chapter #7 chemical reactions. chapter #7 contents 7-1 grade school volcanoes, cars, &...
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Chapter #7Chemical Reactions
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CHAPTER #7 CONTENTS• 7-1 Grade School Volcanoes, Cars, & Detergents• 7-2 Evidence of Chemical Reactions• 7-3 The Chemical Equation• 7-4 How to Write Balanced Chemical Equations• 7-10 Classification of Chemical Reactions• 7-9 Oxidation Reduction Reactions• 7-5 Aqueous Solutions and Solubility• 7-6 Precipitation Reactions• 7-7 Aqueous Reactions• 7-8 Acid/Base and Gas Evolution Reactions
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7-2 Chemical Change Evidence
Chapter 6
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7-2 Chemical Change Evidence
Chapter 6
What is a clue that a chemical reaction has occurred?
a) The color changes.
b) A solid forms.
c) Bubbles are present.
d) A flame is produced.
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7-2 Chemical Change Evidence
Chapter 6
What is a clue that a chemical reaction has occurred?
“Colorless hydrochloric acid is added to a red solution of cobalt(II) nitrate, turning the solution blue.”
a) The color changes.
b) A solid forms.
c) Bubbles are present.
d) A flame is produced.
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7-2 Chemical Change Evidence
Chapter 6
What is a clue that a chemical reaction has occurred?
“A solid forms when a solution of sodium dichromate is added to a solution of lead nitrate.”
a) A gas forms.
b) A solid forms.
c) Bubbles are present.
d) A flame is produced.
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Chapter 6
7-10 Chemical Reactions• A chemical equation is an abbreviated way to
show a chemical or physical change• A chemical change alters the physical and
chemical properties of a substance• Factors that indicate a chemical change
– Change in color– Temperature change– Change in odor– Change in taste (we do not taste chemicals)
• Reactions always contain an arrow that separates the reactants from the products
Reactants Products
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7-10 Types of Chemical Reactions
• Combination reaction (synthesis)– Elements for reactants– Examples:
H2 + O2 H2O
N2 + H2 NH3
Al + O2 Al2O3
The Law of Conservation of matter, states matter cannot be created nor destroyed, the means equations must be balanced.
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7-10 Types of Chemical Reactions
Balance the first equation
H2 + O2 H2O
Note two oxygen atoms on the reactant side and only one on the product side, therefore place a two in front of water
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7-10 Types of Chemical Reactions
Balance the first equation
H2 + O2 2H2O
Note two oxygen atoms on the reactant side and only one on the product side, therefore place a two in front of water
The two now doubles everything in water, thus 4 hydrogen and 2 oxygen. Now place a 2 in front of hydrogen.
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7-10 Types of Chemical Reactions
Balance the first equation
2H2 + O2 2H2O
Note two oxygen atoms on the reactant side and only one on the product side, therefore place a two in front of water
The two now doubles everything in water, thus 4 hydrogen and 2 oxygen. Now place a 2 in front of hydrogen.
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7-10 Types of Chemical Reactions
Now balance the second equation
N2 + H2 NH3
Note two nigrogen atoms on the reactant side and only one on the product side.
Place a 2 in front of ammonia
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7-10 Types of Chemical Reactions
Now balance the second equation
N2 + H2 2NH3
Note two nitrogen atoms on the reactant side and only one on the product side.
Place a 2 in front of ammonia. This makes 2 nitrogen atoms and 6 hydrogen atoms. Now place a 3 in front of hydrogen to balance hydrogen atoms.
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7-10 Types of Chemical Reactions
Now balance the second equation
N2 + 3 H2 2NH3
Note two nitrogen atoms on the reactant side and only one on the product side.
Place a 2 in front of ammonia. This makes 2 nitrogen atoms and 6 hydrogen atoms. Now place a 3 in front of hydrogen to balance hydrogen atoms.
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7-10 Types of Chemical Reactions
• Decomposition Reaction– Compounds form simpler compounds or
elements.– Examples
H2O H2 + O2
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7-10 Types of Chemical Reactions
• Decomposition Reaction– Compounds form simpler compounds or
elements.– Examples
2H2O H2 + O2
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7-10 Types of Chemical Reactions• Decomposition Reaction
– Compounds form simpler compounds or elements.
– Examples
2H2O 2H2 + O2
• Notice decomposition reactions are the opposite of combination reactions
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7-10 Types of Chemical Reactions
Single Replacement reactions have an element and a compound for reactants.
Example:
Zn + HCl
How do we predict the products? Trade places with the metal or nonmetal with the metal or nonmetal in the compound
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7-10 Types of Chemical Reactions
Single Replacement reactions have an element and a compound for reactants.
Example:
Zn + HCl
How do we predict the products? Trade places with the metal or nonmetal with the metal or nonmetal in the compound
![Page 20: Chapter #7 Chemical Reactions. CHAPTER #7 CONTENTS 7-1 Grade School Volcanoes, Cars, & Detergents 7-2 Evidence of Chemical Reactions 7-3 The Chemical](https://reader030.vdocument.in/reader030/viewer/2022032523/56649d745503460f94a53d30/html5/thumbnails/20.jpg)
7-10 Types of Chemical Reactions
Single Replacement reactions have an element and a compound for reactants.
Example:
Zn + HCl ZnCl + H
Now make the products stable. Slide with Clyde
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7-10 Types of Chemical Reactions
Single Replacement reactions have an element and a compound for reactants.
Example:
Zn + HCl ZnCl2 + H2
Now make the products stable. Slide with Clyde
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7-10 Types of Chemical Reactions
Single Replacement reactions have an element and a compound for reactants.
Example:
Zn + HCl ZnCl2 + H2
Now make the products stable. Slide with Clyde
Now Balance
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7-10 Types of Chemical Reactions
Single Replacement reactions have an element and a compound for reactants.
Example:
Zn + 2HCl ZnCl2 + H2
Now make the products stable. Slide with Clyde
Now Balance
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7-10 Types of Chemical Reactions
Single Replacement reactions have an element and a compound for reactants.
Another Example:
Cl2 + MgBr2
How do we predict the products? Trade places with the metal or nonmetal with the metal or nonmetal in the compound. In this case we are trading nonmetals
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7-10 Types of Chemical Reactions
Single Replacement reactions have an element and a compound for reactants.
Another Example:
Cl2 + MgBr2 Br + MgCl
How do we predict the products? Trade places with the metal or nonmetal with the metal or nonmetal in the compound. In this case we are trading nonmetals
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7-10 Types of Chemical Reactions
Single Replacement reactions have an element and a compound for reactants.
Another Example:
Cl2 + MgBr2 Br2 + MgCl2
How do we predict the products? Trade places with the metal or nonmetal with the metal or nonmetal in the compound. In this case we are trading nonmetals
![Page 27: Chapter #7 Chemical Reactions. CHAPTER #7 CONTENTS 7-1 Grade School Volcanoes, Cars, & Detergents 7-2 Evidence of Chemical Reactions 7-3 The Chemical](https://reader030.vdocument.in/reader030/viewer/2022032523/56649d745503460f94a53d30/html5/thumbnails/27.jpg)
7-10 Types of Chemical Reactions
Double Replacement reactions contain compounds as reactants.
HCl + Ca(OH)2 CaCl + HOH
Check formulas, and slide with Clyde when necessary
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7-10 Types of Chemical Reactions
Double Replacement reactions contain compounds as reactants.
HCl + Ca(OH)2 CaCl2 + HOH
Check formulas, and slide with Clyde when necessary
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7-10 Types of Chemical Reactions
Double Replacement reactions contain compounds as reactants.
2HCl + Ca(OH)2 CaCl2 + 2HOH
Check formulas, and slide with Clyde when necessary
Now Balance!
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7-10 Types of Chemical Reactions
Combustion Reactions occur when an element or compound combine with oxygen to produce oxides of each element.
H2 + O2
CH4 + O2
What is the oxide of hydrogen?
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7-10 Types of Chemical Reactions
Combustion Reactions occur when an element or compound combine with oxygen to produce oxides of each element.
H2 + O2
CH4 + O2
What is the oxide of hydrogen? Water
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7-10 Types of Chemical Reactions
Combustion Reactions occur when an element or compound combine with oxygen to produce oxides of each element.
H2 + O2 H2O
CH4 + O2
What is the oxide of hydrogen? Water
And the oxide of carbon?
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7-10 Types of Chemical Reactions
Combustion Reactions occur when an element or compound combine with oxygen to produce oxides of each element.
H2 + O2 H2O
CH4 + O2 CO2 + H2O
What is the oxide of hydrogen? Water
And the oxide of carbon? Carbon dioxide
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7-10 Types of Chemical Reactions
Combustion Reactions occur when an element or compound combine with oxygen to produce oxides of each element.
2H2 + O2 2H2O
CH4 + O2 CO2 + H2O
Now balance
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7-10 Types of Chemical Reactions
Combustion Reactions occur when an element or compound combine with oxygen to produce oxides of each element.
2H2 + O2 2H2O
CH4 + O2 CO2 + 2H2O
Now balance
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7-10 Types of Chemical Reactions
Combustion Reactions occur when an element or compound combine with oxygen to produce oxides of each element.
2H2 + O2 2H2O
CH4 + 2O2 CO2 + 2H2O
Now balance
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7-10 Types of Chemical Reactions
REDOX reactions where the oxidation number changes from reactants to products.
Oxidation is when the oxidation number increases, by losing of electrons.
Reduction is when the oxidation number decreases by gaining electrons.
Consider the following equation:
H2 + O2 H2O
What are the oxidation numbers of hydrogen and oxygen?
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7-10 Types of Chemical Reactions
REDOX reactions where the oxidation number changes from reactants to products.
Oxidation is when the oxidation number increases, by losing of electrons.
Reduction is when the oxidation number decreases by gaining electrons.
Consider the following equation:
H2 + O2 H2O
What are the oxidation numbers of hydrogen and oxygen?
0 0
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7-9 REDOX REACTIONS
H2 + O2 H2O
How about hydrogen and oxygen in water?
00 2(1+) 2- = 0
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7-9 REDOX REACTIONS
H2 + O2 H2O
How about hydrogen and oxygen in water?Oxidation is caused by the oxygen molecule,
so it is referred to as the oxidizing agent (OA)
Reduction is caused by the hydrogen molecule, so it is referred to as the reducing agent (RA)
00 2(1+) 2- = 0
reducedoxidized
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7-9 REDOX REACTIONSNote:
• All of the previously discussed reactions are REDOX except the double replacement reactions.
• The number of electrons lost is equal to the number of electrons gained in a reaction. Why?
• Most elements have variable oxidation numbers, except for hydrogen, oxygen, and the memorized polyatomic ions.
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7-9 REDOX REACTIONSOxidation numbers for a compound must
add up to equal zero, while the oxidation numbers for a polyatomic ion must up to equal the charge of that ion.
Consider the following chlorine compounds
HClO4, HClO3, HClO2, HClO, Cl2, HCl
What is the oxidation number of chlorine in each of these compounds, assuming
H+ and oxygen is 2-
1+ 4(2-)=0
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7-9 REDOX REACTIONSOxidation numbers for a compound must
add up to equal zero, while the oxidation numbers for a polyatomic ion must up to equal the charge of that ion.
Consider the following chlorine compounds
HClO4, HClO3, HClO2, HClO, Cl2, HCl
What is the oxidation number of chlorine in each of these compounds, assuming H is 1+ and oxygen is 2-
1+ 4(2-)=07+
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7-9 REDOX REACTIONSOxidation numbers for a compound must
add up to equal zero, while the oxidation numbers for a polyatomic ion must up to equal the charge of that ion.
Consider the following chlorine compounds
HClO4, HClO3, HClO2, HClO, Cl2, HCl
What is the oxidation number of chlorine in each of these compounds, assuming H is 1+ and oxygen is 2-
1+ 4(2-)=07+ 5+
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7-9 REDOX REACTIONSOxidation numbers for a compound must
add up to equal zero, while the oxidation numbers for a polyatomic ion must up to equal the charge of that ion.
Consider the following chlorine compounds
HClO4, HClO3, HClO2, HClO, Cl2, HCl
What is the oxidation number of chlorine in each of these compounds, assuming H is 1+ and oxygen is 2-
1+ 4(2-)=07+ 5+ 3+
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7-9 REDOX REACTIONSOxidation numbers for a compound must
add up to equal zero, while the oxidation numbers for a polyatomic ion must up to equal the charge of that ion.
Consider the following chlorine compounds
HClO4, HClO3, HClO2, HClO, Cl2, HCl
What is the oxidation number of chlorine in each of these compounds, assuming H is 1+ and oxygen is 2-
1+ 4(2-)=07+ 5+ 3+ 1+
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7-9 REDOX REACTIONSOxidation numbers for a compound must
add up to equal zero, while the oxidation numbers for a polyatomic ion must up to equal the charge of that ion.
Consider the following chlorine compounds
HClO4, HClO3, HClO2, HClO, Cl2, HCl
What is the oxidation number of chlorine in each of these compounds, assuming H is 1+ and oxygen is 2-
1+ 4(2-)=07+ 5+ 3+ 1+ 0
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7-9 REDOX REACTIONSOxidation numbers for a compound must
add up to equal zero, while the oxidation numbers for a polyatomic ion must up to equal the charge of that ion.
Consider the following chlorine compounds
HClO4, HClO3, HClO2, HClO, Cl2, HCl
What is the oxidation number of chlorine in each of these compounds, assuming H is 1+ and oxygen is 2-
1+ 4(2-)=07+ 5+ 3+ 1+ 0 1-
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7-9 REDOX REACTIONS
How about sulfur in SO3 2-
3(2-)=2-
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7-9 REDOX REACTIONS
How about sulfur in SO3 2-
How about carbon in C6H12O6
3(2-)=2-4+
12(1+)+6(2-)=0
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7-9 REDOX REACTIONS
How about sulfur in SO3 2-
How about carbon in C6H12O6
3(2-)=2-4+
12(1+)+6(2-)=00 +
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7-5 Aqueous Ionic CompoundsMost ionic compounds dissolve in water to produce solutions that conduct electricity. The degree to which a solution will conduct electricity is used to determine if a solute is a strong or weak electrolyte. Solutions that do not conduct electricity are called nonelectrolytes. Molecular compounds that dissolve in water to conduct electricity, are acids or bases. Strong acids/bases are referred to as strong electrolytes since they are good conductors of electricity. Weak acid solutions do not conduct electricity well and are called weak electrolytes
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7-5 Aqueous Ionic CompoundsMost ionic compounds dissolve in water to produce solutions that conduct electricity. The degree to which a solution will conduct electricity is used to determine if a solute is a strong or weak electrolyte. Solutions that do not conduct electricity are called nonelectrolytes. Molecular compounds that dissolve in water to conduct electricity, are acids or bases. Strong acids/bases are referred to as strong electrolytes since there solutions are good conductors of electricity. Weak acid/base solutions do not conduct electricity well and are called weak electrolytes.
How do we tell if a solution conducts electricity?
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7-5 Aqueous Ionic Compounds
Strong electrolyte Weak electrolyte Nonelectrolyte
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7-5 Aqueous Ionic CompoundsSolutions are homogeneous mixtures of a solute and a solvent.
• The solute is the solution component in the smallest amount while the solvent is the larger component of a solution.
• Solutes whose solutions conduct electricity are called electrolytes
• Solutes whose solutions do not conduct electricity are called nonelectrolytes
• Electrolytes are solutes that form ions when they dissolve. Ionic solutes or acids usually form solutions that conduct electricity.
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There are some more specific rules that allows us to better estimate the solubility of ionic compounds.
You will be given these if you need them.
7-5 Aqueous Ionic Compounds
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7-6 Precipitation ReactionsUsing the solubility rules on the previous slide asign (s) and (aq) to the formulas for the following equation
NaCl(?) + AgNO3(?) AgCl(?) + NaNO3(?)
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7-6 Precipitation ReactionsUsing the solubility rules on the previous slide asign (s) and (aq) to the formulas for the following equation
NaCl(aq) + AgNO3(?) AgCl(?) + NaNO3(?)
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7-6 Precipitation ReactionsUsing the solubility rules on the previous slide asign (s) and (aq) to the formulas for the following equation
NaCl(aq) + AgNO3(aq) AgCl(?) + NaNO3(?)
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7-6 Precipitation ReactionsUsing the solubility rules on the previous slide asign (s) and (aq) to the formulas for the following equation
NaCl(aq) + AgNO3(aq) AgCl(s) + NaNO3(?)
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7-6 Precipitation ReactionsUsing the solubility rules on the previous slide asign (s) and (aq) to the formulas for the following equation
NaCl(aq) + AgNO3(aq) AgCl(s) + NaNO3(aq)
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7-6 Precipitation ReactionsUsing the solubility rules on the previous slide asign (s) and (aq) to the formulas for the following equation
NaCl(aq) + AgNO3(aq) AgCl(s) + NaNO3(aq)This is called a formula equation
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7-6 Precipitation ReactionsUsing the solubility rules on the previous slide asign (s) and (aq) to the formulas for the following equation
NaCl(aq) + AgNO3(aq) AgCl(s) + NaNO3(aq)This is called a formula equation
When Ionic solids and acids dissolve in water ions are formed, and the aqueous formulas really do not exist. A more realistic equation would be the ionic equation.
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7-6 Precipitation ReactionsNaCl(aq) + AgNO3(aq) AgCl(s) + NaNO3(aq)
formula equationSeparating the aqueous substances into ions produces an ionic equation.
Na+(aq) + Cl-(aq) + Ag+(aq) AgCl(s) + Na+(aq) + NO3- (aq)
ionic equation
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7-6 Precipitation ReactionsNaCl(aq) + AgNO3(aq) AgCl(s) + NaNO3(aq)
formula equationSeparating the aqueous substances into ions produces an ionic equation.
Na+(aq)+Cl-(aq)+Ag+(aq)+NO3-(aq) AgCl(s)+Na+(aq)+NO3
-(aq)
ionic equationSubstances found on both sides of the equation are called spectator ions and are boxed above. Eliminating the spectator ions generates the net ionic equation.
Ag+ (aq) + Cl- (aq) AgCl (s)
Net ionic equation
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7-6 Precipitation Reactions
It is possible for all of the reactants and products to be water soluble and thus produce all spectator ions. If this is the case then all of the ions cancel out and there is no net ionic equation. When this occurs then we say that there is No Reaction, and give the label NR.
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7-6 Precipitation ReactionsFive Driving Forces Favor Chemical Change
1. Formation of a solid (Precipitate formation) 2. Formation of water (acid base reactions)3. Transfer of electrons (REDOX) reaction4. Formation of a gas (many different types)5. Formation of a weak electrolyte (formation weak
acids and bases)
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7-6 Precipitation ReactionsFormation of water is a normal product between acids and bases. Since acids and bases dissolve in water to make solutions that are electrolytes, then we conclude that acids and bases have some ionic character. Since water does not ionize, then when water is formed, we will also have a net ionic equation and then a chemical reaction.
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7-6 Precipitation Reactions
Strong acids and bases ionize 100%!
Memorized Strong acids and bases:
Acids BasesHCl (aq)HI (aq)HBr (aq)HNO3
H2SO4
HClO4
Hydroxides of group I and II metals, except Be and Mg
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Acids undergo characteristic double replacement reactions with oxides, hydroxides, carbonates and bicarbonates.
2HCl (aq) + CuO (s) CuCl2 (aq) + H2O (l)
2HCl (aq) + Ca(OH)2 (aq) CaCl2 (aq) + 2H2O (l)
2HCl (aq) + CaCO3 (aq) CaCl2 (aq) + H2O (l) + CO2 (g)
2HC l (aq) + Sr(HCO3)2 (aq) SrCl2 (aq) + 2H2O (l) + 2CO2 (g)
7-7 Aqueous Reactions
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Acids undergo characteristic double replacement reactions with oxides, hydroxides, carbonates and bicarbonates.
2HCl (aq) + CuO (s) CuCl2 (aq) + H2O (l)
2HCl (aq) + Ca(OH)2 (aq) CaCl2 (aq) + 2H2O (l)
2HCl(aq) +CaCO3(aq) CaCl2 (aq)+H2O (l) +CO2 (g)
2HC l(aq)+Sr(HCO3)2(aq)SrCl2 (aq)+2H2O(l)+ 2CO2
(g)
7-8 Acid/Base Gas Evolution
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Bases undergo a double replacement reaction with acids called neutralization:
NaOH (aq) + HCl (aq) H2O (l) + NaC l (aq)
In words this well known reaction is often described as: “acid plus base = salt plus water”
We previously discussed this reaction when describing types of reactions.
7-8 Acid/Base Gas Evolution
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We have discussed the double replacement reactions and ionic equations before. Since the acids and bases undergo double replacement reactions called neutralization reactions, then they can have ionic equations too.Formula equation:
HCl (aq) + NaOH (aq) NaCl (aq) + H2O (l)
Total ionic equation:
H+ (aq) + Cl- (aq) + Na+ (aq) + OH- (aq) Na+ (aq) + Cl- (aq) + H2O (l)
Net ionic equation:
H+ (aq) + OH- (aq) H2O (l)
7-8 Acid/Base Gas Evolution
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Another property of acids is their reaction with certain metals to produce hydrogen gas, H2 (g).
Zn (s) + 2HC l (aq) H2 (g) + ZnCl2 (aq)
This is an example of a single replacement reaction and is a redox reaction.
Total ionic equation:
Zn (s) + 2H+ (aq) + 2Cl- (aq) H2 (g) + Zn2+ (aq) + 2Cl- (aq)
Net ionic equation:
Zn (s) + 2H+ (aq) H2 (g) + Zn2+ (aq)
7-8 Acid/Base Gas Evolution
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The End