Tuesday, May 31

Section 5: Complete your acid/base packet and study. Answer keys can be found under homework docs.

Friday, May 27

Sections 2H & 4: Complete your acid/base packet and study. Answer keys can be found under homework docs. Enjoy your 3 day weekend!

p.s. start studying for the final! go over old test and quizzes!!!

Thursday, May 26

Sections 2H & 5: Read chapter 15, section 1 of your textbook. Then, answer section review questions 1-5 on page 509. 

Wednesday, May 25

Section 4: Read chapter 15, section 1 of your textbook. Then, answer section review questions 1-5 on page 509. 

Section 5: Answer the questions below in your notebook. Please note that I have given some sample answers. Also, here's a video on acid/base naming, if you found our last homework confusing: Naming Acids and Bases, Chemistry Tutorial CLEAR & SIMPLE

Given the following reactions label the acid, base, conjugate acid and conjugate base.

a. HCO₃^-       +          H₂O     →        H₃O⁺   +          CO₃^2-

b. HCl                  +          H₂O     →        H₃O⁺   +          Cl^-

c. CH₃CO₂H        +          NaOH →        NaCH₃CO₂     +          H₂O

d. NH₄Cl            +          NaH₂PO₄         →        NH₃     +          H₃PO₄ +         NaCl

Name the following acids and bases:

1)         NaOH 

2)         H2SO3 

3)         H2S 

4)         H3PO4 

5)         NH3       

6)         HCN    

7)         Ca(OH)2 

8)         Fe(OH)3  

9)         H3P      

Write the formulas of the following acids and bases:

10)       hydrofluoric acid

11)       hydroselenic acid 

12)       carbonic acid 

13)       lithium hydroxide 

14)       nitrous acid

15)       cobalt (II) hydroxide

16)       sulfuric acid   

17)       beryllium hydroxide

18)       hydrobromic acid

Tuesday, May 24

Sections 2H & 4: Answer the questions below in your notebook. Please note that I have given some sample answers. Also, here's a video on acid/base naming, if you found our last homework confusing: Naming Acids and Bases, Chemistry Tutorial CLEAR & SIMPLE

Given the following reactions label the acid, base, conjugate acid and conjugate base.

a. HCO₃^-       +          H₂O     →        H₃O⁺   +          CO₃^2-

b. HCl                  +          H₂O     →        H₃O⁺   +          Cl^-

c. CH₃CO₂H        +          NaOH →        NaCH₃CO₂     +          H₂O

d. NH₄Cl            +          NaH₂PO₄         →        NH₃     +          H₃PO₄ +          NaCl

Name the following acids and bases:

1)         NaOH 

2)         H2SO3 

3)         H2S 

4)         H3PO4 

5)         NH3       

6)         HCN    

7)         Ca(OH)2 

8)         Fe(OH)3  

9)         H3P      

Write the formulas of the following acids and bases:

10)       hydrofluoric acid

11)       hydroselenic acid 

12)       carbonic acid 

13)       lithium hydroxide 

14)       nitrous acid

15)       cobalt (II) hydroxide

16)       sulfuric acid   

17)       beryllium hydroxide

18)       hydrobromic acid

Monday, May 24

Section 5: Use your textbook (ch. 14) and the resources at the bottom of this webpage to help you answer the following in your notebook:

1) Explain the difference between a strong acid and a weak acid. Do the same for bases. Give examples.

2) Acid-Base Theories

Theory:

Definition: 

Example:

Theory:

Definition:

Example:

Theory:

Definition:

Example:

3) Acid-Base Nomenclature

The three steps for naming a binary acid are:

            1)

            2)

            3)

  

Practice:

H₂S

HF

HI

The following is an example of what kind of acid? H₃PO₄

Friday, May 20

Section 2H & 4: Use your textbook (ch. 14) and the resources at the bottom of this webpage to help you answer the following in your notebook:

1) Explain the difference between a strong acid and a weak acid. Do the same for bases. Give examples.

2) Acid-Base Theories

Theory:

Definition: 

Example:

Theory:

Definition:

Example:

Theory:

Definition:

Example:

3) Acid-Base Nomenclature

The three steps for naming a binary acid are:

            1)

            2)

            3)

  

Practice:

H₂S

HF

HI

The following is an example of what kind of acid? H₃PO₄

Thursday, May 19

Sections 2H & 5: Watch this video before our next class: Acid - Base Intro

Wednesday, May 18

Section 5: Answer the questions below and study for your solutions quiz.

1) If I add 25 mL of water to 125 mL of a 0.15 M NaOH solution, what will the molarity of the diluted solution be?

2) If I add water to 100 mL of a 0.15 M NaOH solution until the final volume is 150 mL, what will the molarity of the diluted solution be?

3) How much 0.05 M HCl solution can be made by diluting 250 mL of 10 M HCl?

4) I have 345 mL of a 1.5 M NaCl solution. If I boil the water until the volume of the solution is 250 mL, what will the molarity of the solution be?

5) How much water would I need to add to 500 mL of a 2.4 M KCl solution to make a 1.0 M solution?

Section 4: Watch this video before our next class: Acid - Base Intro

Tuesday, May 17

Section 4: Answer the questions below and study for your solutions quiz.

1) If I add 25 mL of water to 125 mL of a 0.15 M NaOH solution, what will the molarity of the diluted solution be?

2) If I add water to 100 mL of a 0.15 M NaOH solution until the final volume is 150 mL, what will the molarity of the diluted solution be?

3) How much 0.05 M HCl solution can be made by diluting 250 mL of 10 M HCl?

4) I have 345 mL of a 1.5 M NaCl solution. If I boil the water until the volume of the solution is 250 mL, what will the molarity of the solution be?

5) How much water would I need to add to 500 mL of a 2.4 M KCl solution to make a 1.0 M solution?

Monday, May 16

Sections 2H & 5: Answer the following questions in your notebook.

Molarity = moles of solute/L of solution

1. What does molarity mean?

2. What is the molarity of a solution that contains 4.53 moles of lithium nitrate in 2.85 liters of solution?

3. What is the molarity of a solution that contains 0.00372 moles hydrochloric acid in 2.39 x 10-2 liters of solution?

4. A flask contains 85.5 g C₁₂H₂₂O₁₁ (sucrose) in 1.00 liters of solution. What is the molarity?

5. A beaker contains 214.2 grams osmium (III) fluoride in 0.0673 liters of solution. What is the molarity?

6. Calculate the molarity if a flask contains 1.54 moles potassium sulfate in 125 ml of solution.

7. A chalice contains 36.45 grams ammonium chlorite in 2.36 liters of solution - calculate the molarity.

**** SOLUTIONS QUIZ ALERT:

Section 4 - Wednesday

Sections 2H & 5 - Thursday

Thursday, May 12

Section 2H: If you were not in class today, you must stop by tomorrow during CP for a few minutes to collect your chromatography lab data. You will complete the lab over the weekend. 

Section 4: Finish your lab and answer the following questions in your notebook. You should use the equation we used at the end of class (also, never forget about your textbook - we're in chapter 12!):

Molarity = moles of solute/L of solution 

1.      What does molarity mean? 

2.      What is the molarity of a solution that contains 4.53 moles of lithium nitrate in 2.85 liters of solution?

3.      What is the molarity of a solution that contains 0.00372 moles hydrochloric acid in 2.39 x 10^-2 liters of solution?

4.      A flask contains 85.5 g C₁₂H₂₂O₁₁ (sucrose) in 1.00 liters of solution.  What is the molarity?

5.      A beaker contains 214.2 grams osmium (III) fluoride in 0.0673 liters of solution.  What is the molarity?

6.      Calculate the molarity if a flask contains 1.54 moles potassium sulfate in 125 ml of solution.

7.      A chalice contains 36.45 grams ammonium chlorite in 2.36 liters of solution - calculate the molarity.

Wednesday, May 11

Sections 5: Use the Salts & Solubility phet simulation (link found here) to complete the FIRST PAGE ONLY of the worksheet posted under homework docs.

Also, answer the following two questions in your notebook:

1) On the solubility curve, for most substances, as temperature increases, solubility increases. Why do you think this happens?

2) Two of the curves trend in the opposite direction, these substances are gases. Why do you think gas solubility decreases when temperature increases?

Tuesday, May 10

Sections 2H & 4: Use the Salts & Solubility phet simulation (link found here) to complete the FIRST PAGE ONLY of the worksheet posted under homework docs.

Monday, May 9

Sections 2H & 5: Watch this video: Solubility Curves, and then answer the questions on the solubility curves worksheet you got at the end of class. If you're confused, don't worry, work in pencil - we will go over everything next class

Friday, May 6

Section 4: Watch this video: Solubility Curves, and then answer the questions on the solubility curves worksheet you got at the end of class. If you're confused, don't worry, work in pencil - we will go over everything next class.

Section 5: Based on your textbook reading and the notes we took in class today, answer the following questions:

1) What’s the difference between a solution, a suspension, and a colloid? Give examples of each.

2) What does “like dissolve like” mean?

3) Why don’t oil and vinegar mix? You should discuss this in terms of what happens at a molecular level.

4) Make a drawing of the particles in an NaCl solution to show why this solution conducts electricity. Then, make a drawing of a sugar solution to show why this solution does NOT conduct electricity.

5) Do you expect a packet of sugar to dissolve fast in hot tea or in cold tea? Why?

6) If a warm bottle of soda and a cold bottle of soda are left open, which will go flat first? Why?

7) You are eating pasta with olive oil and you accidentally get some oil on your shirt. What would be the best way to get the stain out? Should you just blot it with water? Why or why not?

Thursday, May 5

Sections 2H & 4: Based on your textbook reading and the notes we took in class today, answer the following questions:

1) What’s the difference between a solution, a suspension, and a colloid? Give examples of each.

2) What does “like dissolve like” mean?

3) Why don’t oil and vinegar mix? You should discuss this in terms of what happens at a molecular level.

4) Make a drawing of the particles in an NaCl solution to show why this solution conducts electricity. Then, make a drawing of a sugar solution to show why this solution does NOT conduct electricity.

5) Do you expect a packet of sugar to dissolve fast in hot tea or in cold tea? Why?

6) If a warm bottle of soda and a cold bottle of soda are left open, which will go flat first? Why?

7) You are eating pasta with olive oil and you accidentally get some oil on your shirt. What would be the best way to get the stain out? Should you just blot it with water? Why or why not?

Wednesday, May 4

All Sections: Complete the Chapter 12 introduction worksheet under 'homework documents'. You must use your textbook (ch 12) for this assignment. You DO NOT need to print out the worksheet - you are welcome to write all the definitions and your answers in your notebook.

Tuesday, May 3

Section 5: Study! Don't forget what a useful tool your textbook is for answering gas law questions (ch. 11)!

Remember: Extra credit work is due in class tomorrow.