Chemical Reactions.

Chemical Reactions

Chemical Reactions All chemical reactions have two parts:
A substance that undergoes a reaction is called a reactant. In other words, reactants are the substances you start with.

Chemical Reactions When reactants undergo a chemical change, each new substance formed is called a product. In other words, the products are the substances you end up with.

Chemical Reactions The reactants turn into the products.
Reactants ® Products

Chemical Reactions In a chemical reaction, the way atoms are joined is changed. Atoms are NOT created or destroyed.

Chemical Reactions Chemical reactions can be described several ways.
In a sentence Copper reacts with chlorine to form copper (II) chloride. In a word equation Copper + chlorine ® copper (II) chloride

Symbols Used in Equations
The arrow separates the reactants from the products The arrow reads “reacts to form.” The plus sign reads “and”

(s) after the formula - solid (g) after the formula - gas (l) after the formula – liquid (aq) after the formula – aqueous (a solid dissolved in water)

indicates a reversible reaction. (More info later) shows that heat is supplied to the reaction is used to indicate a catalyst used supplied, in this case, platinum.

What is a Catalyst? A catalyst is a substance that speeds up a reaction without being changed by the reaction. Enzymes are biological or protein catalysts.

Diatomic Elements There are 7 elements that never want to be alone.
They form diatomic molecules. H2 , N2 , O2 , F2 , Cl2 , Br2 and I2 The –ogens and the –ines 1 + 7 pattern on the periodic table

Diatomic Elements

Indications of a Chemical Reaction
The following are indications that a chemical reaction has occurred: formation of a precipitate evolution of a gas color change absorption or release of heat

Skeleton Equation A skeleton formula uses formulas and symbols to describe a reaction. All chemical equations are sentences that describe reactions.

Problem Fe2S3 (s) + HCl (g)  FeCl2 (s) + H2S (g)
Convert the following sentence to a chemical equation. Solid iron (III) sulfide reacts with gaseous hydrogen chloride to form solid iron (II) chloride and hydrogen sulfide gas. Fe2S3 (s) + HCl (g)  FeCl2 (s) + H2S (g)

Problem HNO3 (aq) + Na2CO3 (s)  H2O (l) + CO2 (g) + NaNO3 (aq)
Convert the following sentence to a chemical equation. Nitric acid dissolved in water reacts with solid sodium carbonate to form liquid water and carbon dioxide gas and sodium nitrate dissolved in water. HNO3 (aq) + Na2CO3 (s)  H2O (l) + CO2 (g) + NaNO3 (aq)

Problem Convert the following chemical equation to a sentence.
Fe (s) + O2 (g) ® Fe2O3 (s) Solid iron reacts with oxygen gas to form solid iron (III) oxide.

Problem Convert the following chemical equation to a sentence.
Cu (s) + AgNO3 (aq) ® Ag (s) + Cu(NO3)2 (aq) Solid copper reacts with silver nitrate dissolved in water to form solid silver and copper (II) nitrate dissolved in water.

Balancing Chemical Equations

The Balanced Equation Atoms cannot be created nor destroyed.
All the atoms we start with we must end up with. A balanced equation has the same number of each element on both sides of the equation.

® O + C C O O C + O2 ® CO This equation is NOT balanced.
There is one carbon atom on the left and one on the right. There are two oxygen atoms on the left and only one on the right.

O + C C O O C + O2 ® CO We need one more oxygen atom in the products. We can’t change the formula, because it describes what it is.

C O O + C O C O In order to have two oxygen atoms, another CO must be produced. But where did the other carbon come from?

C C O O + O C C O We must have started with two carbon atoms.

C C O O + O C C O The balanced chemical equation is 2 C + O2 ® 2 CO

Rules for Balancing Write the correct formulas for all the reactants and products. Count the number of atoms of each type appearing on both sides. Balance the elements one at a time by adding coefficients (the numbers in front). Check to make sure it is balanced.

Never Never change a subscript to balance an equation.
If you change the formula you are describing a different reaction.

Never Never put a coefficient in the middle of a formula.
2 NaCl is okay; Na2Cl is not.

H2 + O2 ® H2O Example Make a table to keep track of where you
are in the balancing process.

Example ® H2 + O2 H2O Reactants Products 2 H 2 2 O 1
We need twice as much O in the product.

Example H2 + O2 2 H2O We need 2 oxygen atoms on the product side, so a coefficient of 2 should be placed in front of water.

Example H2 + O2 2 H2O We must recalculate the number of hydrogen and oxygen atoms on the right. Coefficients are used as multipliers. R P 2 H 2 4 2 O 1 2

Example H2 + O2 2 H2O Now we need 4 hydrogen atoms on the reactant side. R P 2 H 4 2 O 2

Example 2 H2 + O2 2 H2O A coefficient of 2 should be placed in front of hydrogen gas. R P 4 2 H 4 2 O 2

Example 2 H2 + O2 2 H2O The equation is balanced; it has the same number of each kind of atom on both sides! R P 4 H 4 2 O 2

Example R P 4 2 H 2 4 2 O 1 2 2 H2 + O2 ® 2 H2O This is the answer,
not this.

Balancing Hints metals nonmetals hydrogen oxygen
Balance elements in the following order: metals nonmetals hydrogen oxygen

Balancing Hints If an atom appears more than once on a side, balance it last. If you fix everything except one element, and it is even on one side and odd on the other, double the first number, then move on from there.

Problem CH4 + O2 ® CO2 + H2O CH4 + 2 O2 ® CO2 + 2 H2O
Balance the following equation. CH4 + O2 ® CO2 + H2O CH4 + 2 O2 ® CO2 + 2 H2O

Problem AgNO3 + Cu ® Cu(NO3)2 + Ag 2 AgNO3 + Cu ® Cu(NO3)2 + 2 Ag
Balance the following equation. AgNO3 + Cu ® Cu(NO3)2 + Ag 2 AgNO3 + Cu ® Cu(NO3)2 + 2 Ag

Problem Mg + N2 ® Mg3N2 3 Mg + N2 ® Mg3N2
Balance the following equation. Mg + N2 ® Mg3N2 3 Mg + N2 ® Mg3N2

Problem Balance the following equation. P + O2 ® P4O10 4 P + 5 O2 ® P4O10

Problem Na + H2O ® H2 + NaOH 2 Na + 2 H2O ® H2 + 2 NaOH
Balance the following equation. Na + H2O ® H2 + NaOH 2 Na + 2 H2O ® H NaOH

Problem Pb(NO3)2 + K2CrO4  PbCrO4 + KNO3
Balance the following equation. Pb(NO3)2 + K2CrO4  PbCrO4 + KNO3 Pb(NO3)2 + K2CrO4  PbCrO4 + 2 KNO3

Problem MnO2 + HCl  MnCl2 + H2O+ Cl2
Balance the following equation. MnO2 + HCl  MnCl2 + H2O+ Cl2 MnO2 + 4 HCl  MnCl2 + 2 H2O+ Cl2

Problem Ba(CN)2 + H2SO4  BaSO4 + HCN Ba(CN)2 + H2SO4  BaSO4 + 2 HCN
Balance the following equation. Ba(CN)2 + H2SO4  BaSO4 + HCN Ba(CN)2 + H2SO4  BaSO4 + 2 HCN

Problem Zn(OH)2 + H3PO4  Zn3(PO4)2 + H2O
Balance the following equation. Zn(OH)2 + H3PO4  Zn3(PO4)2 + H2O 3 Zn(OH)2 + 2 H3PO4  Zn3(PO4) H2O

Predicting the Products
Types of Reactions Predicting the Products

Types of Reactions

Types of Reactions Reactions fall into 5 categories.
We will recognize the type by the reactants. We will be able to predict the products. For some we will be able to predict whether they will happen at all.

How to Recognize Which Type
Look at the reactants. (E = element; C = compound) E + E Synthesis C Decomposition E + C Single replacement C + C Double replacement hydrocarbon + O2 Combustion

How to Recognize Which Type
Note: Two other common synthesis reactions include: nonmetallic oxide + water and metallic oxide + water. Use Page 6 of the Chemistry Reference Table as a guide.

Problem Identify whether the reaction is synthesis, decomposition, single replacement, double replacement or combustion. H2 + O2 ® (synthesis) H2O ® (decomposition)

Problem Mg(OH)2 + H2SO3 ® HgO ®
Identify whether the reaction is synthesis, decomposition, single replacement, double replacement or combustion. Mg(OH)2 + H2SO3 ® (double replacement) HgO ® (decomposition)

Problem KBr + Cl2 ® Zn + H2SO4 ®
Identify whether the reaction is synthesis, decomposition, single replacement, double replacement or combustion. KBr + Cl2 ® (single replacement) Zn + H2SO4 ® (single replacement)

Problem AgNO3 + NaCl ® C6H6 + O2 ®
Identify whether the reaction is synthesis, decomposition, single replacement, double replacement or combustion. AgNO3 + NaCl ® (double replacement) C6H6 + O2 ® (combustion)

Synthesis Reactions Synthesize - put together
Whenever two or more substances combine to form one single product, the reaction is called a synthesis reaction. Ca + O2 ® CaO P2O5 + 3 H2O ® 2 H3PO4

Synthesis Reactions

Synthesis Reactions We can predict the products if they are two elements. All you need to do is combine the elements, metals first, and criss-cross oxidation numbers if necessary.

Synthesis Reactions Example Mg + N2 ® 3- 2+ Mg N

Synthesis Reactions Mg N The charges do not add to give zero. 2+ 3- 3

Synthesis Reactions Example Mg + N2 ® Mg3N2

Synthesis Reactions Mg + N2 ® Mg3N2 3
Now the reaction needs to be balanced. Mg + N2 ® Mg3N2 3

Synthesis Reactions CaO + H2O ® Example
On page 6 of the Chemistry Reference Packet, this reaction is an example of “Metal oxide - water reactions.”

Synthesis Reactions CaO + H2O ® Example
The product listed in the packet is “base.” A base is a metallic hydroxide.

Synthesis Reactions Example CaO + H2O ® 1- 2+ Ca OH

Synthesis Reactions ( ) Ca OH
The charges do not add to give zero, so you must criss-cross. The hydroxide needs parenthesis. 2+ 1- ( ) Ca OH 1 2

Synthesis Reactions Example CaO + H2O ® Ca(OH)2

Synthesis Reactions CaO + H2O ® Ca(OH)2 Check the balancing.
The reaction is already balanced!

Synthesis Reactions SO2 + H2O ® Example
On page 6 of the Chemistry Reference Packet, this reaction is an example of “Nonmetal oxide - water reactions.”

The product listed in the packet is “acid.” The acid is a ternary acid. Ternary acids start with H and end in O.

The other element goes in the center.

Synthesis Reactions H S O SO2 + H2O ® Example
This is the ONLYcompound for which you can add the number of elements and use these numbers as subscripts.

Synthesis Reactions H S O SO2 + H2O ® Example 2 1 3
There are 2 hydrogens. There is one sulfur. There are three oxygens.

Synthesis Reactions SO2 + H2O ® H2SO3 Example
The reaction is balanced.

Problem Ca + Cl2 ® Ca + Cl2  CaCl2
Write and balance the following synthesis reaction. Ca + Cl2 ® Remember that the first step is to write the formula. Then balance. Ca + Cl2  CaCl2

Problem Fe + O2 ® 2 Fe + O2  2 FeO
Write and balance the following synthesis reaction. Fe + O2 ® HINT: Use iron (II). 2 Fe + O2  2 FeO

Problem K2O + H2O ® K2O + H2O  2 KOH
Write and balance the following synthesis reaction. K2O + H2O ® K2O + H2O  2 KOH

Problem Al + O2 ® 4 Al + 3 O2  2 Al2O3
Write and balance the following synthesis reaction. Al + O2 ® 4 Al O2  2 Al2O3

Problem SO3 + H2O ® SO3 + H2O  H2SO4
Write and balance the following synthesis reaction. SO3 + H2O ® SO3 + H2O  H2SO4

Problem N2O5 + H2O ® N2O5 + H2O  2 HNO3
Write and balance the following synthesis reaction. N2O5 + H2O ® N2O5 + H2O  2 HNO3

Decomposition Reactions
decompose = fall apart In a decomposition reaction, one compound breaks down into two or more simpler substances. NaCl Na + Cl2 CaCO CaO + CO2

Can predict the products if it is a binary compound. A binary compound is made up of only two elements. The compound merely falls apart into its elements.

H2O H O 2 2 Both of these elements are diatomic!!!

H2O H O 2 2 Now we must balance. 2 H2O H O2 2

HgO Hg O 2 Oxygen is diatomic!!!

HgO Hg O 2 Now we must balance. 2 HgO Hg + O2 2

If the compound has more than two elements, you must consult the Reference Tables, page 6.

Example NiCO3 Write and balance the following decomposition reaction.
Once again, refer to page 6 in the Chemistry Reference Packet.

Example NiCO3 NiCO3 is called nickel (II) carbonate.
The packet states that a metallic carbonate decomposes to form a MO (metallic oxide) and CO2.

Example Ni O NiCO3 The metallic oxide is nickel (II) oxide. 2+ 2-
The two oxidation numbers add to give zero, so the formula is NiO.

Example NiCO3 NiO + CO2 Check the balancing.
The reaction is already balanced!

Problem KClO3 ® 2 KClO3  2 KCl + 3 O2
Write and balance the following decomposition reaction. KClO3 ® 2 KClO3  2 KCl O2

Problem CaBr2 ® CaBr2  Ca + Br2
Write and balance the following decomposition reaction. CaBr2 ® CaBr2  Ca + Br2

Problem Li2CO3 ® Li2CO3  Ca + Br2
Write and balance the following decomposition reaction. Li2CO3 ® Li2CO3  Ca + Br2

Problem Cr(OH)2 ® Cr(OH)2  CrO + H2O
Write and balance the following decomposition reaction. Cr(OH)2 ® Cr(OH)2  CrO + H2O

Problem NaHCO3 ® 2 NaHCO3  Na2O + H2O + 2 CO2
Write and balance the following decomposition reaction. NaHCO3 ® 2 NaHCO3  Na2O + H2O CO2

Problem HNO3 ® 2 HNO3  N2O5 + H2O
Write and balance the following decomposition reaction. HNO3 ® Dinitrogen pentoxide one of the products. 2 HNO3  N2O5 + H2O

Single Replacement In a single-displacement reaction, one element takes the place of another in a compound. One reactant must be an element and one reactant must be a compound. The products will be a different element and a different compound. F2 + LiCl ® LiF + Cl2

Single Replacement Remember zinc, Zn, always forms a +2 ion doesn’t need parenthesis. ZnCl2 is zinc chloride. In addition, silver, Ag, always forms a +1 ion. AgCl is silver chloride.

Single Replacement Some single replacement reactions do not occur because some elements are not as active as others. Only a more active element will replace a less active element.

Single Replacement There is a list referred to as the Activity Series on page 7 of your Chemistry Reference Packet. A higher element on the list replaces lower element. If the element by itself is lower on the list, the reaction will NOT occur.

Single Replacement K + NaCl ® Metals replace metals
Potassium wants to replace sodium. You must check the activity series on page 7 of your Chemistry Reference Packet to see if this is possible.

Single Replacement K + NaCl ® YES!! Metals replace metals
Is potassium higher than sodium on the Activity Series of Metals? YES!!

Single Replacement K + NaCl ® KCl + Na Metals replace metals
Because K is higher, potassium can replace sodium. The potassium will bond with the chlorine and the sodium will be alone.

Single Replacement K + NaCl ® KCl + Na K Cl Metals replace metals
You must always check to see if the compound formed needs criss-crossing. 1+ 1- K Cl

Since the charges add to get zero, the formula remains KCl.

Check for balancing. The reaction is balanced!

Single Replacement Sn + FeCl3 ® Metals replace metals
Tin wants to replace iron. You must check the activity series on page 7 of your Chemistry Reference Packet to see if this is possible.

Single Replacement Sn + FeCl3 ® NO!! Metals replace metals
Is tin higher than iron on the Activity Series of Metals? NO!!

Single Replacement Sn + FeCl3 ® No reaction Metals replace metals
Because Sn is NOT higher, tin cannot replace iron. No reaction occurs.

Problem Rb + AlN ® 3 Rb + AlN  Rb3N + Al
Write and balance the following single replacement reaction. Rb + AlN ® 3 Rb + AlN  Rb3N + Al

Problem Zn + HCl ® Zn + 2 HCl  ZnCl2 + H2
Write and balance the following single replacement reaction. Zn + HCl ® Zn HCl  ZnCl2 + H2

Problem Ag + CoBr2 ® Ag + CoBr2  no reaction
Write and balance the following single replacement reaction. Ag + CoBr2 ® Ag + CoBr2  no reaction

Problem Ag + H2O (steam) ® Ag + H2O (steam)  no reaction
Write and balance the following single replacement reaction. Ag + H2O (steam) ® Ag + H2O (steam)  no reaction

Problem Cu + H2SO4 ® Cu + H2SO4  no reaction
Write and balance the following single replacement reaction. Cu + H2SO4 ® Cu + H2SO4  no reaction

Problem Cr + H3PO4 ® 2Cr + 2H3PO4  2CrPO4 + 3H2
Write and balance the following single replacement reaction. Cr + H3PO4 ® (HINT: Use Cr3+ ) 2Cr + 2H3PO4  2CrPO H2

Problem Ca + H2O (steam) ® Ca + 2H2O (steam)  Ca(OH)2 + H2
Write and balance the following single replacement reaction. Ca + H2O (steam) ® Ca + 2H2O (steam)  Ca(OH)2 + H2

Single Replacement Nonmetals can replace other nonmetals.
This is limited to F2 , Cl2 , Br2 , I2 The order of activity is listed in the Chemistry Reference Packet, page 7. Higher replaces lower.

Single Replacement F2 + HCl ® YES!!
Is fluorine above chlorine in the activity series of halogens? YES!!

Single Replacement F2 + HCl ® HF + Cl
Fluorine replaces the chlorine, bonding with hydrogen.

Single Replacement F2 + HCl ® HF + Cl 1+ 1- H F 2
But chlorine is diatomic. Check the oxidation numbers of H and F. 1+ 1- H F

Single Replacement F2 + HCl ® HF + Cl F2 + HCl ® HF + Cl2 2 2 2
Check balancing. F HCl ® HF + Cl2 2 2

Problem Br2 + KCl ® Br2 + KCl  no reaction
Write and balance the following single replacement reaction. Br2 + KCl ® Br2 + KCl  no reaction

Problem Cl2 + KI ® Cl2 + 2 KI  2 KCl + I2
Write and balance the following single replacement reaction. Cl2 + KI ® Cl KI  2 KCl + I2

Combustion A combustion reaction is one in which a substance rapidly combines with oxygen to form one or more oxides. Combustion reactions involve a hydrocarbon (C, H, sometimes O) that is reacted with oxygen gas (O2).

Combustion If the combustion is complete, the products will be CO2 and H2O. Combustion reactions produce heat, and are therefore considered exothermic reactions.

Combustion

Combustion C4H10 + O2 ® CO2 + H2O
Complete and balance the following combustion reaction. C4H O2 ® CO2 + H2O Now balance.

Combustion C4H10 + O2 ® CO2 + H2O 13/2 4 5 C4H10 + O2 ® CO2 + H2O 2 13
Fractions are not allowed, so multiply all coefficients by 2. C4H O2 ® CO H2O 2 13 8 10

Problem C6H12O6 + O2 ® C6H12O6 + 6 O2  6 CO2 + 6 H2O
Complete and balance the following combustion reaction. C6H12O6 + O2 ® C6H12O O2  6 CO H2O

Problem C8H8 + O2 ® C8H8 + 10 O2  8 CO2 + 4 H2O
Complete and balance the following combustion reaction. C8H8 + O2 ® C8H O2  8 CO H2O

Problem C3H8O3 + O2 ® 2 C3H8O3 + 7 O2  6 CO2 + 8 H2O
Complete and balance the following combustion reaction. C3H8O3 + O2 ® 2 C3H8O O2  6 CO H2O

Double Replacement In double-displacement reactions, the positive portions of two ionic compounds are interchanged. The reactants must be two ionic compounds or acids. Double replacement reactions usually take place in aqueous solution.

Double Replacement NaOH + FeCl3 ® The positive ions change place.
You must check to see if you need to criss-cross the products. NaOH + FeCl3 ® Fe+3 OH- + Na+1Cl-1 NaOH + FeCl3 ® Fe(OH)3 + NaCl

Double Replacement NaOH + FeCl3 ® Fe(OH)3 + NaCl
Now balance. NaOH + FeCl3 ® Fe(OH) NaCl 3 3

Double Replacement A double replacement reaction will only happen if one of the products: doesn’t dissolve in water and forms a solid (insoluble), is a gas that bubbles out, or is a covalent compound usually water.

Compounds in Aqueous Solution
Using the solubility rules printed on page 6 of the NCDPI Reference Tables for Chemistry, determine whether the following salts are soluble in water. a) sodium chloride (soluble)

b) mercury (I) acetate (soluble) c) potassium nitrate (soluble)

d) nickel carbonate (insoluble) e) BaSO4 (insoluble)

f) NH4Br (soluble) g) CaS (soluble)

Double Replacement Predict if the reaction will occur, and if so, what compound is the preceipitate. 3NaOH + FeCl3 ® Fe(OH) NaCl None of the products are familiar gases. Both products are ionic (not covalent) because they start with metals.

Double Replacement 3NaOH + FeCl3 ® Fe(OH)3 + 3NaCl
We must consult the Solubility Rules on page 6 of the Chemistry Reference Tables to determine if a solid (a precipitate) is formed.

The “Soluble” side of the Solubility Rules states that Group 1 (IA) salts are soluble; therefore, NaCl is soluble and is NOT the precipitate.

The “Insoluble” side of the Solubility Rules states that all hydroxides except Group 1, Sr2+, Ba2+ and NH41+ are INSOLUBLE. Therefore, Fe(OH)3 is the precipitate (solid).

Net Ionic Equations 3NaOH + FeCl3 ® Fe(OH)3 + 3NaCl
In molecular equations, the formulas of the compounds are written as though all species existed as molecules or whole units. Molecular equation: 3NaOH + FeCl3 ® Fe(OH) NaCl

Net Ionic Equations An ionic equation shows dissolved ionic compounds in terms of their free ions. Complete ionic equation: 3Na+ + 3OH- + Fe3+ + 3Cl-  Fe(OH)3 + 3Na+ + 3Cl-

Net Ionic Equations 3OH- (aq) + Fe3+ (aq)  Fe(OH)3 (s)
Ions that are not involved in the overall reaction are called spectator ions. The net ionic equation indicates only the species that actually take part in the reaction. Net ionic equation: 3OH- (aq) + Fe3+ (aq)  Fe(OH)3 (s)

Net Ionic Equations The following steps are useful for
writing ionic and net ionic equations: 1) Write a balanced molecular equation for the reaction.

Net Ionic Equations Rewrite the equation to indicate which substances are in ionic form in solution. Remember that all soluble salts (and other strong electrolytes), are completely dissociated into cations and anions. This procedure gives us the ionic equation.

Net Ionic Equations Lastly, identify and cancel spectator ions on both sides of the equation to arrive at the net ionic equation.

3NaOH + FeCl3 ® Fe(OH)3 + 3NaCl
Molecular equation: 3NaOH + FeCl3 ® Fe(OH) NaCl Complete ionic equation: 3Na+ + 3OH- + Fe3+ + 3Cl-  Fe(OH)3 + 3Na+ + 3Cl- Net ionic equation: 3OH- (aq) + Fe3+ (aq)  Fe(OH)3 (s)

Problem CaCl2 + 2 NaOH  Ca(OH)2 + 2 NaCl
Write and balance the following double replacement reaction. Assume the reaction takes place. CaCl2 + NaOH ® CaCl NaOH  Ca(OH) NaCl

Problem CaCl2 + 2 NaOH  Ca(OH)2 + 2 NaCl
Identify the precipitate and write the net ionic equation. CaCl NaOH  Ca(OH) NaCl Ca(OH)2 is the precipitate. Ca OH-  Ca(OH)2

Problem CuCl2 + K2S  CuS + 2 KCl
Write and balance the following double replacement reaction. Assume the reaction takes place. CuCl2 + K2S ® CuCl2 + K2S  CuS KCl

Problem CuCl2 + K2S  CuS + 2 KCl
Identify the precipitate and write the net ionic equation. CuCl2 + K2S  CuS KCl CuS is the precipitate. Cu S2-  CuS

Problem 3 KOH + Fe(NO3)3  3 KNO3 + Fe(OH)3
Write and balance the following double replacement reaction. Assume the reaction takes place. KOH + Fe(NO3)3 ® 3 KOH + Fe(NO3)3  3 KNO3 + Fe(OH)3

Problem Identify the precipitate and write the net ionic equation.
3 KOH + Fe(NO3)3  3 KNO3 + Fe(OH)3 Fe(OH)3 is the precipitate. Fe OH-  Fe(OH)3

Problem (NH4)2SO4 + BaF2  2 NH4F + BaSO4
Write and balance the following double replacement reaction. Assume the reaction takes place. (NH4)2SO4 + BaF2 ® (NH4)2SO4 + BaF2  2 NH4F + BaSO4

Problem Identify the precipitate and write the net ionic equation.
(NH4)2SO4 + BaF2  2 NH4F + BaSO4 BaSO4 is the precipitate. Ba SO42-  BaSO4

Chemical Reactions.

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