Acid and Base Worksheet 4 Answer by vwi13045

VIEWS: 1,942 PAGES: 18

More Info
									NAME__________________________________ PERIOD _______                         Page 1 of 18
             UNIT 12 HW – ACID AND BASE CHEMISTRY ALL WORK MUST BE SHOWN FOR CREDIT
                                    NOTE: Ka & Kb TABLES AT END!

Worksheet 12-1: Acid Base: Conjugate Pairs and Naming/Writing formulas (2 PGS) (REQUIRES
INITIALS FOR STAMP!
                                                   TEACHER INITIALS:
Give the conjugate acid of the following bases:

BASE        CONJUGATE ACID                        BASE          CONJUGATE ACID
H2O                                               ClO─

acetate                                           H2PO4 ─

NH3                                               HSO4─

hydroxide                                         A─

CO32-                                             Methylamine
                                                  (CH3NH2)

Give the acid of the following conjugate bases:

ACID        CONJUGATE BASE                        ACID          CONJUGATE BASE
            Water                                               OH─

            ammonia                                             bromide ion


            SO42-                                               O32-


            HCO3-                                               CH3NH2

            cyanide ion                                         C2H3O2-



Give the base of the following conjugate acids:

BASE        CONJUGATE ACID                        BASE          CONJUGATE ACID
            HCN                                                 hydronium

            HCO3─                                               CH3NH3+

            ammonium                                            H2O

            HF                                                  HSO3─

            HC2H3O2                                             HA
NAME__________________________________ PERIOD _______                                               Page 2 of 18

Give the conjugate base of the following acids:

ACID                   CONJUGATE BASE                                ACID                        CONJUGATE BASE
HC2H3O2                                                              H2SO4

HA                                                                   oxalic acid

hydrochloric acid                                                    H3PO4


NH4+                                                                 H2CO3

HCN                                                                  hydrosulfuric acid


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

         (a)   NH3 (g) +        H3O+ (aq)            NH4+ (aq)       +       H2O (l)

         (b)   CH3COOH (l)          +       NH2-             CH3COO- (aq)         +    NH3 (g)

         (c)    NH2 -(g) +      H2O (l)            NH3 (g)     +      OH-(aq)

         (d)    HClO4 (aq)      +       H2O (l)         H3O+ (aq)        +      ClO4- (aq)

Name the following acids (they may not all exist, but use your rules to propose a name)

Formula    Anion Name             Acid Name                   Formula         Anion Name         Acid Name

H2Te                                                          H 2S

H2SO2                                                         HNO2

HBrO3                                                         HIO

H2CrO5                                                        H3PO3

HCl                                                           HF

H3PO2                                                         H2CrO4

HIO2                                                          H2SO3

HClO3                                                         H2Se

H2SO4                                                         HI

HBr                                                           HNO

HNO4                                                          HClO

HBrO2                                                         H2CrO2
NAME__________________________________ PERIOD _______                    Page 3 of 18
Worksheet 12-1 Con’t

Name                   Formula                 Name                 Formula
Hyponitrous acid                               Perchromic acid

Hydrobromic acid                               Nitrous acid

Chloric acid                                   Permanganic acid

Chromous acid                                  Hydrochloric acid

Hydrotelluric acid                             Hyposulfurous acid

Hypoiodous acid                                Iodic acid

Bromic acid                                    Bromous acid

Phosphorous acid                               Perchloric acid

Hypochromous acid                              Hydroselenic acid

Hydrosulfuric acid                             Hypochlorous acid
NAME__________________________________ PERIOD _______                                                     Page 4 of 18
WKS 12-2 Calculations pH (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 M]

        (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.      (a) If the pH of a solution is 12.5, what is the hydroxide ion concentration? (3.16 x 10-2)

        (b)   What is the hydrogen ion concentration?        (3.16 x 10-13 M)

        (c)    What is the pOH of this solution?       (pOH = 1.50)

        (d)    What is the pH of this solution?       (pH = 12.50)

6. Which would have a higher pH—a solution whose pOH is 5.42 or a solution whose hydrogen ion concentration is 9.44 x 10-8 M?
(pOH = 5.42)




7. 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)
NAME__________________________________ PERIOD _______                                                       Page 5 of 18
WKS 12-3 pH OF STRONG ACIDS AND BASES (two pages) SHOW ALL WORK AND CIRCLE FINAL ANSWER
Part A: Given molarity
1. What is the pH of 0.80 M hydrobromic acid? (pH = 0.097)


2.   If the pH of a strong acid solution is known to be 3.25, what is the molar concentration of the acid
                            solution assuming the acid is diprotic? (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 0.166 M barium 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 Ba+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.        (a) If the pH of a hydroiodic acid solution is known to be 3.21, what is the hydroxide ion concentration? (1.62 x 10-11 M)


         (b) What is the molar concentration of the acid solution?     (6.17 x 10-4)


7.        (a) What is the molar concentration of the hydroxide ion for a 0.45 M calcium hydroxide solution?        [0.90 M]


         (b) What is the pOH of this solution?    (pOH = 0.05)


         (c) What is the pH of a 0.45 M calcium hydroxide solution?         (pH = 13.95)


         (d) What is the hydrogen ion concentration of this solution?      (1.12 x 10-14 M)


         (e) What is the molar concentration of the calcium ion? [0.45 M]
NAME__________________________________ PERIOD _______                                                   Page 6 of 18
WKS 12-3 pH OF STRONG ACIDS AND BASES continued

Part B: More Challenging: Calculating Molarity from pH or pOH

8.   A solution was prepared using 5.413 g of oxalic acid and a 0.50000 L volumetric flaks. Calculate the molarity of the solution.
     (0.1200 M)




         (b) What is the pH of the solution assuming both hydrogen ions dissociate (not a good assumption but let’s run with it!)
      (0.62)




9.   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)




10. (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. (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?


11. 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)


12. 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)


13. 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)
NAME__________________________________ PERIOD _______                                               Page 7 of 18
Worksheet 12-4 WEAK ACID AND BASE PROBLEM PRACTICE (three pages)

A. Given molarity & K’s, find other stuff

1.      Answer the following questions regarding a 0.35 M acetic acid solution.

R
                                                                                  Ka =
I
C
                                                                                  % ionization =
E
_______________          (a) What is the percent ionization? (0.72%)

_______________          (b) What is the pH of this solution? (pH = 2.60)

_______________          (c) What is the hydroxide concentration in this solution? [4.0 x 10-12]


2.      Answer the following questions regarding a 2.35 M ammonia solution.

R
                                                                                  Kb =
I
C
                                                                                  % ionization =
E
_______________          (a) What is the pH? (pH = 11.81)


_______________          (b) What is the hydroxide ion concentration in this solution? (6.50 x 10-3 M)


_______________          (c) What percent is this solution ionizing? (0.28%)


_______________          (d) Would you expect a more dilute ammonia solution to ionize a greater amount or a lesser percentage of
                         its molecules compared to a more concentrated ammonia solution? (greater; more water available per
                         molecule)

_______________          (e) How many grams of ammonia must be added to water to make 1.0 liter of an ammonia solution with
                         a pH of 11.81? (40 g)


_______________          (f) Which would have a LOWER pH, a 2.35 M ammonia solution or a 0.235 M solution? Why?



3.      Would you expect a 2.4 M or a 1.2 M solution of methylamine to ionize the greater percent? Justify your answer with
        calculations. (1.2 M) problem continued on next page!

R
                                                                                  Kb =
I
C
                                                                                  % ionization =
E
NAME__________________________________ PERIOD _______                                                     Page 8 of 18
WKS 12-4 Cont.

R
                                                                                    Kb =
I
C
                                                                                    % ionization =
E




B. Given pH & K’s, find other stuff

4.       Answer the following questions for a nitrous acid solution that is known to have a pH of 3.21.

R
                                                                                    Ka =
I
C
                                                                                    % ionization =
E

_______________            (a) What is the hydrogen ion concentration of this solution? (6.17 x 10-4 M)


_______________            (b) what is the molar concentration of the acid? (8.45 x 10-4 M)


_______________            (c) Would you expect a 2.0 M or a 3.0 M nitrous acid solution to have a HIGHER pH? (2.0 M)


_______________            (d) Would you expect a 2.0 M or a 3.0 M nitrous acid solution to ionize the greater percentage?
                                 Why? (see question 5 for a hint!) (2.0 M)


5.   How many grams of aniline, C6H5NH2, must be dissolved in water to make 3.00 L of solution whose pH is 8.8? (26.9 g)
R
I
                                                                                    Kb =
C
E
NAME__________________________________ PERIOD _______                                                 Page 9 of 18
WKS 12-4 Cont.

C. Given molarity and % ionization, find K and other stuff.

6.      Answer the following questions regarding a 4.0 M hydroflouric acid solution that is known to ionize 1.3 %.

R
                                                                                  Ka =
I
C
                                                                                  % ionization =
E

_______________          (a) What is the hydrogen ion concentration? (5.0 x 10-2 M)


_______________          (b) What is the pH of the solution? (pH = 1.28)


_______________          (c) What is the hydroxide ion concentration of the solution? (1.92 x 10-13 M)


_______________          (d) Would you expect a 1.5 M hydroflouric acid solution to have a higher or a lower pH than the
                         4.0 M solution? (higher)


_______________          (e) Does a 4.0 M solution of hydroflouric acid or a 1.5 M solution of hydrofluoric acid ionize a
                         greater amount? Why? (1.5 M)


_______________          (f) Does a 4.0 M solution of hydroflouric acid or a 1.5 M solution of Hydrofluoric acid have a
                         LOWER pH? Why?

7.      Answer the following questions regarding a 0.15 M solution of a weak acid, HA, that is known to ionize 0.23%.

R
                                                                                  Ka =
I
C
                                                                                  % ionization =
E
_______________          (a) Find the Ka of the weak acid. (7.9 x 10-7)


_______________          (b) What is the pH of this acid solution? (pH = 3.46)


_______________          (c) What is the hydroxide ion concentration of this solution? (2.9 x 10-11 M)


_______________          (d) Is this acid a weaker or a stronger acid than acetic acid? How do you how? (weaker; Ka is
                         smaller)
NAME__________________________________ PERIOD _______                                        Page 10 of 18
WKS 12-5 pH OF ACIDS AND BASES – Mixed Strong and Weak (one page)

Find the pH of each of the following acids or bases:         8     0.50 M hypochlorous acid (pH = 3.91)

1.   0.80 hydrobromic acid (pH = 0.10)




2.   0.40 M ammonia (pH = 11.43)

                                                             9.    0.35 M sodium hydroxide    (pH = 13.54)




                                                             10.    0.72 M hydroflouric acid (pH = 1.80)
3.   0.35 M formic acid (pH = 2.10)




                                                             11. If the pH of a potassium hydroxide solution is 9.5, what is
4.   0.066 M strontium hydroxide   (pH = 13.12)              the hydroxide ion concentration? (3.16 x 10-5 M)
                                                             (b) What is the molar concentration of the potassium
                                                             hydroxide solution? (3.16 x 10-5 M)



5.   0.33 M lithium hydroxide (pH = 13.52)                   12. If the pH of a hydrobromic acid solution is 1.3, what is
                                                             the hydrogen ion concentration? [5.0 x 10-2]
                                                              (b) What is the molar concentration of the acid? [5.0 x 10-2]
                                                              (c) What is the hydroxide ion concentration of the acid
                                                             solution? [2.0 x 10-13]

6.   0.025 M hydroiodic acid (pH = 1.60)



                                                             13. If the pH of a nitrous acid solution is 4.5, what is the
                                                             hydroxide ion concentration of the solution? [3.2 x 10-10 M]
7.   1.50 M ethylamine (C2H5NH2) solution     (pH = 12.49)    (b) What is the molar concentration of the nitrous acid
                                                             solution? [2.2 x 10-6 M]
NAME__________________________________ PERIOD _______                                                       Page 11 of 18

Worksheet 12-6 pH OF SALTS, ACIDS, AND BASES WORKSHEET (one page)


Indicate whether each of the following salt solutions would be acidic, basic, neutral, or near neutral. YOU MUST SHOW
THE HYDROLYSIS REACTION FOR EACH SALT FOR CREDIT!

            Salt                                  Hydrolysis reaction                           Acid         Base Strength     acidity
                                                                                              strength
1.   ammonium nitrate

2.   potassium nitrate

3.   strontium acetate

4.   iron (III) phosphate

5.   beryllium perchlorate

6.   copper (II) chloride

7.   cesium sulfite

8.   chromium (III) chloride




_______________ 9.           (a)What is the pH of a 0.025 M hydrochloric acid solution?       (pH = 1.60)



_______________              (b) What is the hydroxide ion concentration in this solution? (4 x 10-13 M)




_______________ 10.         If the pH of an acetic acid solution is found to be 3.95, what is the molar concentration of the acetic
                              acid? (6.99 x 10-4 M)




_______________              (b) What is the percent ionization of the above acid? (16.0%)




_______________ 11.         If 10.0 grams of sodium hydroxide are dissolved in enough water to make 2.00 liters of solution,
                              what is the pH of the solution? (pH = 13.1)




_______________ 12.         If the pH of a strontium hydroxide solution is found to be 11.54, what is the molar concentration
                              of the solution? (1.734 x 10-3 M)
NAME__________________________________ PERIOD _______                                             Page 12 of 18
Worksheet 12-7 More Practice, Please (two pages)

1.  (a) Find the pH of a 0.0030 M solution of hydrochloric        5.  If the pH of an ammonia solution is known to be 11.85,
    acid. (pH = 2.52)                                                 what is the molar concentration of the weak
(b) What is the [H+] of the above solution? (0.0030 M)                 base? (2.78 M)
(c) What is the [0H-] of the above solution? (3.33 x 10-12 M)     (b) What is the percent ionization of this ammonia solution?
(d) What is the pOH of the above solution? (pOH = 11.48)          (0.25 %)




2.  (a) If the pH of a nitric acid solution is 2.1, what is the
    molar concentration of the acid? (0.0079 M)
(b) What is the [OH-] of the above solution? (1.27 x 10-12 M)


                                                                  6.  If the pH of a calcium hydroxide solution is known to be
                                                                      8.5, what is the molar concentration of the solution?
                                                                       (1.58 x 10-6M)
                                                                  (b) What is the percent ionization of the above compound?
                                                                  (100 %)
                                                                  (c) What is the [OH-] of this solution? (3.16 x 10-6)


3.  (a) If the pH of a HF solution is 2.3, what is its molar
    concentration? (0.071 M)
(b) What is the [H+] of this acid? (0.00501M)
(c) What is the percent ionization of this acid? (7.0 %)




                                                                  7.  If a 0.15 M solution of a weak acid is known to be 0.114%
                                                                      ionized, what is the Ka for this acid? (Ka = 1.43 x 10-7)
                                                                  (b) What is the [H+] for this acid? (0.00017 M)
4.  (a) Find the pH of a 0.32 M solution of strontium             (c) What is the pH for this acid? (pH = 3.77)
    hydroxide. (pH = 13.81)
(b) What is the [OH-] of the above? (0.64 M)
(c) What is the [H+] of the above? (1.56 x 10-14)
NAME__________________________________ PERIOD _______                                              Page 13 of 18
WKS 12-7 Cont.                                                    11. (a) If the pH of a solution is 12.3, how many grams of
8. Find the pH of a 1.50 M solution of hydroflouric acid. (pH          calcium hydroxide have been dissolved to make 500. ml of
   = 1.48)                                                             solution? (0.369 g)
                                                                  (b) What is the hydroxide ion concentration? (2.00 x 10-2 M)
                                                                  (c) What is the calcium ion concentration? (9.98 x 10-3 M)
                                                                  (d) What is the molar concentration of the solution? (9.98 x
                                                                  10-3 M)




9.  (a) Find the molar concentration of a potassium hydroxide
    solution if its pH is 11.3. (2.0 x 10-3 M)
(b) What is the [OH-] of the above solution? (2.0 x 10-3 M)




                                                                  12. What is the percent ionization of 0.33 M lactic acid
                                                                      solution? (2.1 %)
                                                                  (b) What is the hydrogen ion concentration? (6.8 x 10-3 M)
                                                                  (c) What is the hydroxide ion concentration? (1.5 x 10-12 M)
                                                                  (d) What is the pH of this solution? (pH = 2.17)




10. If the pH of a hypoiodous acid solution is 5.5, what is the
    molar concentration of the acid? (0.50 M)
(b) What is the percent ionization of this acid? (6.3 x 10-4 %)
(c) What is the hydroxide ion concentration? (3.16 x 10-9 M)
(d) What is the hydrogen ion concentration? (3.16x 10-6 M)


                                                                  13. How many grams of strontium hydroxide must be dissolved
                                                                      to make 3500 ml of a solution whose pH is 12.7? (10.7 g)
                                                                  (b) What is the hydroxide ion concentration of this solution?
                                                                  (5.01 x 10-2 M)
                                                                  (c) What is the strontium ion concentration of this solution?
                                                                  (2.51 x 10-2 M)
                                                                  (d) What is the molar concentration of the solution?(2.51 x 10-2)
NAME__________________________________ PERIOD _______                                         Page 14 of 18


   WKS 12-8: Titration Problems & Vocab review ( 3 pages)
   1.   What is the molarity of a solution of HCl if 25.0 mL is titrated to an endpoint by 10.0 mL of a 0.200-M solution
        of NaOH? (0.08 M HCl)



   2.   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 HCl that is 0.00300 M? (4.5 x 10-4 M Ba(OH)2)



   3.   What is the molarity of a nitric acid solution if 21.0 mL are needed to completely neutralize 25.0 mL of 0.300
        M NaOH? (0.357 M HNO3)



   4.   What is the molarity of a solution of KOH if 45.0 mL are completely neutralized by 15.0 mL of 0.500-M
        sulfuric acid solution in a reaction in which K2SO4 is one of the products? (0.333 M)



   5.   What is the concentration of a Sr(OH)2 solution if 20.0 mL of it is neutralized by 25.0 mL of a standard 0.0500
        M HCl? (0.0313 M)


   6.   If 25.0 mL of a 0.10 M NaOH solution are required to neutralize 15.0 mL of HCl, what is the molarity of the
        acid? (0.17 M)


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


   8.   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)


   9.   How many mL of 0.0200 M LiOH will neutralize 15.0 mL of 0.400 sulfuric acid? (600 mL)



   10. What volume of 0.196 M LiOH is required to neutralize 27.3 mL of 0.413 M HBr? (57.5 mL)




   11. What is the concentration of a solution of NaOH if 21.2 mL of a 0.0800 M solution of HBr is needed to
       neutralize 25.0 mL of the base? (0.0678 M base)



   12. If 86.2 mL of 0.765 M NaOH neutralize 30.0 mL of HCl, what is the concentration of the acid? (2.20 M HCl)

   13. If 40.8 mL of 0.106 M sulfuric acid neutralize 61.8 mL of KOH, what is the concentration of the base? (0.140
       M)
NAME__________________________________ PERIOD _______                                          Page 15 of 18
1         2         3                   4                                                           5

                                        6                                       7                              8

                                                                                                9

                                                  10

               11

                                                                                                    12

                    13                                                          14




                                                                 15

          16                       17




                         18                  19                                           20

21                                                          22




                                                                                     23

          24   25                                      26




                                                                           27

                                        28                                                                         29

     30                                                                                   31

32




               33                                                     34                  35             36

                              37                  38

                                                                                39

                                                                                                                   40

                                   41                       42

43                       44

                                                                                45        46

                                                       47

                                                                                                         48

                                                                      49             50

          51
NAME__________________________________ PERIOD _______                                     Page 16 of 18
ACROSS                                                   3. each whole number on the pH scale indicates the
                                                         acid or base is _____ stronger or weaker than the
1. Substances such as water or HCO3─ are called          next number (2 words)
____________________ because they can act as an          4. Indicators change ____ to show different pH
acid or a base.                                          values
6. pH 11 is ______ _________ times stronger than         5. Acid could have the pH value:
pH 8 (2 words)                                           7. precipitation with a pH of less than 5.6 (2 words)
9. Strong bases can do this to the skin                  8. Strong acids ionize __________ ____________
10. H3O+ = ______ ion                                    _________ (three words)
11. Mathematical tool for weak acids or bases            12. Bases feel __________________
13. conducts electricity                                 15. Characteristic of a substance that reacts strongly
14. Type of solution that forms during the               with a metal
hydrolysis of potassium fluoride                         17. Substance that can accept an electron pair (two
16. Reaction between an acid and a base                  words)
18. Substance that can donate an electron pair is        18. Bronsted’s buddy
called a ____________base                                19. Type of mathematics used for strong acids and
21. Type of acid or base that must be present in a       bases
buffer solution                                          20. used to measure strength of an acid or base (two
22. taste of an acid                                     words)
23. Common name for well known weak acid used            21. one of the products of neutralization
in food preparation                                      25. one product of a neutralization reaction
24. A polyatomic with a suffix “-ite” would form an      27 An acid with the suffix “-ic” is derived from a
acid with the suffix “-_____”                            polyatomic with the suffix “-____”
26. Pure water would have this pH                        29. pH of a solution that turns faint pink in the
28. These pairs differ only by a proton                  presence of phenolphthalein
31 A base could have this pH value                       30. When the forward rate is equal to the reverse
32. point in a titration when an acid or base is fully   rate in a solution of weak acid or base, the system
neutralized (two words)                                  has reached ______________________
35. Resulting pH for the hydrolysis of ammonium          31. The hydroxide ion has this kind of charge
perchlorate                                              33. organic material that changes color with an acid
37. Phosphoric acid is called _____________              or base
because it can donate more than one proton.              34. indicator made from a lichen, comes in red or
42. highest number on pH scale                           blue
43. process used to find the concentration of an acid    36. Mathematical relationship between base
or base by neutralizing it with a known amount of        molarity and pH
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 ion       50. the hydroxide ion is represented by this
2. Measure of the strength of an acid or base (two       chemical formula
words)
NAME__________________________________ PERIOD _______                      Page 17 of 18



                                Acid-Dissociation Constants at 25°C

ACID                Formula              Ka1               Ka2             Ka3
Acetic              CH3COOH             1.8 x 10 -5

Acetylsalicylic     C 9H 8O 4           3.0 x 10 -4

Arsenic             H3AsO4              5.6 x 10 -3      1.7 x 10 -7    4.0 x 10 -12

Arsenious           H3AsO3              6 x 10 -10

Ascorbic            HC6H7O6             8.0 x 10 -5

Benzoic             C6H5COOH            6.5 x 10 -5

Boric               H3BO3               5.8 x 10 -10

Carbonic            H2CO3               4.3 x 10 -7      5.6 x 10 -11

Chloroacetic        CH2ClCOOH           1.4 x 10 -3

Citric              C 6H 8O 7           7.1 x 10 -4      1.7 x 10 -5    4.1 x 10 -7

Cyanic              HCNO                1.8 x 10-4
Formic              HCOOH               1.8 x 10 -4

Hydrazoic           HN3                 1.9 x 10 -5

Hydrocyanic         HCN                 4.9 x 10 -10
Hydrofluoric        HF                  3.5 x 10 -4

Hydrogen Peroxide   H 2O 2              2.4 x 10 -12

Hydrosulfuric       H 2S                1.0 x 10 -7      ~10 -19

Hypobromous         HBrO                2.0 x 10 -9
Hypochlorous        HClO                3.5 x 10 -8
Hypoiodous          HIO                 2.3 x 10 -11
Lactic              HC3H5O3             1.4 x 10-4
Nitrous             HNO2                4.5 x 10-4
Propionic           HC3H5O2             1.3 x 10-5
NAME__________________________________ PERIOD _______                   Page 18 of 18



                           Base-Dissociation Constants at 25°C

Base                           Formula                     Kb
Ammonia                        NH3                        1.8 x 10-5

Aniline                        C6H5NH2                    4.3 x 10-10
Codeine                        C18H21NO3                  1.6 x 10-6
Dimethylamine                  (CH3)2NH                   5.4 x 10-4
Ethylamine                     C2H5NH2                    6.4 x 10-4
Hydrazine                      N 2H 4                     8.9 x 10-7
Hydroxylamine                  NH2OH                      9.1 x 10-9
Methylamine                    CH3NH2                     4.3 x 10-4
Morphine                       C17H19NO3                  1.6 x 10-6
Piperidine                     C5H11N                     1.3 x 10-3
Propylamine                    C3H7NH2                    5.1 x 10-4
Pyridine                       C5H5N                      1.8 x 10-9
Strychnine                     C21H22N2O2                 1.8 x 10-6
Trimethylamine                 (CH3)3N                    6.5 x 10-5

								
To top