SOLUTIONS-Chemistry



12/5/14 Friday, Day 69

1. Take test

2. cw/hw Watch and take notes on the WHS SOLUTIONS video minutes 1-24.25 OR take notes on slides 1-22 of SOLUTIONS PPT

- complete worksheets 1-2

12/8/14 Monday, Day 70

1. Go over hw

2. Solutions

3. Solubility rules

4. Solubility/Solubility curve

5. Rate of solution

6. slides 23-41 should be viewed today

7. CW / HW: worksheets 3-4 all required

Video minutes 52.45-56.45 review this if needed

12/9/14 Tuesday, Day 71

1. Go over/check hw

2. Molarity

3. Dilutions

4. Slides 42-58

5. CW: Molarity (wks5)

Molarity dilutions (wks6)

6. HW Finish worksheets

Watching minutes 24.25 - 35 & 40-46.20 of the video is recommended (molality not required)

12/10/14 Wednesday, Day 72 Exam review can be checked

1. Be prepared for a quiz on solutions

2. Props. of acids and bases

3. Naming acids/bases (wks 7)

4. Bronsted-Lowry A/B (wks 8)

5. Conjugate A/B pair (wks 9)

6. Take home Acid/Base lab (B) (beneath wks 6)

7. hw – complete worksheets 7-9

12/11/13 Thursday, Day 73 Exam review can be checked

1. Go over homework

2. pH and pOH

4. hw: pH and pOH (wks 10, 11)

pH and pOH continues (wks 12)

12/12/14 Friday, Day 74 Exam review can be checked

1. Go over homework

2. Titration

3. Acid-Base Titration as demo

4. CW/HW A/B titration (13)

12/15/14 Monday, Day 75 Exam review can be checked

1. Go over hw

2. Review / prepare for test

3. Hw – organize packet

Make a study guide

12/16/14 Tuesday, Day 76

1. Test

SOLUBILITY (POLAR VS. NONPOLAR) WORKSHEET 1

Generally, “like dissolves like.” Polar molecules dissolve other polar molecules and ionic compounds. Nonpolar molecules dissolve other nonpolar molecules. Alcohols, which have characteristics of both, tend to dissolve in both types of solvents, but will not dissolve ionic solids.

Check the appropriate columns as to whether the solute is soluble in a polar or nonpolar solvent.

|SOLUTES |SOLVENTS |

| |Water CCl4 Alcohol |

|1. NaCl | | | |

|2. I2 | | | |

|3. ethanol | | | |

|4. benzene (C6H6) | | | |

|5. Br2 | | | |

|6. KNO3 | | | |

|7.octane (gasoline) | | | |

|8. Ca(OH)2 | | | |

ELECTROLYTES WORKSHEET 2

Electrolytes are substances that break up (dissociate or ionize) in water to produce ions. These ions are capable of conducting an electric current.

Generally, electrolytes consist of acids, bases and salts (ionic compounds).

Nonelectrolytes are usually covalent compounds, with the exception of acids/bases.

Classify the following compounds as either an electrolyte or a nonelectrolyte.

|Compound |Electrolyte |Nonelectrolyte |

|1. NaCl | | |

|2. CH3OH (methyl alcohol) | | |

|3. C3H5(OH)3 (glycerol) | | |

|4. HCl | | |

|5. C6H12O6 (sugar) | | |

|6. NaOH | | |

|7. C2H5OH (ethyl alcohol) | | |

|8. HC2H3O2 (acetic acid) | | |

|9. NH4OH | | |

|10. H2SO4 | | |

SOLUBILITY CURVES WORKSHEET 3

Answer the following questions based on the solubility curve.

1. Which salt is least soluble in water at 200 C? ______________

2. How many grams of potassium chloride can be dissolved in 200 g of water at 800 C? _______________

3. At 4Q0 C, how much potassium nitrate can be dissolved in 300 g of water? _______________________

4. Which salt shows the least change in solubility from O0 - 1000 C? _____________________________

5. At 3O0 C, 90 g of sodium nitrate is dissolved in 100g of water. Is this solution saturated, unsaturated or supersaturated? _____________________

6. A saturated solution of potassium chlorate is formed from one hundred grams of water. If the saturated solution is cooled from 800 C to 5O0 C, how many grams of precipitate are formed? ________________

7. What compound shows a decrease in solubility from Q0 to 1000C? ______________

8. Which salt is most soluble at 100 C? _________________

9. Which salt is least soluble at 5O0 C? __________________

10. Which salt is least soluble at 9O0 C? __________________

Worksheet 4

Precipitation Reactions – Solubility rules

|Will a precipitate form if solutions of potassium sulfate and barium nitrate are combined? If so, write the balanced equation including all |

|states. |

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|Will a precipitate form if solutions of potassium nitrate and magnesium sulfate are combined? If so, write the balanced equation including |

|all states. |

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|Will a precipitate form if solutions of barium chloride and sodium sulfate are combined? If so, write the balanced equation including all |

|states. |

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|Write the balanced formula equation (includes states) that shows the possible products of a double displacement reaction between calcium |

|nitrate(aq) and sodium chloride(aq). |

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|Write the balanced formula equation (includes states) that shows the possible products of a double displacement reaction between mercury (II)|

|chloride(aq) and potassium sulfide(aq). |

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|Write the balanced formula equation (includes states) that shows the possible products of a double displacement reaction between sodium |

|carbonate(aq) and calcium chloride(aq). |

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|Write the balanced formula equation (includes states) that shows the possible products of a double displacement reaction between copper (II) |

|chloride(aq) and potassium sulfide(aq). |

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|Copper (II) chloride and lead (II) nitrate react in aqueous solutions. Write the balanced chemical equation. If 13.45 g of each reactant |

|react, what is the maximum amount of precipitate that could be formed? |

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MOLARITY WORKSHEET 5

SOLVE THE PROBLEMS BELOW.

|What is the molarity of a solution in which 58 g of NaCl are dissolved in 1.0 L of solution? |

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| What is the molarity of a solution in which 10.0 g of AgNO3 is dissolved in 500. mL of solution? |

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|How many grams of KNO3 should be used to prepare 2.00 L of a 0.500 M solution? |

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|To what volume should 5.0 g of KCl be diluted in order to prepare a 0.25 M solution? |

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|How many grams of CuSO4 • 5H2O are needed to prepare 100. mL of a 0.10 M solution? |

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MOLARITY BY DILUTION WORKSHEET 6

Acids are usually acquired form chemical supply houses in concentrated form. These acids are diluted to the desired concentration by adding water. Solve the following problems.

| How much concentrated 18M sulfuric acid is needed to prepare 250 mL of a 6.0 M solution? |

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| How much concentrated 12 M hydrochloric acid is needed to prepare 100. mL of a 2.0M solution? |

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| To what volume should 25mL of 15M nitric acid be diluted to prepare a 3.0M solution? |

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| To approximately how much water should 50.mL of 12M hydrochloric acid be added to produce a 4.0M solution? |

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| To how much water should 100. mL of 18M sulfuric acid be added to prepare a 1.5M solution? |

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TAKE HOME ACID/BASE LAB

For homework you are to test eight or more of the following substances to tell if it is an acid, base or a neutral substance. In the school lab we could not taste the food substances but at home you may have tasted the food items and could find some relationship between the tastes.

MATERIAL: red and blue litmus paper, vinegar, mustard, pickle juice, orange juice, grapefruit juice, lemon juice, cranberry juice, grape juice, sour mild or buttermilk, yogurt, lemon-lime soda, fruit-flavored gelatin in liquid form, milk, water, household ammonia, drain cleaner, lime (spice), lye, liquid antacid medication, milk of magnesia, oven cleaner.

PROCEDURE:

1. Place a small quantity of each of your substances in a small bowl or saucer. (The same container may be repeatedly used but be sure to wash thoroughly between substances.)

2. If the substance is in solid form, dissolve a small amount in water before testing.

3. Test the substance with red and blue litmus paper. (If blue turns red it is an acid. If red litmus turns blue it is a base. Neither paper will change if it is neutral.)

4. Record both the substance and whether it is an acid or base.

5. Bring your results to class.

QUESTION: Do you recognize the ingredients in any substance as an acid or base.

Do you recognize a similarity in taste (food items only), or use of any of these products?

What are other household substances you could test?

Test those items which you have.

Naming Acids and Bases WORKSHEET 7

Name the following acids/bases.

1. HNO3 __________________________________

2. HCl __________________________________

3. H2SO4 __________________________________

4. H2SO3 __________________________________

5. H2S __________________________________

6. HC2H3O2__________________________________

7. HBr __________________________________

8. H2CO3 __________________________________

9. NaOH __________________________________

10. HNO2 __________________________________

11. H3PO4 __________________________________

12. Ba(OH)2 __________________________________

13. Zn(OH)2 __________________________________

14. H3PO3 __________________________________

15. Al(OH)3 __________________________________

Write the formulas of the following acids/bases.

16. Sulfuric acid __________________________________

17. nitric acid ________________________

18. hydrochloric acid ________________________

19. acetic acid ________________________

20. hydrofluoric acid ________________________

21. phosphorous acid ________________________

22. carbonic acid ________________________

23. nitrous acid ________________________

24. oxalaic acid ________________________

25. hydrosulfuric acid________________________

26. ammonium hydroxide_____________________

27. iron(III) hydroxide________________________

28. potassium hydorixe_______________________

29. chloric acid ________________________

30. chlorous acid ________________________

Bronsted-Lowry Acids and Bases WORKSHEET 8

According to Bronsted-Lowry theory, an acid is a proton (H+) donor, and a base is a proton acceptor.

Label the Bronsted-Lowry acids and bases in the following reactions and show the direction of proton transfer.

1. H2O + H2O (( H3O+ + OH-

2. H2SO4 + OH- (( HSO4- + H2O

3. HSO4- + OH- (( SO4-2 + H2O+

4. OH- + H3O+ (( H2O + H2O

5. NH3 + H2O (( NH4+ + OH-

Bronsted-Lowry Acids and Bases WORKSHEET9

Complete the table with the conjugate acid base pairs.

| |Acid |Base |Equation |

|Sample |H2SO4 |HSO4- |H2SO4 (( H+ + HSO4- |

| |H3PO4 | | |

| | |F- | |

| |NO3- | | |

| |H2PO4- | | |

| |H2O | | |

| | |SO4-2 | |

| |HPO4-2 | | |

| |NH4+ | | |

| | |H2O | |

| | |HSO4+ | |

1. Which is a stronger base, HSO4- or H2PO4-?________________________

2. Which is a weaker base, Cl- or NO2-? ________________________

Acids, Bases or Salt WORKSHEET 10

Classify each of the following compounds as an acid, base or salt. Then, indicate whether each acid and base is strong or weak.

1. HNO3 ______________________________ _________________________________

2. NaOH ______________________________ _________________________________

3. NaNO3 ______________________________ _________________________________

4. HCl ______________________________ _________________________________

5. KCl ______________________________ _________________________________

6. Ba(OH)2 ______________________________ _________________________________

7. KOH ______________________________ _________________________________

8. H2S ______________________________ _________________________________

9. Al(NO3)3 ______________________________ _________________________________

10. H2SO4 ______________________________ _________________________________

11. CaCl2 ______________________________ _________________________________

12. H3PO4 ______________________________ _________________________________

13. CaCl2 ______________________________ _________________________________

14. Mg(OH)2 ______________________________ _________________________________

15. H2CO3 ______________________________ _________________________________

16. NH4OH ______________________________ _________________________________

17. NH4Cl ______________________________ _________________________________

18. HBr ______________________________ _________________________________

19. FeBr3 ______________________________ _________________________________

20. HF ______________________________ _________________________________

pH and pOH WORKSHEET 11

Complete the following chart.

| |[H+] |pH |[OH-] |pOH |Acidic or Basic |

|Sample |10-5M |5 |10-9M |9 |Acidic |

| | |7 | | | |

| | | |10-4M | | |

| |10-2M | | | | |

| | | | |11 | |

| | |12 | | | |

| | | |10-5M | | |

| |10-11M | | | | |

| | | | |13 | |

| | |6 | | | |

| | | | |2 | |

pH and pOH continued WORKSHEET 12

Calculate the pH of the solutions below.

1. 0.01 MHCl

2. 0.0010 M NaOH

3. 0.050 M Ca(OH)2

4. 0.030 M HBr

5. 0.150 M KOH

6. 2.0 M HC2H3O2 (Assume 5.0% dissociation)

7. 3.0 M HF (Assume 10. % dissociation)

8. 0.50 M HNO3

9. 2.50 M NH4OH (Assume 5.0% dissociation)

10. 5.0 M HNO2 (Assume 1.0% dissociation)

A/B Titrations WORKSHEET 13

To determine the concentration of an acid (or base), we can react it with a base (or acid) of known conentration until it is completely neutralized. This point of exact neutralization, known as the end point, is neoted by the change in color of the indicator..

1. A 25.0 mL sample of HCl was titrated to the endpoint with 15.0mL of 2.0 M NaOH. What was the molarity of the HCl? 1.2 M

2. A 10.0 mL sample of H2SO4 was exactly neutraized by 13.5 mL of 1.0 M KOH. What is the molarity of the H2SO4? 0.68M

3. How much 1.5M NaOH is necessary to exactly neutralize 20.0 mL of 2.5M H3PO4? 1.0E2 mL

4. How much of 0.5 M HNO3 is necessary to tirate 25.0mL of 0.05M Ca(OH)2 solution to the endpoint? 5mL

5. What is the molarity of a NaOH solution if 15.0mL is exactly neutralized by 7.5mL of a 0.02M HC2H3O2 solution? 0.01M

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Take notes on PowerPoint OR on You Tube video: WHS Solutions

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