Toxins Unit Review



Toxins Unit Review

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Acid and Bases

1. What are the colors produced with litmus paper for an acid, base, and neutral?

2. Find the pH of each solution and determine if it is an acid, base, or neutral substance.

a). [H+] = 0.0001 M b). [OH-]= 0.000001 M

c).[H+] = 1.0 x 10 -3 M d). [OH-] = 1.0 x 10 -9 M

e). [H+] = 1.0 x 10 -10 M f) [OH-] = 1.0 x 10 -4 M

g) pOH= 3.5 h) pOH= 7.7

3. What is the difference between the Arrhenius and BrØnstead-Lowry definition of an acid and base?

4. Label each substance acid, Arrhenius base, BrØnstead-Lowry base, or neutral.

a. HF b. HNO3 c. CH3NH2 d. NH3 e. N2H4

f. HC2H3O2 g. C3H6O h. LiCl i. C2H6 j. SrCl2

k. HI l. C2H4O m. H20 n. H3PO4 o. CH3OH

5. How do you neutralize an acid?

Solutions

6. Define a solute, solvent, and solution. What are two ways to make a solution?

7. How many moles of vinegar are in a 0.67M solution that is 1.2 L in volume?

8. What is the molarity of a solution of 2.8 moles nitric acid prepared in 250 mL water?

9. If you have 35g NaCl dissolved in 750 mL of water, what is the molarity?

10. 45g of Ca(OH)2 was used to make a 2.0M solution. How much water was used?

11. You have 250 mL of 0.75M solution of KF(aq), how many grams of KF was dissolved in this solution?

Chemical Reactions

12. What are the four types of chemicals reactions we have learned? Give an example of all four types.

13. Complete the following reactions and then balance them.

a. CuCl2 + Al2(SO3)3 → ______ + _______

b. Ba(OH)2 + LiF → ______ + _______

Moles

14. Answer the following questions about a mole.

a. How many atoms are in 1 mole of Au, gold?

b. How many molecules are in 2 mole of H2O, water?

c. How many atoms are in 0.5 moles of Fe, iron?

15. What is the molar mass of Al2(SO4)3?

16. Answer the following questions about the relationship between mole and mass.

a. How many moles are in 1.5 grams of H2O, water?

b. How many grams are 0.55 moles of H2O, water?

17. Answer the following questions about the relationship between moles, mass, and atoms.

a. How many molecules are in 66.0 grams of NaCl, sodium chloride?

b. How many grams are in 3.80 x 1022 atoms of Cu, Copper?

Stoichiometry

Use the following double displacement reaction to answer the following questions.

2 AlBr3 + 3 K2SO4 ( 6 KBr + Al2(SO4)3

18. How many moles of AlBr3, aluminum bromide, will produce 2.5 moles of KBr, potassium bromide?

19. How many grams of K2SO4, potassium sulfate, will be needed to produce 1.50 moles of Al2(SO4)3, aluminum sulfate?

20. How many moles of KBr, potassium bromide, will be produced if there is 25.0 grams of AlBr3, aluminum bromide?

21. How many grams of AlBr3, aluminum bromide, are needed to produce 175 grams of K2SO4, potassium sulfate?

** Make sure you still review all your notes, making sense, and exercise pages in your notebook.

Toxins Unit Review

ANSWER KEY

Acid and Bases

1. What are the colors produced with litmus paper for an acid, base, and neutral?

Acids turn red with litmus paper. Bases turn blue with litmus paper. Neutral substances does not change litmus paper.

2. Find the pH of each solution and determine if it is an acid, base, or neutral substance.

a). [H+] = 0.0001 M pH=4 Acid b). [OH-]= 0.000001 M pH= 8 Base

c).[H+] = 1.0 x 10 -3 M pH=3 Acid d). [OH-] = 1.0 x 10 -9 M pH=5 Acid

e). [H+] = 1.0 x 10 -10 M pH=10 Base f) [OH-] = 1.0 x 10 -4 M pH=10 Base

g) pOH= 3.5 pH=10.5 Base h) pOH= 7.7 pH=6.3 Acid

3. What is the difference between the Arrhenius and BrØnstead-Lowry definition of an acid and base? Arrhenius acid adds a hydrogen ion (H+) in solution and a BrØnsted-Lowry acid is a substance from which a proton is removed. So the definitions are similar. Arrhenius bases add hydroxide ions (OH-) to the solution and BrØnsted bases remove a proton from a substance like water. (Ex: NH3 + H2O → NH4+ + OH-)

4. Label each substance acid, Arrhenius base, BrØnstead-Lowry base, or neutral.

a. HF Acid b. HNO3 Acid c. CH3NH2 B-L Base d. NH3 B-L Base e. N2H4 B-L Base

f. HC2H3O2 Acid g. C3H6O Neutral h. LiCl Neutral i. C2H6 Neutral j. SrCl2 Neutral

k. HI Acid l. C2H4O Neutral m. H20 Neutral n. H3PO4 Acid o. CH3OH Neutral

5. How do you neutralize an acid? You neutralize an acid with a base. You can also add water to a strong acid so that it becomes a weak acid. Large amounts water can also make an acid become neutral.

Solutions

6. Define a solute, solvent, and solution. What are two ways to make a solution?

A solute is the substance of lesser amount that is being dissolved. The solvent is the greater amount substance (usually a liquid) in which the solute is dissolved into. A solution is when a solute is completely dissolved and dispersed in a solvent. For example, salt (solute) dissolves in water (solvent) to make a solution of salt water. You can make a solution by dissolving the solute (like salt) or you can take a made solution and dilute with water to the concentration you desire.

7. How many moles of vinegar are in a 0.67M solution that is 1.2 L in volume?

Use molarity triangle for the questions #7-10.

0.67 x 1.2 L = 0.80 moles vinegar

8. What is the molarity of a solution of 2.8 moles nitric acid prepared in 250 mL water?

250mL ÷ 1000 = 0.25 L

2.8 moles ÷ 0.25 L = 11 M nitric acid

9. If you have 35g NaCl dissolved in 750 mL of water, what is the molarity?

750mL ÷ 1000 = 0.75 L

35g ÷ 58.44 g/mol NaCl = 0.5989 moles NaCl

0.5989 moles ÷ 0.750 L = 0.79854 ≈ 0.80 M NaCl

10. 45g of Ca(OH)2 was used to make a 2.0M solution. How much water was used?

45g ÷ 74.10 g/mol Ca(OH)2 = 0.60729 moles Ca(OH)2

0.60729 moles ÷ 2.0 M = 0.30 L Ca(OH)2

11. You have 250 mL of 0.75M solution of KF(aq), how many grams of KF was dissolved in this solution?

250 mL÷1000 = 0.25 L

0.25 L x 0.75M = 0.1875 moles KF

0.1875 moles x 58.1g/mole = 10.89375 ≈ 11 g KCl

Chemical Reactions

12. What are the four types of chemicals reactions we have learned? Give an example of all four types.

Combination A + B → AB

Decomposition AB → A + B

Single Displacement AB + C → CB + A

Double Displacement AB + CD → AD + CB

13. Complete the following reactions and then balance them.

c. 3CuCl2 + Al2(SO3)3 → __3CuSO3____ + __2AlCl3_____

d. Ba(OH)2 + 2LiF → ___BaF2___ + __2LiOH_____

Moles

14. Answer the following questions about a mole.

b. How many atoms are in 1 mole of Au, gold? 6.02 x 1023 atoms Au

b. How many molecules are in 2 mole of H2O, water? 1.20 x 1024 molecules of water

c. How many atoms are in 0.5 moles of Fe, iron? 3.01x 1023 atoms Fe

15. What is the molar mass of Al2(SO4)3? 342.17 g/mol

16. Answer the following questions about the relationship between mole and mass.

a. How many moles are in 1.5 grams of H2O, water?

1.5 g ÷ 18.02 g/mol water = 0.083 moles of water

b. How many grams are 0.55 moles of H2O, water?

0.55 moles x 18.02 g/mol = 9.9 grams of water

17. Answer the following questions about the relationship between moles, mass, and atoms.

a. How many molecules are in 66.0 grams of NaCl, sodium chloride?

66.0 g NaCl x 1 mole x 6.02 x 1023 molecules = 6.80 x 1023 molecules NaCl

58.44 g 1 mole

b. How many grams are in 3.80 x 1022 atoms of Cu, Copper?

3.80 x 1022 atoms Cu x 1mole x 63.55g = 4.01 grams Cu

6.02 x 1023 atoms 1mole

Stoichiometry

Use the following double displacement reaction to answer the following questions.

2 AlBr3 + 3 K2SO4 ( 6 KBr + Al2(SO4)3

18. How many moles of AlBr3, aluminum bromide, will produce 2.5 moles of KBr, potassium bromide?

2.5 moles KBr x 2 moles AlBr3 = 0.83 moles AlBr3

6 moles KBr

19. How many grams of K2SO4, potassium sulfate, will be needed to produce 1.50 moles of Al2(SO4)3, aluminum sulfate?

1.5 moles Al2(SO4)3 x 3moles K2SO4 x 174.27 g K2SO4 = 784 g K2SO4

1mole Al2(SO4)3 1mole K2SO4

20. How many moles of KBr, potassium bromide, will be produced if there is 25.0 grams of AlBr3, aluminum bromide?

25.0 g AlBr3 x 1 moles AlBr3 x 6 moles KBr = 0.281 moles KBr

266.68 g AlBr3 2 moles AlBr3

21. How many grams of AlBr3, aluminum bromide, are needed to produce 175 grams of K2SO4, potassium sulfate?

175 g K2SO4 x 1 mole K2SO4 x 2 moles AlBr3 x 266.68 g AlBr3 = 179 g AlBr3

174.27 g K2SO4 3 moles K2SO4 1mole AlBr3

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