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Name___________________________________ Period_____

Acids and Bases OTHS Academic Chemistry

Objectives: Define acids and bases and distinguish between Arrhenius and Bronsted-Lowry definitions

Distinguish between degrees of dissociation for strong and weak acids and bases

Understand, differentiate, and predict products among acid-base reactions,

Define pH and use the hydrogen or hydroxide ion concentrations to calculate the pH of a solution

Vocabulary: acid, base, alkaline, pH scale, bitter, sour, conjugate acid, conjugate base, neutralization,

dissociation, complete ionization, soluble, Molarity, electrolyte, logarithm, titration, indicator, buret, equivalence point, end point, and coefficient

Memorize: Acid/Base Nomenclature

Provided: pH + pOH= 14 [H+] x [OH-]= 1.0 x 10-14 pH= -log [H+] pOH= -log [OH-] [H+]= 10^-pH [OH-]=10^-pOH nb Ma Va = na Mb Vb CHECKLIST: How to be successful in OTHS Academic Chemistry

Pay attention and take notes in class

Ask questions in class on material that is not clear

Work every page in the practice packet for the unit

Check answers to the practice packet online at http://othschem.weebly.com/

Come to tutorials with any chemistry teacher

Do the online homework and check solutions once they become available

Always do the practice test for every test & ask good questions on review day

Keep up with the calendar for the class/be aware of approaching quizzes, tests, & other deadlines

Use videos posted on website as a quick and convenient tutorial

Read chapter in the book

pH pOH Solution type

= 7 = 7 Neutral < 7 > 7 Acidic > 7 < 7 Basic

Name_____________________________ Per. _______

Note that H3O+ ions are “hydrated” hydrogen ions. H+ and H3O+ are interchangeable. H+ + H2O = H3O+

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Name: _____________________________ Period: _______

Properties and Identification of ACIDS, BASES AND SALTS SECTION 1: IDENTIFICATION - Identify the following examples as: A = acid B = base S = salt Remember from the previous units, a salt is any ionic compound, excluding what we classify as a base. ____1. AgOH

____2. MgSO4

____3. ZnCO3

____4. H2SO4

____5. NaOH

____6. HClO

____7. Mg(OH)2

____8. HNO3

____9. Pb(ClO)2

____10. (NH4)2CO3

____11. HC2H3O2

____12. HBr

SECTION 2: PROPERTIES – Determine if each of the following is an acid (A) or a base (B) using the descriptions listed. _______ 13. A cleaning solution turns litmus paper blue.

_______ 14. Your breakfast juice tasted sour.

_______ 15. The substance you are analyzing in lab has a greater concentration of H+ than OH-.

_______ 16. The face wash you used this morning felt slippery.

_______ 17. The battery in your remote control was alkaline.

_______ 18. The bumper on your car started to corrode because the rain water had a pH of 5.

_______ 19. Your mom washed your mouth out with soap (you probably deserved it) and it tasted bitter.

_______ 20. Drinking too much Coke is bad for my teeth and it will turn litmus paper red.

_______ 21. The bleach I spilled on my favorite shirt had a pH of 10.

_______ 22. The Drano that I used to unclog the drain has more OH- ions than H+ ions.

SECTION 3: ELECTROLYTES – Using your notes, determine if each of the following is an electrolyte (E) or nonelectrolyte (N). Remember, soluble salts make ions in solution, so they are also electrolytes. If a compound is not a strong acid, strong base or soluble salt, it is a nonelectrolyte and does not produce ions in solution. ______ 23. HCl

______ 24. CO2

______ 25. NaOH

______ 26. HClO3

______ 27. NaNO3

______ 28. KOH

______ 29. HNO3

______ 30. C6H12O6

______ 31. LiOH

______ 32. H2SO4

______ 33. HI

______ 34. Na2SO3

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Name______________________ Per. ___

Practice Worksheet: Acid/Base Nomenclature Decide whether each is an acid or base, and then write formulas: 1. sulfuric acid ____________ 2. chloric acid ___________ 3. magnesium hydroxide_________ 4. nitric acid ____________ 5. hydrofluoric acid ____________

6. sodium hydroxide___________ 7. phosphorous acid____________ 8. ammonia ____________ 9. calcium hydroxide____________ 10. hydrobromic acid____________

Decide whether each is an acid or base, and then write names: 11. H2CO3 _________________________ 12. Al(OH)3 _________________________ 13. H3PO4 _________________________ 14. HClO4 _________________________ 15. KOH _________________________ 16. HCl _________________________ 17. HNO2 _________________________ 18. Ba(OH)2 _________________________ 19. H2SO3 _________________________ 20. HCN _________________________

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Name: _________________________________ Period: _____ pHooey!

Part I: Discovering the math behind pH Instructions: The following data table contains some data collected in a lab by students just like you. I have added some additional information to help you understand and make connections between the values for pH and the math used to determine these values from concentration. Complete this table by adding in the missing values: Substance Acidic or

Basic? pH [H+] (in decimal) [H+] (in scientific

notation) Stomach acid (0.1 M HCl) Acidic 0.1 M 1.0 x 10-1 M Clear Soda 3 0.001 M Rain Water Acidic 1.0 x 10-6 M Distilled Water 7 0.0000001 M Alcohol Neutral Salt Water 0.0000001 M Washing soda Basic 8 1.0 x 10-8 M Ammonia 0.0000000001 M 1.0 x 10-10 M Drain Cleaner (0.1 M NaOH) 13 1 M NaOH 1.0 x 10-14 M 1 M HCl Answer the following questions:

1. What does [H+] stand for?

2. If you know the concentration of [H+] of a solution in decimal form, explain how you can determine its pH.

3. If you know the concentration of [H+] of a solution in scientific notation, explain how you can determine its pH.

4. As the value of pH increases, what happens to the concentration of H+?

5. As the value of pH decreases, what happens to the concentration of H+?

6. Solution A has a pH of 5. Solution B has a pH of 9.

a. What is the [H+] of Solution A? Solution B?

b. Identify the solutions as acidic or basic.

c. Which solution has the greatest concentration of H+? How many times greater is the concentration of H+ ?

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Part II: Looking at hydroxide, OH- Instructions: Imagine the following table contains results of a series of dilutions of HCl and NaOH. Additional information about the solutions (the pOH) is included. Complete this table by adding in the missing values: HCl Solution NaOH Solution Answer the following questions:

1. What does [OH-] stand for?

2. What can you say about the concentration of OH- in solutions with high acidity?

3. How is the value of the pH related to the value of the pOH for each concentration?

4. If you know the value of the pH, how can you determine the value of the pOH for the same solution?

Making the connection: How are pH and pOH related to each other mathematically? How are [H+]and [OH-] related to each other mathematically?

Well pH [H+] [OH-] pOH A 1 1.0 x 10-1 M 13 B 2 1.0 x 10-2 M 1.0 x 10-12 M 12 C 3 1.0 x 10-3 M D 4 1.0 x 10-4 M 1.0 x 10-10 M 10 E 5 1.0 x 10-5 M F 6 1.0 x 10-6 M G 7 1.0 x 10-7 M H 7 1.0 x 10-7 M 1.0 x 10-7 M 7 I 7 1.0 x 10-7 M 7 R 7 1.0 x 10-7 M 1.0 x 10-7 M 7 Q 7 1.0 x 10-7 M 7 P 7 1.0 x 10-7 M O 8 1.0 x 10-8 M N 9 1.0 x 10-9 M 1.0 x 10-5 M 5 M 10 1.0 x 10-10 M L 11 1.0 x 10-11 M 3 K 12 1.0 x 10-12 M 1.0 x 10-2 M J 13 1.0 x 10-13 M 1.0 x 10-1 M 1

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Name________________________ Per. _____

pH Practice Worksheet Use the “Guide to pH Calculations” to do these problems.

Given Unknown Acidic, Basic, or Neutral? (A/B/N)

1. pH = 7

pOH =

2. pOH = 12.5

pH =

3. [H+] = 2.6 x 10 - 4

pH =

4. [H+] = 1.0 x 10 - 8

pH =

5. [OH -] = 1.3 x 10 - 12

pOH =

6. [OH -] = 7.8 x 10 - 2

pOH =

7. [OH -] = 1.0 x 10 - 10

[H+] =

8. [OH -] = 5.2 x 10 - 3

[H+] =

9. [H+] = 1.0 x 10 - 7

[OH -] =

10. [H+] = 9.1 x 10 - 13

[OH -] =

11. pH = 3.0

[H+] =

12. pH = 11.6

[H+] =

13. pOH = 12.5

[OH -] =

14. pOH = 9.0

[OH -] =

15. pH = 10.3

pOH =

16. pH = 5.2

[H+] =

17. pOH = 14.0

pH =

18. pOH = 4.4

[OH-] =

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Name_______________________ Per. _____

Practice Worksheet Neutralization Reactions

I. Nomenclature Name the following: Write formulas for the following: 1. Al(NO3)3 4. potassium sulfate 2. HNO3 5. lithium hydroxide 3. Ca(C2H3O2)2 6. calcium carbonate II. Neutralization Reactions: write the balanced equation for the reaction between the following acids and bases: 7. acetic acid and sodium hydroxide 8. hydrochloric acid and calcium hydroxide 9. phosphoric acid and magnesium hydroxide 10. carbonic acid and potassium hydroxide 11. sulfuric acid and ammonia (use NH4OH for ammonia; it’s NH3 + H2O) 12. nitric acid and lithium hydroxide

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Titration Worksheet

1. What is the purpose of a titration?

2. Why do you need an indicator in a titration?

3. What is the difference between an endpoint and an equivalence point?

4. Why is it important not to “overshoot” the titration? Refer to your answer to #1.

5. Write the neutralization reaction between hydrochloric acid and potassium hydroxide.

6. What is the mole ratio of acid to base in the above reaction?

7. Write the neutralization reaction between nitric acid and calcium hydroxide.

8. What is the mole ratio of acid to base in the above reaction?

9. Write the neutralization reaction between sulfuric acid and lithium hydroxide.

10. What is the mole ratio of acid to base in the above reaction?

11. Calculate the molarity of an acetic acid solution if 34.57 mL of this solution are needed toneutralize 25.19 mL of 0.1025 M sodium hydroxide. IS THE EQUATION BALANCED?

HC2H3O2 (aq) + NaOH (aq) NaC2H3O2 (aq) + H2O (l)

12. 50 mL of 0.60 M sodium hydroxide neutralized 20 mL of sulfuric acid. Determine theconcentration of the acid. BALANCE THE EQUATION FIRST!

___ H2SO4 (aq) + ___ NaOH ___ Na2SO4 (aq) + ___ H2O (l)

13. 25.0 mL of 0.10 M nitric acid neutralized 40.0 mL of barium hydroxide. Determine theconcentration of the base. BALANCE!

___ HNO3 (aq) + ___ Ba(OH)2 (aq) ___ Ba(NO3)2 (aq) + ___ H2O (l)

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