 M)




   10. What is the molarity of a solution of Ba(OH)2 if 50.0 mL are titrated to an endpoint by 15.0 mL of a solution of
       H2SO4 that is 0.300 M? (0.0900 M)




   11. What is the purpose of a buffer?




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Pre-AP Chemistry Unit 13 HW Packet                                               Name ______________________________________
                           WKS 13.8 – Vocabulary Crossword Puzzle (2 pages)
   1          2             3                   4                                                                   5

                                                6                                              7                                8

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                      11

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                                 18                  19                                                  20

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              24      25                                           26




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                      33                                                             34                  35

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                                           41                              42

   43                            44

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 WORD BANK:                burn                           hydrogen                        nine                           seven
                           color                          hydronium                       OH                             slippery
 acetic                    conjugate                      ide                             one hundred percent            sour
 acid rain                 corrosive                      indicator                       one thousand                   stoichiometry
 acidic                    down                           inverse                         ous                            stronger
 alkaline                  electrolyte                    lewis                           percent ionization             ten times
 amphoteric                endpoint                       lewis acid                      pH scale                       titration
 arrhenius                 equilibrium                    litmus                          pOH                            tri
 ate                       equivalence point              lowry                           polyprotic                     water
 basic                     focus                          negative                        proton                         weak
 bitter                    four                           neutral                         rice
 buffer                    fourteen                       neutralization                  salt
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Pre-AP Chemistry Unit 13 HW Packet                                Name ______________________________________

                         WKS 13.8 – Vocabulary Crossword Puzzle (2 pages)
   ACROSS                                                   2. Measure of the strength of an acid or base (two
                                                                words)
   1. Substances such as water or HCO3─ are called          3. Each whole number on the pH scale indicates the
       ____________________ because they can act as             acid or base is _____ stronger or weaker than the
       an acid or a base.                                       next number (2 words)
   6. pH 11 is ______ _________ times stronger than         4. Indicators change ____ to show different pH
       pH 8 (2 words)                                           values
   9. Strong bases can do this to the skin                  5. Acid could have the pH value:
   10. H3O+ = ______ ion                                    7. Precipitation with a pH of less than 5.6 (2 words)
   11. Mathematical tool for weak acids or bases            8. Strong acids ionize __________ ____________
   13. conducts electricity                                     _________ (three words)
   14. Type of solution that forms during the               12. Bases feel __________________
       hydrolysis of potassium fluoride                     15. Characteristic of a substance that reacts strongly
   16. Reaction between an acid and a base                      with a metal
   18. Substance that can donate an electron pair is        17. Substance that can accept an electron pair (two
       called a ____________base                                words)
   21. Type of acid or base that must be present in a       18. Bronsted’s buddy
       buffer solution                                      19. Type of mathematics used for strong acids and
   22. Taste of an acid                                         bases
   23. Common name for well known weak acid used            20. Used to measure strength of an acid or base (two
       in food preparation                                      words)
   24. A polyatomic with a suffix “-ite” would form an      21. One of the products of neutralization
       acid with the suffix “-_____”                        25. One product of a neutralization reaction
   26. Pure water would have this pH                        27. An acid with the suffix “-ic” is derived from a
   28. These pairs differ only by a proton                      polyatomic with the suffix “-____”
   31. A base could have this pH value                      29. pH of a solution that turns faint pink in the
   32. Point in a titration when an acid or base is fully       presence of phenolphthalein
       neutralized (two words)                              30. When the forward rate is equal to the reverse
   35. Resulting pH for the hydrolysis of ammonium              rate in a solution of weak acid or base, the
       perchlorate                                              system has reached ______________________
   37. Phosphoric acid is called _____________              31. The hydroxide ion has this kind of charge
       because it can donate more than one proton.          33. Organic material that changes color with an acid
   42. Highest number on pH scale                               or base
   43. Process used to find the concentration of an acid    34. Indicator made from a lichen, comes in red or
       or base by neutralizing it with a known amount           blue
       of acid or base                                      37. Negative log base 10 of [OH─]
   45. Point in a titration when an indicator changes       38. Ion formed when an acid ionizes
       color                                                39. Taste of a base
   47. A mixture that can resist changes in pH              40. pH for a solution of potassium chloride
   49. Acids with larger values of Ka are                   41. Mathematical relationship between pH and [H+]
       ______________ acids                                 42. What you must do to pass Pre-AP Chemistry
   51. Gas that forms when active metals react with             (focus)
       acids.                                               44. The binary acid, hydrobomic acidy had an ion
                                                                with the suffix “______-“ in its name.
   DOWN                                                     46. As the molarity of an acid increases, the pH of
                                                                the solution goes _______________
   1. Dead guy whose theory defines a base as a             48. Phosphoric acid is a ______protic acid.
      substance that dissociates to form a hydroxide        50. The hydroxide ion is represented by this
      ion                                                       chemical formula




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