chapter 7 chapter opener with space shuttle launch chemical...

Chapter 7

Chemical

Reactions

Chapter opener

with space shuttle launch

Chapter 7 Chemical Reactions•7.1 Kindergarten Volcanoes, Automobiles, and Laundry Detergents

•7.2 Evidence of a Chemical Reaction

•7.3 The Chemical Equation

•7.4 How to Write Balanced Chemical Equations

•7.5 Aqueous Solutions, Solubility: Compounds Dissolved in Water

•7.6 Precipitation Reactions: Reactions in Aqueous Solution that

Form Solids

•7.7 Writing Chemical Equations for Reactions in Solution:

Molecular, Complete Ionic, and Net Ionic Equations

•7.8 Acid Base and Gas Evolution Reactions

•7.9 Oxidation-Reduction Reactions

•7.10 Classifying Chemical Reactions

7.1 Kindergarten Volcanoes,

Automobiles, and Laundry

Detergents

Tro's "Introductory Chemistry",

Chapter 7

3

Some chemical reactions

• Kindergarten Volcano with baking soda and

vinegar – shows bubbles

• Gasoline burning – (next slide) releases heat

• Soap scum precipitation out of hard water

• Soap scum dissoilved by laundry detergent

• All these are chemical reactions changes in

composition Tro's "Introductory Chemistry",

Chapter 7

4

5

Combustion Reactions

Reactants + O2 Products

(also heat)

Figure 7.1 octane burning in and

engine with oxygen make carbon

dioxide and water

7.2 Evidence of a Chemical

Reaction


Chapter 7

6


Chapter 7

7

Evidence of Chemical Change

Color Change

Formation of Solid PrecipitateFormation of a Gas

Emission of LightRelease or Absorption of Heat

Five figures on page 202


Chapter 7

8

Evidence of Chemical Change,

ContinuedIs boiling water

a chemical change?

No, there is no change

in composition this

Is a physical change.

Water boiling Figure 7.5


Chapter 7

9

Practice—Decide Whether Each of the

Following Involve a Chemical Reaction.

• Photosynthesis

• Heating sugar until it turns black

• Heating ice until it turns liquid

• Digestion of food

• Dissolving sugar in water

• Burning of alcohol in a flambé dessert

Yes, CO2 and H2O combine into carbohydrates

Yes, sugar decomposing

No, molecules still same

Yes, food decomposing and combining

with stomach acid

No, molecules still same

Yes, alcohol combining with O2 to make CO2 and H2O


Chapter 7

10

7.3The Chemical Equations

Chemical Equations

• A Chemical Equation consists of

Reactants on the left

An arrow

Products on the right

2Na(s) + Cl2(g) 2NaCl(s)

reactants products

The number ―2‖ are called coefficient, which multiply

the number of molecules or formula units 11


Chapter 7

12

The Combustion of Methane

• Methane gas burns to produce carbon dioxide gas and gaseous water.

Whenever something burns it combines with O2(g).

Methane burning Figure on page 205


Chapter 7

13

Combustion of Methane,

Balanced• Tthe equation must be balanced.

Adjust the numbers of molecules so there are equal numbers of atoms of each element on both sides of the arrow.

CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g)

Molecular equation at bottom of

Page 204


Chapter 7

14

Symbols Used in Equations• Symbols used to indicate state.

(g) = gas; (l) = liquid; (s) = solid.

(aq) = aqueous = dissolved in water.

• Energy symbols used above the arrow for

decomposition reactions.

D = heat.

hn = light.

shock = mechanical.

elec = electrical.


Chapter 7

15

7.4 How to Write Balanced Chemical

Equations


Chapter 7

16

Balancing Equations

•There are some tips on balancing equations in your text. On

page 206.

•Most important: Do not change subscruipts, only change

coefficients.

•The goal is to have the same number of each type of atom

on both sides.

•Some examples:

•H2(g) + Cl2(g) HCl(g)

•There are 2 H on left, but 1 on right. 2 in front of HCl

•H2(g) + Cl2(g) 2 HCl(g)

•The equation is balanced.


Chapter 7

17

More examples Example

Cr(s) + O2(g) Cr2O3(s)

• Balance the Cr with a 2

2 Cr(s) + O2(g) Cr2O3(s)

•The right has 2 O but the left has 3 O. Balance

by switch those and there will be 6 O on both sides.

2 Cr(s) + 3O2(g) 2Cr2O3(s)

•This unbalances the Cr, fix by changing the 2 to a 4

4 Cr(s) + 3 O2(g) 2Cr2O3(s)

•Always check at the end.

•4 Cr 4 Cr

•6 O 6 O

18

Another Example

FcCl3(aq) + NaOH Fe(OH)3(s) + NaCl(aq)

•Balance the Cl with a 3

FcCl3(aq) + NaOH Fe(OH)3(s) + 3 NaCl(aq)

•Balance the Na with a 3

FcCl3(aq) + 3 NaOH Fe(OH)3(s) + 3NaCl(aq)

•All other elements are balanced


Chapter 7

19

Predicting Whether a Reaction

Will Occur in Aqueous Solution• ―Forces‖ that drive a reaction:

Formation of a solid. (Precipitation)

Formation of water. (Happens in acid + base)

Formation of a gas.

Transfer of electrons. (Called oxidation-reduction)

• We will look at each type of reaction

Aqueous Solutions, Solubility:

Compounds Dissolved in Water


Chapter 7

20


Chapter 7

21

Aqueous Solutions

Aqueous solutions are a substance (solute) dissolved in water

(solvent). The resulting mixture is a solution.

Ionic solids that dissolve in water dissociate (or break up) into ions

That are surrounded by water in solution. Do nmot break apart

Polyatomic ions. Subbscipts Coefficents

NaCl(s) Na+(aq) + Cl-(aq)

MgCl2(s) Mg2+(aq) + 2 Cl–(aq)

Al2 (SO4) 3(s) 2Al3+(aq) + 3SO42-(aq)


Chapter 7

22

Dissociation of soluble ionic

compounds

Figure of NaCl and AgNO3 in

solution on page 209


Chapter 7

23

Dissociation, Continued• Potassium iodide dissociates in water into

potassium cations and iodide anions.

KI(aq) → K+1(aq) + I-1(aq)

• Copper(II) sulfate dissociates in water into

copper(II) cations and sulfate anions.

CuSO4(aq) → Cu+2(aq) + SO4-2(aq)


Chapter 7

24

Dissociation, Continued

• Potassium sulfate dissociates in water into

potassium cations and sulfate anions.

K2SO4(aq) → 2 K+1(aq) + SO4-2(aq)


Chapter 7

25

Electrolytes

• Electrolytes are

substances whose water

solution is a conductor

of electricity.

• All electrolytes have

ions dissolved in water.

Figures left side

Page 209


Chapter 7

26

Electrolytes, Continued

• In strong electrolytes, 100% of

formula units are separated into

ions.

• In nonelectrolytes, none of the

molecules are separated into

ions.

• In weak electrolytes, a small

percentage of the molecules are

separated into ions.


Chapter 7

27

Types of Electrolytes

• Salts = Water soluble ionic compounds.

Strong electrolytes.

• Acids = Form H+ ions and anions in water solution.

In binary acids, the anion is monoatomic. In oxyacids, the anion

is polyatomic.

Sour taste.

React and dissolve many metals.

Strong acid = strong electrolyte, weak acid = weak electrolyte.

• Bases = Water-soluble metal hydroxides.

Bitter taste, slippery (soapy) feeling solutions.

Increases the OH- concentration.


Chapter 7

28

When Will a Salt Dissolve?

• A compound is soluble in a liquid if it dissolves in that liquid.

• The compound is a solute, the liquid is a solvent, and the mixture is a solution.

NaCl is soluble in water, but AgCl is not soluble.

NaCl top beaker

Page 209

AgCl bottom beaker

Page 209

Solubility Rules•A set of solubility rules have been

developed to help predict when a

compound will dissolve

•Two tables show these rules

•Soluble compounds with exceptions

•Insoluble compounds with exceptions

•These tables will be provided with the

quiz


Chapter 7

30

Compounds containing the

following ions are generally

soluble

Exceptions

(when combined with ions on the

left the compound is insoluble)

Li+, Na+, K+, NH4+ none

NO3–, C2H3O2

– none

Cl–, Br–, I– Ag+, Hg22+, Pb2+

SO42– Ca2+, Sr2+, Ba2+, Pb2+

Solubility Rules:

Compounds that Are Generally Soluble in Water


Chapter 7

31

Compounds containing the

following ions are generally

insoluble

Exceptions

(when combined with ions on the

left the compound is soluble or

slightly soluble)

OH– Li+, Na+, K+, NH4+,

Ca2+, Sr2+, Ba2+

S2– Li+, Na+, K+, NH4+,

Ca2+, Sr2+, Ba2+

CO32–, PO4

3– Li+, Na+, K+, NH4+

Solubility Rules:

Compounds that Are Generally Insoluble


Chapter 7

32

Using the Solubility Rules to Predict an Ionic If a

Precipitation Reaction occurs in Water

• Dissociate soluble compounds into ions

• Check combinations of cations and anions for

solubility using the rules.

• If cation is Li+, Na+, K+, or NH4+, then the

compound will be soluble in water.

• If another cation, follow the rules for the anion.

• If a precipitate forms, use charges to write correct

formula for the precipitate and the other product.

33

Determine if Each of the Following Is Soluble

in Water

• KOH K+ and OH-

soluble, all K+ compounds are soluble

• AgBr Ag+ and Br-

insoluble, all Br- are soluble, but Ag+ is an exception.

• CaCl2 Ca2+ and Cl-

Soluble, all Cl- are soluble, and Ca2+ is not an exception

• Pb(NO3)2 Pb2+ and NO3-

Soluble, All NO3- are soluble.

• PbCO3 Pb2+ and CO42-

Insoluble, CO32- are usually insoluble , but Pb2+ is not an

exception.

Compounds ions

7.6 Precipitation Reactions:

Reactions in Aqueous Solution

that Form Solids


Chapter 7

34


Chapter 7

35

Precipitation

Reactions

A precipitate forming


Chapter 7

36

Precipitation Reactions, Continued

2 KI(aq) + Pb(NO3)2(aq) 2 KNO3(aq) + PbI2(s)

Figure 7.7, the above reaction


Chapter 7

37

Precipitation Reactions, Continued

2 KI(aq) + Pb(NO3)2(aq) 2 KNO3(aq) + PbI2(s)

Beakers on page 212 illustrating

this precipitation


Chapter 7

38

No Precipitate Formation =

No ReactionKI(aq) + NaCl(aq) KCl(aq) + NaI(aq)

All ions still present, no reaction.

Figure 7.8 illustrating no reaction

Predicting if a precipitate will form


Chapter 7

39

•Dissociate soluble ionic compounds into ions.

•Look at possible combinations of cations and anions,

and use the solubility rules top determine if a precipitate

will form.

•If a precipitate forms determine its formula from ioninc

charges. Alos the formula of soluble products.

•Write a balanced equations.

•A mixture is made of solutions of potassium phosphate

and nickel(II)chloride. Will a precipitate form?

•K3PO4(aq) + NiCl2(aq) precipitate ??

Predicting Precipitates (continued)


Chapter 7

40

K3PO4(aq) + NiCl2(aq) precipitate ??

Dissoiciate (number of ions is not important at this point

K+ PO43- Ni 2+ Cl-

insoluble

soluble

Inner combination is insoluble because PO43- compounds are

insoluble and Ni2+ is not an exception.

The outer combination is soluble because K+ compounds

are always soluble.

Predicting Precipitates (continued)


Chapter 7

41

K+ and Cl- make KCl(aq)

Ni 2+ and PO43- make Ni3(PO4)2(s)

Reactants and products:

K3PO4(aq) + NiCl2(aq) KCl(aq) + Ni3(PO4)2(s)

And balance:

2K3PO4(aq) + 3NiCl2(aq) 6KCl(aq) + Ni3(PO4)2(s)

7.7 Writing Chemical Equations

for Reactions in Solution:

Molecular, Complete Ionic, and

Net Ionic Equations


Chapter 7

42

Ionic Equations


Chapter 7

43

•The equations listed in the previous section identify

the precipitate and soluble compounds.

•These equations do not reflect the actual structure of

the species in solution.

•Ionic equations reveal the actual state of ionics.


Chapter 7

44

Ionic Equations

• molecular equations.

All compounds complete:

2 KOH(aq) + Mg(NO3)2(aq) 2 KNO3(aq) + Mg(OH)2(s)

• complete ionic equations.

Aqueous electrolytes are written as ions.

Soluble salts, strong acids, strong bases.

Insoluble substances and nonelectrolytes written in intact form.

Solids, liquids, and gases are not dissolved, therefore, molecule form.

2K+(aq) + 2OH-

(aq) + Mg+2(aq) + 2NO3

-(aq) K+

(aq) + 2NO3-(aq) + Mg(OH)2(s)


Chapter 7

45

Ionic Equations

• spectator ions. Species that are identical on both sides

2K+(aq) + 2OH-

(aq) + Mg+2(aq) + 2NO3

-(aq) K+

(aq) + 2NO3-(aq) + Mg(OH)2(s)

•When spectator ions are removed the result is thenet ionic equation:

2OH-1(aq) + Mg+2

(aq) Mg(OH)2(s)

Another example• Molecular equations.

All compounds complete:

K2(SO4) (aq) + Ba(NO3)2(aq) 2 KNO3(aq) + BaSO4(s)

• Ionic Equation :

As the supecies actually appear in solution:• 2K+

(aq) + SO42-

(aq) + Ba+2(aq) + 2NO3

-(aq) K+

(aq) + 2NO3-(aq) + BaSO4(s)

• Net Ionic Equation:

Spectator ions removed

Ba+2(aq) + 2NO3

-(aq) BaSO4(s) 46


Chapter 7

47

Summary

• A molecular equation is a chemical

equation showing the complete, neutral

formulas for each compound in a reaction.

• A complete ionic equation is a chemical

equation showing all of the species as they

are actually present in solution.

• A net ionic equation is an equation

showing only the species that actually

participate in the reaction.

7.8 Acid Base and Gas Evolution

Reactions


Chapter 7

48


Chapter 7

49

Properties of Acids• Sour taste.

• Change color of vegetable dyes.

• React with ―active‖ metals, not noble

metals to produce hydrogen.

i.e., Al, Zn, Fe, but not Cu, Ag or Au.

Zn + 2 HCl ZnCl2 + H2

Corrosive.

• React with carbonates, producing CO2.

Marble, baking soda, chalk, limestone.

CaCO3 + 2 HCl CaCl2 + CO2 + H2O

• React with bases to form ionic salts.

And often water.

A woman eating

a lemon

Litmus paper

changing to

red


Chapter 7

50

Common Acids

Chemical name Formula Old name Strength

Nitric acid HNO3 Aqua fortis Strong

Sulfuric acid H2SO4 Vitriolic acid Strong

Hydrochloric acid HCl Muriatic acid Strong

Phosphoric acid H3PO4 Moderate

Chloric acid HClO3 Moderate

Acetic acid HC2H3O2 Vinegar Weak

Hydrofluoric acid HF Weak

Carbonic acid H2CO3 Soda water Weak

Boric acid H3BO3 Weak


Chapter 7

51

Properties of Bases

• A.k.a. alkalis.

• Taste bitter.

• Feel slippery.

• Change color of vegetable dyes.

Different color than acid.

Litmus = blue.

• React with acids to form ionic salts.

And often water.

Neutralization.

Litmus paper

changing to

blue


Chapter 7

52

Common BasesChemical

name

Formula Common

name

Strength

Sodium

hydroxide

NaOH Lye,

caustic soda

Strong

Potassium

hydroxide

KOH Caustic potash Strong

Calcium

hydroxide

Ca(OH)2 Slaked lime Strong

Magnesium

hydroxide

Mg(OH)2 Milk of magnesia Weak

Ammonium

hydroxide

NH4OH,

{NH3(aq)}

Ammonia water,

aqueous ammonia

Weak


Chapter 7

53

Acid–Base Reactions• Also called neutralization reactions.• the H+ from the acid and OH- from the base make water.• The cation from the base combines with the anion from

the acid to make the salt (salt = ionic compound).

acid + base salt + water

2 HNO3(aq) + Ca(OH)2(aq) Ca(NO3)2(aq) + 2 H2O(l)

• Ionic Equation:

2H+(aq) + 2NO3

-(aq) + Ca+2

(aq) + 2OH-(aq) H+

(aq) + 2NO3-(aq) + H2O (l)

• The net ionic equation for an acid-base reaction often is:

H+(aq) + OH-(aq) H2O(l)


Chapter 7

54

Gas Evolution Reactions• gas evolution reactions.

• Directly from the ion exchange.

K2S(aq) + H2SO4(aq) K2SO4(aq) + H2S(g)

• decomposition of an unstable ion exchange products into a gas and water.

K2SO3(aq) + H2SO4(aq) K2SO4(aq) + ―H2SO3(aq)‖

The quotes indicate the compound is unstable.

H2SO3 H2O(l) + SO2(g)

Final equation:K2SO3(aq) + H2SO4(aq) K2SO4(aq) + H2O(l) + SO2(g)

Gas evolving

page 218


Chapter 7

55

Compounds that Undergo

Gas Evolving Reactions

Reactant

type

Reacting

with

Ion

exchange

product

Decom-

pose?

Gas

formed

Example

MetalnS,

metal HS

Acid H2S No H2S K2S(aq) + 2HCl(aq)

2KCl(aq) + H2S(g)

MetalnCO3,

metal HCO3

Acid H2CO3 Yes CO2 K2CO3(aq) + 2HCl(aq)

2KCl(aq) + CO2(g) + H2O(l)

MetalnSO3

metal HSO3

Acid H2SO3 Yes SO2 K2SO3(aq) + 2HCl(aq)

2KCl(aq) + SO2(g) + H2O(l)

(NH4)nanion Base NH4OH Yes NH3 KOH(aq) + NH4Cl(aq)

KCl(aq) + NH3(g) + H2O(l)

Molecular, Total Ionic, and Net

Ionic for Gas Evolving Reaction

(Example 1)


Chapter 7

56

Initial Equation (before carbonic acid breaks down)

K2SO3(s) + 2 HCl(aq) 2KCl(aq) + ―H2SO3(aq)‖

Molecular Equation

K2SO3(s) + 2 HCl(aq) 2KCl(aq) + + H2O(l) + SO2(g)

Ionic Equation2K+

(aq) + SO32-(s) + 2H+

(aq) + 2Cl-(aq) K+

(aq) + Cl-(aq) + H2O (l) + SO2(g)

Net Ionic Equation

+ SO32-(s) + 2H+

(aq) H2O (l) + SO2(g)

Molecular, Total Ionic, and Net

Ionic for Gas Evolving Reaction

(Example 2)


Chapter 7

57

Initial Equation (before carbonic acid breaks down)

CaCO3(s) + 2 HCl(aq) CaCl2(aq) + ―H2CO3(aq)‖

Molecular Equation

CaCO3(s) + 2 HCl(aq) CaCl2(aq) + H2O(l) + CO2(aq)

Ionic Equation

CaCO3(s) + 2H+(aq) + 2Cl-

(aq) Ca2+(aq) + 2Cl- + H2O (l) + CO2(g)

Net Ionic Equation

CaCO3(s) + 2H+(aq) + Ca2+

(aq) + H2O (l) + CO2(g)

7.9 Oxidation-Reduction

Reactions


Chapter 7

58

Oxidation/Reduction


Chapter 7

59

•Metal + a non-metal

Ca(s) + Cl2(g) CaCl2 (s)

•Combustion with oxygen

2C4H8 (g) + 6O2(g) 4CO2(g) + 4H2O(l)

•More general: electrons are transferred

•LEO says GER

•Loss of Electrons is Oxidation

•Gain of Electreons is Reduction


Chapter 7

60

Oxidation–Reduction Reactions

• The element that loses electrons in the reaction is oxidized.

• Substance that gains electrons in the reaction is reduced.

• You cannot have one without the other.

• In combustion, the O atoms in O2 are reduced, and the non-O atoms in the other material are oxidized.


Chapter 7

61

Combustion as Redox

• In the following reaction:

2 Mg(s) + O2(g) 2 MgO(s)

• The magnesium atoms are oxidized.

2Mg0 2Mg2+ + 4 e

• The oxygen atoms are reduced.

O20 + 4 e 2O2

• Adding the oxidation and reduction cancels

the electrons and gives the overall reaction


Chapter 7

62

Combustion as Redox, Continued• Even though the following reaction does not involve ion

formation, electrons are still transferred.

CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g)

• The carbon atoms are oxidized.

C4 C4+ + 8 e

These are not charges, they are called oxidation numbers, but they help us see the electron transfer.

• The oxygen atoms are reduced.

4O0 + 8 e 4O2-


Chapter 7

63

Reactions of Metals with Nonmetals

(Oxidation–Reduction)• Metals react with nonmetals to form ionic compounds.

Ionic compounds are solids at room temperature.

• The metal loses electrons and becomes a cation.

The metal undergoes oxidation.

• The nonmetal gains electrons and becomes an anion.

The nonmetal undergoes reduction.

• In the reaction, electrons are transferred from the metal to the nonmetal.

2 Na(s) + Cl2(g) NaCl(s)


Chapter 7

64

Ionic Compound Formation

as Redox

• In the reaction:

Mg(s) + Cl2(g) MgCl2(s)

• The magnesium atoms are oxidized.

Mg0 Mg2+ + 2 e

• The chlorine atoms are reduced.

2Cl0 + 2 e 2Cl

65

Recognizing Redox Reactions• O2 is a reactant or a product.

• Any reaction between a metal and a nonmetal.

• Any reaction where electrons are transferred is redox.

When a free element gets combined

N2(g) + H2(g) NH3(g)

Nitrogen (-3) reduced and hydrogen (0 +1) oxidized

When a metal cation changes its charge, it will be either oxidized if its charge increases or reduced if its charge decreases.

Cu(s) + 2AgCl(aq) CuCl2(aq) + 2Ag(s)

Net equation:

Cu0(s) + 2Ag+(aq) Cu2+(aq) + 2Ag0 (s)

Copper (0 2+) is oxidized, and silver (1+ 0) is reduced.

A free element (uncombined) like Cu(s), Ag(s), or O2(g) has charge zero


Chapter 7

66

Practice—Decide Whether Each of the

Following Reactions Is a Redox Reaction.

2 Al(s) + 3 Br2(l) 2 AlBr3(s) redox (metal + nonmetal)

Ba(NO3)2(s) + 2 KCl(aq) BaCl2(s) + KNO3(aq) Not redox

Fe2O3(s) + C(s) 2 Fe(s) + 3 CO(g) redox (Fe3+ Fe0)

SO2(g) + O2(g) + H2O(l) H2SO4(aq) redox (O2 combines)

67

Classifying Reactions

• One way is based on the process that happens.

Precipitation, neutralization, formation of a gas, or

transfer of electrons.

Figure on page 222

68

Classifying Reactions, Continued• Another scheme classifies reactions by what

the atoms do. We studied this in lab.

Type of reaction General equation

Synthesis A + B AB

Decomposition AB A + B

Displacement A + BC AC + B

Double displacement AB + CD AD + CB

Figure on Page 225


Chapter 7

69

Synthesis Reactions

• composition or combination reactions.

• Two (or more) reactants combine together to

make one product.

Simpler substances combining together.

2 CO + O2 2 CO2

2 Mg + O2 2 MgO

HgI2 + 2 KI K2HgI4


Chapter 7

70

Decomposition Reactions

• A large molecule is broken apart into smaller molecules or its elements.

Have only one reactant, make 2 or more products.

2h

3

2

223

O 3 O 2

O Hg 2 HgO 2

Cl FeCl 2 FeCl 2

D

)(

)()()(

g(l)(s)

glselec


Chapter 7

71

Decomposition of Water

(g)(g)(l) 22elec

2 O H 2 OH 2

Figure upper left page 224


Chapter 7

72

Single Displacement Reactions

• One atom displacing another and replacing it in a compound.

• Zn(s) + 2 HCl(aq) ZnCl2(aq) + H2(g),

Zn displaces H.

• Other examples of displacement reactions are:

Fe2O3(s) + Al(s) Fe(s) + Al2O3(s)

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


Chapter 7

73

Double Displacement Reactions

• Two ionic compounds exchange ions.

• May be followed by decomposition of one

of the products to make a gas.

• X Yq (aq) + A Bq (aq) XB + AY

• Precipitation, acid–base, and gas evolving

reactions are also double displacement

reactions.


Chapter 7

74

Examples of Double Displacement

Precipitation

CaCl2(aq) + Na2CO3(aq) CaCO3(s) + 2 NaCl(aq)

Acid base

Ba(OH)2(s) + 2 HNO3(aq) Ba(NO3)2(aq) + 2 H2O(l)

Gas evolving

Li2CO3(aq) + 2 HCl(aq) 2 LiCl(aq) + CO2(g) + H2O(l)

chapter 7 chapter opener with space shuttle launch chemical...

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