Name ___________

WPHS ChemistryUnit 4

Chemical Reactions

Bergmann-Sams

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Name ___________

Chemistry: Unit 4 Outline: Chemical ReactionsAssignment WB Page Number Score Out ofPodcast 4.1 (CB 1-3) Online Worksheet A pg 7-9 Podcast 4.2 (CB 5-9) Online Demo: Types of Reactions In Class

Worksheet BPg 10-12

Lab: Small Scale Single Replacement Pg 4 100Podcast 4.3 (CB 11-13) Online Worksheet C Pg 13-15 Lab: Small Scale Double Replacement

Pg 5-6 100

Podcast 4.4 (CB 15-17) Online Worksheet D Pg 16 Technology Lab Teacher Handout 100Worksheet E (Review) Pg 17-20 Unit 4 Exam In Class 100

(You must score 85/100 on all assignments with a number to move to the next unit. For those assignments with a check, you need to do it to the satisfaction of your teacher)

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Name ___________

Unit 4 Chemical Reactions: Composition Book Outline8-1: Describing Chemical Change1 Converting Word Equations into Formulaic Equations (pg 203-206)

Question: Answer the following question What is the difference between a word equation and a chemical equation

Define Catalyst

Copy: Table 8.1 on page 2063 Balancing Chemical Equations (pg 207-211)

Read the section and: “Balancing Chemical Equations” and come up with an analogy like the bicycle and write the balanced chemical equation.Leave the rest of the page blank

8-2: Types of Chemical Equations5 Reaction Types (pgs 212-216)

Define: Combination Reactions, Decomposition Reaction, Single Replacement Reaction, Double Replacement Reaction, Combustion Reaction Do one at a time with the examples underneath eachList: Two examples of each type (written with formulas—not words)

7 Predicting Single Replacement ReactionsCopy: Table 8.2 on page 217

9 Predicting Single Replacement ReactionsLeave blank for teacher notes

11 Predicting and Writing Double Replacement ReactionsLeave blank for teacher notes

13 Predicting and Writing Double Replacement ReactionsLeave blank for teacher notes

8-3: Reactions in Aqueous Solutions15 Ionic and Net Ionic Equations (pg 225-228)

Leave blank for teacher notes17 Ionic and Net Ionic Equations (pg 225-228)

Leave blank for teacher notes

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Name ___________

Activity Series of Metals LabPurpose: To observe an activity series of different metals.

Procedure: 1. Using the well plates, select a row of wells for each solution listed in the data

table. Make sure that you write down which letter and number your wells are for each solution. There should be three wells for each solution (one of the three for each of the metals).

2. Put five drops of each solution in the wells chosen for that solution. 3. Put one piece of magnesium in one of the wells for each solution. For example,

you should have a well of copper sulfate with magnesium in it, a well of magnesium sulfate with magnesium in it, and a well of sodium chloride with magnesium in it, a well of zinc sulfate with magnesium in it and a well of silver nitrate with magnesium in it.

4. Repeat step 3 with copper instead of magnesium.5. Repeat step 3 with zinc instead of magnesium.6. After l minute has passed, make observations of both the metal strips and the

solutions. Put these observations in a data table in your comp book that looks like the one below. Label this data table as 1 minute.

7. After 5 total minutes have passed, take another set of observations. Make another data table like the one below and label it 5 minutes.

8. After 15 total minutes have passed, take another set of observations. Again, make another data table and label it 15 minutes.

Data Table:CuSO4 MgSO4 NaCl ZnCl2 AgNO3

Cu metalMg metalZn metal

Analysis Questions: (as always with labs, these questions should be written in complete sentences)

1. Why doesn’t the metal react with the same metal solution?2. In which wells did the appearance of the metal change? Be sure to tell your

teacher what both of the reactants of the well were.3. Write a balanced equation for each visible reaction between a metal and it’s

solution. Be sure to identify what types of reactions these are.4. Based on the results of your experiment construct your own activity series for the

five metals. Put the most active metal first and the least active metal last. Be sure to include your reasoning for your rankings.

5. In a short summary paragraph, describe and explain the patterns that you see in your reaction table.

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Name ___________Double Replacement Lab

Use Beral Pipets to add each solution on the grid. For those that have a reaction occur, describe the reaction. For those that do not, record NVR (No visible reaction) When done you need to:

1. Write out each complete reaction that occurs (you must balance it)2. Write out the ionic equation for each reaction that occurs.3. Write out the net-ionic equation for each reaction that occurs.

Put “flimsy” over the top of this page and mix all of the chemicals. Do not mix the same chemical with the same.Chemical NaCl AgNO3 Pb(NO3)2 Na2SO4 BaCl2 NaOH Na3PO4

NaCl

X X X X X XAgNO3

X X X X X XPb(NO3)2

X X X X X XNa2SO4

X X X X XBaCl2

X X X X X XNaOH

X X X X X XNa3PO4

X X X X X X

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Name ___________Data Table: Write in your observations here.Chemical NaCl AgNO3 Pb(NO3)2 Na2SO4 BaCl2 NaOH Na3PO4

NaCl

AgNO3

Pb(NO3)2

Na2SO4

BaCl2

NaOH

Na3PO4

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Name ___________Equation Worksheet A:Balancing Chemical Equations

Balance the following equations and identify the type of reaction: (Double Replacement, Single Replacement, Combination, Decomposition, or Combustion)

1) __HgO __Hg + __O2 Type: ________________

2) __HCl + __Mg __H2 + MgCl2 Type: ________________

3) __CH4 + __O2 __CO2 + __H2O Type: ________________

4) __C6H12O6 + __O2 __CO2 + __H2O Type: ________________

5) __H2 + __O2 __H2O Type: ________________

6) __H2 + __N2 __NH3 Type: ________________

7) __NO + __O2 __NO2 Type: ________________

8) __Al2O3 __Al + __O2 Type: ________________

9) __CaO + __H2O __Ca(OH)2 Type: ________________

10) Hydrogen gas reacts with iodine to produce hydroiodic acid.Type: ________________

11) Sulfur reacts with oxygen to produce sulfur dioxide.Type: ________________

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Name ___________12) Calcium acetate reacts with sodium carbonate to produce calcium carbonate and

sodium acetate.Type: ________________

13) Write the chemical reaction that shows how rust forms: (Iron III oxide)Type: ________________

14) Iron combines with oxygen and water to form iron (III) hydroxideType: ________________

15) Sulfur trioxide is bubbled through water to produce sulfuric acidType: ________________

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Name ___________16) Copper metal is made by treating copper ore the following way: Copper (II)

sulfide is heated with carbon and oxygen to produce copper and sulfur dioxide and carbon dioxide.

Type: ________________

17) Copper-bottomed cooking pans turn black because copper combines with oxygen to form copper (II) oxide.

Type: ________________

18) Magnesium hydroxide neutralizes stomach acid, HCl, to produce magnesium chloride and water.

Type: ________________

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Name ___________Equation Worksheet B: Single Replacement Reactions

A. Predict the products and balance the following single replacement reactions. If no reaction occurs write N.R. For transition metals use the following charges:

Iron: Fe3+ Mercury: Hg2+

Lead: Pb4+ Copper: Cu1+

1. Fe + CuCl2

2. Hg + Sn(SO4)2

3. Ba + Ni3(PO4)2

4. Pb + Au(NO3)3

5. Li + HOH

6. K + AgCl

7. Ca + NaOH

8. Cu + Fe(OH)3

9. Fe + Cu(OH)2

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Name ___________

10. Lead II Chloride + Magnesium

11. Barium Nitrate + Zinc

12. Potassium + Tin IV Nitrate

13. Copper + Silver Nitrate

14. Sodium Phosphate + Potassium

15. Gold + Hydrochloric acid

16. Magnesium + Aluminum Hydroxide

17. Iron + Copper II Sulfate

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Name ___________

18. Iron + Nickel II Iodide

19. Sodium Permanganate + Calcium

20. hydrochloric acid + Zinc

21. Aluminum + Iron II dichromate

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Name ___________Equation Worksheet C: Double Replacement Reactions

Complete and Balance the following reactions. If no reaction occurs then write N.R.

1) Na2SO4 (aq) + Ba(NO3)2(aq) ---->

2) NaNO3(aq) + NH4Cl(aq) ----->

3) Pb(NO3)2 (aq) + Na2CrO4(aq)

4) ZnCl2(aq) + K2CO3(aq) ---->

5) Ammonium Chloride + Silver Nitrate ------>

6) Barium Acetate + Copper II Chromate

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Name ___________

7) Solutions of Silver Nitrate and ammonium chloride are mixed

8) Solutions of Lead II nitrate and Sodium Chloride are mixed

9) Solutions of zinc sulfate and magnesium chloride are mixed

10) Solutions of Ammonium phosphate and Zinc Chlorate are mixed

11) Solutions of Aluminum bromide and Iron II Iodide are mixed

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Name ___________

12) Solutions of sodium sulfide and Iron II Chlorate are mixed

13) Solutions of copper II bromide and potassium phosphate are mixed

14) Solutions of barium acetate and zinc sulfate are mixed

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Name ___________ Equation Worksheet D: Net Ionic Equation WorksheetFor the following reactions write the:

a. Complete Equation (Indicate states): Balanceb. Ionic Equationc. Net Ionic Equation

1. ZnCl2 (aq) + Na2S (aq) ZnS(s) + NaCl(aq)

2. (NH4)3PO4 + AgNO3

3. Magnesium Nitrate + Potassium phosphate Magnesium Phosphate (s) + Potassium Nitrate.

4. Lead II Acetate + Potassium Iodide

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Name ___________

Equations Worksheet E: Mixed Types of Reactions

Directions: For each of the following reactions:1) Complete the reaction (Put NR if no reaction takes place)2) Balance it3) Identify the type of reaction (Single Replacement, combination, double replacement,

decomposition, or combustion)4) Indicate states of matter for each reaction

1) NaCl + AgNO3

2) Fe + CuSO4

3) C4H10 + O2

4) Ba(NO3)2 + Na2SO4

5) AgNO3 + Li

6) LiBr + Cu

7) MgS + NaOH

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Name ___________

8) Hg + LiCl

9) Li + HgCl2

10) C3H8 + O2

11) Ammonium Nitrate is added to sodium chloride

12) Lithium Chloride is added to Zinc Phosphate

13) Zinc is added to lithium chloride

14) Iron is added to a solution of silver nitrate

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Name ___________

15) A solution of copper II sulfate is added to an iron nail

16) Octane (C8H18) is burned in air

17) A solution of Tin IV sulfate is added to a solution of ammonium hydroxide

18) Sodium hydroxide is added to hydrochloric acid

19) Calcium hydroxide is added to sulfuric acid

20) Nickel is added to hydrochloric acid

21) Strontium is added to water

22) Hydrochloric acid is added to copper metal

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Name ___________

23) Solid bismuth is added to a solution of barium hydroxide.

24) Methanol (CH3OH) is burned in air

25) Solid gold is added to hydrochloric acid

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Name ___________Name: ______________

Period: ______________

Balancing Reactions WorksheetSynthesis and Decomposition

Part A (Review): Balance the following reactions and indicate whether they are synthesis or decomposition reactions.

1. SO3 + H2O ---> H2SO4 Type:_____________2. H2O ---> H2 + O2 Type:_____________3. HgO ---> Hg + O2 Type:_____________4. Al2O3(s) ---> Al(s) + O2(g) Type:_____________5. P + O2 ---> P2O5 Type:_____________

Part B: Predict the products and indicate type (include states):1. KBr ---> Type: _________

2. Li + Cl2 ---> Type: _________3. Rb2CO3 ---> Type: _________4. NiO ---> Type: _________5. CO2 + H2O---> Type: _________

Part C: Predict the products, balance, include states, and indicate type.

1. Potassium Chlorate is heated vigorously Type: _________

2. Molten sodium is reacted with chlorine gas Type: _________

3. Calcium is added to water Type: _________

4. Zinc carbonate is heate Type: _________

5. Aluminum chloride decomposes into it's elements Type: _________

6. Cesium hydroxide is heated Type: _________

7. Sulfurous Acid is heated Type: _________

8. Potassium and Bromine are reacted Type: _________

9. Potassium Oxide and Carbon dioxide react Type: _________

10. Calcium chlorate is heated Type: _________

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Name ___________11. Sodium hydroxide is heated Type: _________

12. Iodine reacts with hydrogen Type: _________

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Name ___________Balancing Chemical Equations Worksheet 1 Name

Period

Balance the following equations:

1. 2HgO 2Hg + O2

2. HCl + Mg H2 + MgCl2

3. CH4 + 2O2 CO2 + 2H2O4. C6H12O6 + 6O2 6CO2 + 6H2O5. 2H2 + O2 2H2O6. 2H2 + Cl2 2HCl7. 3H2 + N2 2NH3

8. 2 NO + O2 2NO2

9. 3Al2O3 4Al +2O2

10. CaO + H2O Ca(OH)2 already balanced11. Hydrogen gas reacts with iodine to produce hydrogen iodide.

H2+ I2 2HI

12. Sulfur reacts with oxygen to produce sulfur dioxide.S + O2 SO2

13. Calcium acetate reacts with sodium carbonate to produce calcium carbonate and sodium acetate.

Ca(C2H3O2)2 + Na2CO3 2NaC2H3O2 +CaCO3

14. Write the chemical reaction that shows how rust forms:4Fe + 3O2 2Fe2O3

15. Iron combines with oxygen and water to form iron (III) hydroxideFe + O2 + 6H2O 4Fe(OH)3

16. Sulfur trioxide is bubbled through water to produce hydrogen sulfateSO3+ H2O H2SO4 already balanced

17. Copper metal is made by treating copper ore the following way: Copper (II) sulfide is heated with carbon and oxygen to produce copper and sulfur

dioxide and carbon dioxide. CuS +C + 4O2 SO2 + CO2 + Cu

Copper-bottomed cooking pans turn black because copper combines with oxygen to form copper (II) oxide.

2Cu + O2 2CuO

18. Any Group I metal reacts with water to produce hydrogen gas and the metal hydroxide. Write the reaction that occurs when rubidium is dropped in water.

2Rb + 2HOH 2RbOH + H2

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Name ___________

19. Magnesium hydroxide neutralizes stomach acid, HCl, to produce magnesium chloride and water.

Mg(OH)2 + 2HCl MgCl2 + 2H2O

20. Limestone is dissolved by acid (Remember our carbonate lab in September?). This is why statues are dissolved by acid rain. First, the acid is formed in the atmosphere. Second, it falls on the statue and dissolves it. Write two reactions that show how thishappens. First, nitrogen dioxide reacts with water to form hydrogen nitrate. Second, hydrogen nitrate combines with calcium carbonate to form carbon dioxide and water and calcium nitrate.

4NO2+ 2H2O 4HNO3 balancing is difficult extra credit if you can2HNO3 + CaCO3 Ca(NO3)2+ H2O+ CO2

Balancing Reactions WorksheetSynthesis and Decomposition

Part A (Review): Balance the following reactions and indicate whether they are synthesis or decomposition reactions.

1. SO3 + H2O ---> H2SO4 balanced Type: synthesis

2. 2H2O ---> 2H2 + O2 Type: decomposition

3. 2HgO ---> 2Hg + O2 Type: decomposition4. 2Al2O3(s) ---> 4Al(s) + 3O2(g) Type: Decomposition

5. 4P + 5O2 ---> 2P2O5 Type: Synthesis

Part B: Predict the products and indicate type (include states):1. 2KBr ---> 2K + Br2 Type: decomp2. 2Li + Cl2 ---> 2LiCl Type: synth3. Rb2CO3 ---> Rb2O + CO2 Type: decomp4. 2NiO ---> 2Ni + O2 Type: decomp5. CO2 + H2O---> H2CO3 Type: synth

Part C: Predict the products, balance, include states, and indicate type.

1) Potassium Chlorate is heated vigorously2KClO3 2KCl + 3O2 decomposition

2) Molten sodium is reacted with chlorine gas2Na + Cl2 2NaCl synthesis

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Name ___________

3) Calcium is added to waterCa + 2HOH Ca(OH)2 synthesis

4) Zinc carbonate is heateZnCO3 ZnO + CO2 decomposition

5) Aluminum chloride decomposes into it's elements2AlCl3 2Al + 3Cl2 decomposition

6) Cesium hydroxide is heated4CsOH 2Cs2O + 2H2 decomposition

7) Sulfurous Acid is heatedH2SO3 H2O + SO2 decomposition

8) Potassium and Bromine are reacted2K+ Br2 2KBr decomposition

9. Potassium Oxide and Carbon dioxide reactK2O + CO2 K2CO3 decomposition

10. Calcium chlorate is heatedCa(ClO3)2 CaCl2 + 3O2 decomposition

1) Sodium hydroxide is heated4NaOH 2Na2O + 2H2 decomposition

12. Iodine reacts with hydrogenI2 + H2 2HI synthesis

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Name ___________Single Replacement Reactions Worksheet Name: Do work on a separate sheet of paper

A. Predict the products and balance the following single replacement reactions. If no reaction occurs write N.R.

1) Fe + CuCl2 2) Hg + Sn(SO4)2 3) Ba + Ni3(PO4)2 4) F2 + NaCl 5) Cl2 + NH4Br 6) Pb + Au(NO3)3 7) Li + HOH 8) K + AgCl 9) Ca + NaOH 10) Cu + Fe(OH)3 11) Fe + Cu(OH)2 12) Br2 + KI

B. Write the reactions and predict the products of each of the following single replacement reactions. Balance all reactions. If no reaction occurs write N.R.

13) Lead II Chloride + Magnesium14) Barium Nitrate + Zinc15) Potassium + Tin IV Nitrate16) Copper + Silver Nitrate17) Sodium Phosphate + Potassium18) Gold + Hydrogen chloride19) Magnesium + Aluminum Hydroxide20) Iron + Copper II Sulfate21) Iron + Nickel II Iodide22) Sodium Permanganate + Calcium23) Hydrogen Chloride + Zinc24) Aluminum + Iron II dichromate

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Name ___________Name:____________

Period:____________Mixed Types of Reactions

Directions: For each of the following reactions:5) Complete the reaction (Put NR if no reaction takes place)6) Balance it7) Identify the type of reaction8) (Single Replacement, combination, double replacement, decomposition, or

combustion)9) Indicate states of matter for each reaction

26) NaCl + AgNO3 27) Fe + CuSO4 28) C4H10 + O2 29) Ba(NO3)2 + Na2SO4 30) AgNO3 + Li 31) LiBr + Cu 32) MgS + NaOH 33) HG + LiCl 34) Li + HgCl2 35) C3H8 + O2 36) Ammonium Nitrate is added to sodium chloride37) Lithium Chloride is added to Zinc Phosphate38) Zinc is added to lithium chloride39) Iron is added to a solution of silver nitrate40) A solution of copper II sulfate is added to an iron nail41) Octane (C8H18) is burned in air

42) A solution of Tin IV sulfate is added to a solution of ammonium hydroxide43) Sodium hydroxide is added to hydrochloric acid44) Calcium hydroxide is added to sulfuric acid45) Nickel is added to hydrochloric acid46) Strontium is added to water47) Hydrochloric acid is added to copper metal48) Solid bismuth is added to a solution of barium hydroxide.49) A solution of potassium iodide is added to liquid bromine.50) Methanol (CH3OH) is burned in air51) Solid gold is added to hydrochloric acid

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Name ___________Ws E KEY

Types of Reactions Work Sheet

Directions: For each of the following reactions: Complete the reaction (Put NR if no reaction takes place) Balance it Identify the type of reaction

(Single Replacement, combination, double replacement, decomposition, or combustion)

Indicate states of matter for each reaction

1) Sodium chloride plus silver nitrateNaCl(aq)+AgNO3(aq) AgCl(s) + NaNO3(aq) Double Replacement

2) Iron plus copper II sulfate2Fe(s) + 3CuSO4(aq) 3Cu(s) + Fe2(SO4)3(aq)

Fe(s) + CuSO4(aq) Cu(s) + FeSO4(aq)

Single Replacement

3) Butane (C4H10) burns completely in the presence of oxygen C4H10 (g) + 13/2O2 (g) 4CO2 (g) + 5H2O (g)

2C4H10 (g) + 13O2 (g) 8CO2 (g) + 10H2O (g)

Combustion

4) Barium Nitrate + sodium sulfateBa(NO3)2 (aq) + Na2SO4 (aq) BaSO4 (s) + 2NaNO3 (aq)

Double Replacement

5) Silver nitrate Plus LithiumAgNO3(aq) + Li (s) - LiNO3 (aq) + AgSingle Replacement

6) Lithium bromide plus copperLiBr (aq) + Cu No reaction

7) Magnesium sulfide plus sodium hydroxide.MgS (s) + NaOH (aq) No reaction

8) Liquid mercury reacts with aqueous lithium chlorideHg (l) + LiCl (aq) No Reaction

9) Solid Lithium is dropped into a solution of Mercury II chloride2Li (s) + HgCl2 (aq) 2LiCl (aq) + Hg (l)

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Name ___________Single Replacement

10) Propane (C3H8) is burned in the presence of airC3H8 (g) + 5O2 (g) 3CO2 (g) + 4H2O (g)

Combustion

11) Ammonium Nitrate is added to sodium chlorideNH4NO3 (aq) + NaCl (aq) No reaction

12) Lithium Chloride is added to Zinc PhosphateLiCl (aq) + Zn3(PO4)2(s) No reaction

13) Zinc is added to lithium chlorideZn (s) + LiCl(aq) No reaction

14) Iron is added to a solution of silver nitrateFe (s) + 3AgNO3(aq) 3Ag(s) + Fe(NO3)3

Fe (s) + 2AgNO3(aq) 2Ag(s) + Fe(NO3)2

Single Replacement

15) A solution of copper II sulfate is added to an iron nail3CuSO4 (aq) + 2Fe (s) Fe2(SO4)3 (aq) + 3Cu(s)

CuSO4 (aq) + Fe (s) FeSO4 (aq) + CuSingle Replacement

16) Octane (C8H18) is burned in airC8H18(g) + 12.5O2(g) 8CO2(g) + 9H2O(g)

2C8H18(g) + 25O2(g) 16CO2(g) + 18H2O(g)

combustion

17) A solution of Tin IV sulfate is added to a solution of ammonium hydroxideSn(SO4)2(aq) + 4NH4OH(aq)

Sn(OH)4(s) + 2(NH4)2SO4(aq)

double replacementOr: No Reaction: Really a reaction will occur

18) Sodium hydroxide is added to hydrochloric acidNaOH(aq) + HCl(aq) H2O(l) + NaCl(aq)

double replacement

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Name ___________

19) Calcium hydroxide is added to sulfuric acidCa(OH)2 (s) + H2SO4 (aq)

CaSO4 (s) + 2H2O(l)

double replacement

20) Nickel is added to hydrochloric acidNi(s) + 2HCl(aq) NiCl2(aq) + H2 (g)

2Ni(s) + 6HCl(aq) 2NiCl3(aq) + 3H2 (g)

Single Replacement

21) Strontium is added to waterSr(s) + 2HOH(l) Sr(OH)2(s) + H2(g)

Single replacement

22) Hydrochloric acid is added to copper metalHCl(aq) + Cu No reaction

23) Solid bismuth is added to a solution of barium hydroxide.Bi(s) + Ba(OH)2(s) No reaction

24) A solution of potassium iodide is added to liquid bromine.2KI(aq) + Br2(l) 2KBr(aq) + I2 (s)

single replacement

25) Methanol (CH3OH) is burned in air2CH3OH(g) + 3O2(g)

2CO2(g) + 4H2O(g)

combustion

26) Solid gold is added to hydrochloric acidAu(s) + HCl(aq) no reaction

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Name ___________Reaction Type WorksheetBalance and then identify each of the following reactions as: combustion, synthesis, decomposition, Single Displacement, Double Displacement.

1. Na + Cl2 NaCl Type: ______________

2. AgNO3 + NaCl AgCl + NaNO3 Type: ______________

3. NH4CO3 (NH4)2O + CO2 Type: ______________

3. CuSO4 + Li Li2SO4 + Cu Type: ______________

4. C2H6 + O2 CO2 + H2O Type: ______________

5. Na3PO4 + CuCl2 Cu3(PO4)2 + NaCl Type: ______________

6. AgNO3 + Zn Zn(NO3)2 + Ag Type: ______________

7. CH3OH + O2 CO2 + H2O Type: ______________

8. CaO + CO2 CaCO3 Type: ______________

9. Pb(NO3)2 + Na2CrO4 NaNO3 + PbCrO4 Type: ______________

10. KClO3 KCl + O2 Type: ______________

11. Magnesium + Iron III Chloride Magnesium Chloride + Iron

12. Nickel II Iodide + Silver I Nitrate Silver I Iodide + Nickel II Nitrate

13. Sodium carbonate decomposes into sodium oxide and carbon dioxide

14. Butane (C4H10) reacts with oxygen to form carbon dioxide and water

15. Magnesium oxide reacts with carbon dioxide to make magnesium carbonate

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Name ___________

16. Potassium Phosphate + Chromium III ChloridePotassium Chloride + Chromium III Phosphate

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