Name ______

WPHS Chemistry

Unit 4

Chemical Reactions

Bergmann-Sams

Chemistry: Unit 4 Outline: Chemical Reactions

Assignment / WB Page Number / Score / Out of
Podcast 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 B

/ Pg 10-12 / 
Lab: Small Scale Single Replacement / Pg 4 / 100
Podcast 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 / 100
Worksheet 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)Unit 4 Chemical Reactions: Composition Book Outline

8-1: Describing Chemical Change

1 / 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 206
3 / 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 Equations

5 / 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 each
List: Two examples of eachtype (written with formulas—not words)
7 / Predicting Single Replacement Reactions
Copy: Table 8.2 on page 217
9 / Predicting Single Replacement Reactions
Leave blank for teacher notes
11 / Predicting and Writing Double Replacement Reactions
Leave blank for teacher notes
13 / Predicting and Writing Double Replacement Reactions
Leave blank for teacher notes

8-3: Reactions in Aqueous Solutions

15 / Ionic and Net Ionic Equations (pg 225-228)
Leave blank for teacher notes
17 / Ionic and Net Ionic Equations (pg 225-228)
Leave blank for teacher notes

Activity Series of Metals Lab

Purpose: 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 metal
Mg metal
Zn 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.

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 / X
AgNO3 / X / X / X / X / X / X
Pb(NO3)2 / X / X / X / X / X / X
Na2SO4 / X / X / X / X / X
BaCl2 / X / X / X / X / X / X
NaOH / X / X / X / X / X / X
Na3PO4 / X / X / X / X / X / X

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

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+__O2Type: ______

2)__HCl+__Mg__H2+MgCl2 Type: ______

3)__CH4+__O2__CO2+__H2O Type: ______

4)__C6H12O6+ __O2__CO2+ __H2OType: ______

5)__H2+__O2__H2OType: ______

6)__H2+__N2__NH3Type: ______

7)__NO+__O2__NO2Type: ______

8)__Al2O3__Al+__O2Type: ______

9)__CaO+__H2O__Ca(OH)2Type: ______

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

Type: ______

11)Sulfur reacts with oxygen to produce sulfur dioxide.

Type: ______

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) hydroxide

Type: ______

15)Sulfur trioxide is bubbled through water to produce sulfuric acid

Type: ______

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: ______

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
  1. Hg +Sn(SO4)2 
  1. Ba +Ni3(PO4)2 
  1. Pb +Au(NO3)3
  1. Li +HOH
  1. K +AgCl
  1. Ca +NaOH 
  1. Cu +Fe(OH)3
  1. Fe +Cu(OH)2
  1. Lead II Chloride + Magnesium
  1. Barium Nitrate + Zinc
  1. Potassium + Tin IV Nitrate
  1. Copper + Silver Nitrate
  1. Sodium Phosphate + Potassium
  1. Gold + Hydrochloric acid
  1. Magnesium + Aluminum Hydroxide
  1. Iron + Copper II Sulfate
  1. Iron + Nickel II Iodide
  1. Sodium Permanganate + Calcium
  1. hydrochloric acid + Zinc
  1. Aluminum + Iron II dichromate

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

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

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

Equation Worksheet D: Net Ionic Equation Worksheet

For the following reactions write the:

  1. Complete Equation (Indicate states): Balance
  2. Ionic Equation
  3. Net Ionic Equation
  1. ZnCl2 (aq) + Na2S (aq)  ZnS(s) + NaCl(aq)
  1. (NH4)3PO4 + AgNO3
  1. Magnesium Nitrate + Potassium phosphate  Magnesium Phosphate (s) + Potassium Nitrate.
  1. Lead II Acetate + Potassium Iodide

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 it

3)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 

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

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

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

Name: ______

Period: ______

Balancing Reactions Worksheet

Synthesis and Decomposition

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

1.SO3+H2O--->H2SO4Type:______

2.H2O--->H2+O2Type:______

3.HgO--->Hg+O2Type:______

4.Al2O3(s)--->Al(s)+O2(g)Type:______

5.P+O2--->P2O5Type:______

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 vigorouslyType: ______

2. Molten sodium is reacted with chlorine gasType: ______

3. Calcium is added to waterType: ______

4. Zinc carbonate is heateType: ______

5. Aluminum chloride decomposes into it's elementsType: ______

6. Cesium hydroxide is heatedType: ______

7. Sulfurous Acid is heatedType: ______

8. Potassium and Bromine are reactedType: ______

9. Potassium Oxide and Carbon dioxide reactType: ______

10. Calcium chlorate is heatedType: ______

11. Sodium hydroxide is heatedType: ______

12. Iodine reacts with hydrogenType: ______

Balancing Chemical Equations Worksheet 1Name

Period

Balance the following equations:

  1. 2HgO 2Hg+O2
  2. HCl+MgH2+MgCl2
  3. CH4+2O2CO2+2H2O
  4. C6H12O6+6O26CO2+6H2O
  5. 2H2+O22H2O
  6. 2H2+Cl22HCl
  7. 3H2+N22NH3
  8. 2 NO+O22NO2
  9. 3Al2O34Al+2O2
  10. CaO+H2OCa(OH)2 already balanced
  11. Hydrogen gas reacts with iodine to produce hydrogen iodide.

H2+ I2 2HI

  1. Sulfur reacts with oxygen to produce sulfur dioxide.

S + O2  SO2

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

Ca(C2H3O2)2 + Na2CO3 2NaC2H3O2 +CaCO3

  1. Write the chemical reaction that shows how rust forms:

4Fe + 3O2 2Fe2O3

  1. Iron combines with oxygen and water to form iron (III) hydroxide

Fe + O2 + 6H2O  4Fe(OH)3

  1. Sulfur trioxide is bubbled through water to produce hydrogen sulfate

SO3+ H2O  H2SO4 already balanced

  1. 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

  1. 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

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

Mg(OH)2 + 2HCl  MgCl2 + 2H2O

  1. 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 this
    happens. 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 can

2HNO3 + CaCO3 Ca(NO3)2+ H2O+ CO2

Balancing Reactions Worksheet

Synthesis and Decomposition

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

1.SO3+H2O--->H2SO4balancedType: synthesis

2.2H2O--->2H2+O2Type: decomposition

3.2HgO--->2Hg+O2Type: decomposition

4.2Al2O3(s)--->4Al(s)+3O2(g)Type: Decomposition

5.4P+5O2--->2P2O5Type: Synthesis

Part B: Predict the products and indicate type (include states):

1. 2KBr --->2K + Br2Type: decomp

2. 2Li + Cl2 --->2LiClType: synth

3. Rb2CO3 --->Rb2O + CO2Type: decomp

4. 2NiO --->2Ni + O2Type: decomp

5. CO2 + H2O--->H2CO3Type: synth

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

1)Potassium Chlorate is heated vigorously

2KClO3  2KCl + 3O2decomposition

2) Molten sodium is reacted with chlorine gas

2Na + Cl2 2NaClsynthesis

3)Calcium is added to water

Ca + 2HOH  Ca(OH)2synthesis

4)Zinc carbonate is heate

ZnCO3 ZnO + CO2decomposition

5)Aluminum chloride decomposes into it's elements

2AlCl3 2Al + 3Cl2decomposition

6) Cesium hydroxide is heated

4CsOH  2Cs2O + 2H2decomposition

7)Sulfurous Acid is heated

H2SO3 H2O + SO2decomposition

8)Potassium and Bromine are reacted

2K+ Br2 2KBrdecomposition

9. Potassium Oxide and Carbon dioxide react

K2O + CO2 K2CO3decomposition

10. Calcium chlorate is heated

Ca(ClO3)2  CaCl2 + 3O2decomposition

1)Sodium hydroxide is heated

4NaOH  2Na2O + 2H2decomposition

12. Iodine reacts with hydrogen

I2 + H2  2HIsynthesis

Single Replacement Reactions WorksheetName:

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 + Magnesium

14)Barium Nitrate + Zinc

15)Potassium + Tin IV Nitrate

16)Copper + Silver Nitrate

17)Sodium Phosphate + Potassium

18)Gold + Hydrogen chloride

19)Magnesium + Aluminum Hydroxide

20)Iron + Copper II Sulfate

21)Iron + Nickel II Iodide

22)Sodium Permanganate + Calcium

23)Hydrogen Chloride + Zinc

24)Aluminum + Iron II dichromate

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 it

7)Identify the type of reaction

8)(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 chloride

37)Lithium Chloride is added to Zinc Phosphate

38)Zinc is added to lithium chloride

39)Iron is added to a solution of silver nitrate

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

41)Octane (C8H18) is burned in air

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

43)Sodium hydroxide is added to hydrochloric acid

44)Calcium hydroxide is added to sulfuric acid

45)Nickel is added to hydrochloric acid

46)Strontium is added to water

47)Hydrochloric acid is added to copper metal

48)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 air

51)Solid gold is added to hydrochloric acid

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 nitrate

NaCl(aq)+AgNO3(aq) AgCl(s) + NaNO3(aq)

Double Replacement

2)Iron plus copper II sulfate

2Fe(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 sulfate

Ba(NO3)2(aq) + Na2SO4(aq)  BaSO4 (s) + 2NaNO3(aq)

Double Replacement

5)Silver nitrate Plus Lithium

AgNO3(aq) + Li (s) - LiNO3 (aq) + Ag

Single Replacement

6)Lithium bromide plus copper

LiBr (aq) + Cu  No reaction

7)Magnesium sulfide plus sodium hydroxide.

MgS (s) + NaOH (aq)  No reaction

8)Liquid mercury reacts with aqueous lithium chloride

Hg (l) + LiCl (aq)  No Reaction

9)Solid Lithium is dropped into a solution of Mercury II chloride

2Li (s) + HgCl2(aq)  2LiCl (aq) + Hg (l)

Single Replacement

10)Propane (C3H8) is burned in the presence of air

C3H8(g) + 5O2(g)  3CO2(g) + 4H2O (g)

Combustion

11)Ammonium Nitrate is added to sodium chloride

NH4NO3(aq) + NaCl (aq)  No reaction

12)Lithium Chloride is added to Zinc Phosphate

LiCl (aq) + Zn3(PO4)2(s) No reaction

13)Zinc is added to lithium chloride

Zn (s) + LiCl(aq) No reaction

14)Iron is added to a solution of silver nitrate

Fe (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 nail

3CuSO4(aq) + 2Fe (s) Fe2(SO4)3(aq) + 3Cu(s)

CuSO4(aq) + Fe (s) FeSO4(aq) + Cu

Single Replacement

16)Octane (C8H18) is burned in air

C8H18(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 hydroxide

Sn(SO4)2(aq) + 4NH4OH(aq)

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

double replacement

Or: No Reaction: Really a reaction will occur

18)Sodium hydroxide is added to hydrochloric acid

NaOH(aq) + HCl(aq)  H2O(l) + NaCl(aq)

double replacement

19)Calcium hydroxide is added to sulfuric acid

Ca(OH)2(s) + H2SO4(aq) 

CaSO4(s) + 2H2O(l)

double replacement

20)Nickel is added to hydrochloric acid

Ni(s) + 2HCl(aq) NiCl2(aq) + H2(g)

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

Single Replacement

21)Strontium is added to water

Sr(s) + 2HOH(l)  Sr(OH)2(s) + H2(g)

Single replacement

22)Hydrochloric acid is added to copper metal

HCl(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 air

2CH3OH(g) + 3O2(g)

2CO2(g) + 4H2O(g)

combustion

26)Solid gold is added to hydrochloric acid

Au(s) + HCl(aq)  no reaction

Reaction Type Worksheet

Balance and then identify each of the following reactions as: combustion, synthesis, decomposition, Single Displacement, Double Displacement.

1. Na+Cl2 NaClType: ______

2. AgNO3+ NaCl  AgCl + NaNO3Type: ______

3. NH4CO3 (NH4)2O+ CO2Type: ______

3. CuSO4+ Li Li2SO4+ CuType: ______

4. C2H6 + O2  CO2 + H2OType: ______

5. Na3PO4 + CuCl2  Cu3(PO4)2 + NaClType: ______

6. AgNO3 + Zn  Zn(NO3)2 + AgType: ______

7. CH3OH + O2  CO2 + H2OType: ______

8. CaO + CO2 CaCO3Type: ______

9. Pb(NO3)2 + Na2CrO4  NaNO3 + PbCrO4Type: ______

10. KClO3  KCl + O2Type: ______

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

16. Potassium Phosphate + Chromium III Chloride

Potassium Chloride + Chromium III Phosphate

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