Chapter 7 reactions in aqueous solution
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Chapter 7–Reactions in Aqueous Solution. Electrolytes Writing Chemical Equations for Aqueous Reactions Double Displacement or Exchange Reactions Precipitation Acid-Base Gas Formation Oxidation-Reduction Reactions (Redox) Single Displacement or Replacement Combustion

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Chapter 7–Reactions in Aqueous Solution

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Chapter 7 reactions in aqueous solution

Chapter 7–Reactions in Aqueous Solution

  • Electrolytes

  • Writing Chemical Equations for Aqueous Reactions

  • Double Displacement or Exchange Reactions

    • Precipitation

    • Acid-Base

    • Gas Formation

  • Oxidation-Reduction Reactions (Redox)

    • Single Displacement or Replacement

    • Combustion

    • Synthesis or Combination

    • Decomposition


Example 1 three ways of writing chemical equations

Example 1 – Three Ways of Writing Chemical Equations

Write balanced molecular, complete ionic,

and net ionic equations for the following

reactions:

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

  • H2SO4(aq) + KOH (aq)  H2O(l) + K2SO4(aq)


Solubility rules for ionic compounds

Solubility Rules for Ionic Compounds

  • Compounds containing Group IA metals, ammonium, acetates and nitrates are allsoluble.

  • Most halides (Group 7Al, chlorides, etc.) are soluble. Exceptions include Ag+, Pb2+, and Hg22+ halides.

  • Most sulfates are soluble. Exceptions include Ba+2, Sr2+, Ag+, Pb2+, and Ca2+ sulfates.

  • Most hydroxidesinsoluble. Exceptions include hydroxides of Group 1A metals, ammonium, Ca+2, Sr+2, and Ba+2.

  • Most phosphates, carbonates, chromates, and sulfides are insoluble. Exceptions include those compounds containing Group 1A metals and ammonium.

  • In addition, allacids are soluble!


Example 2 precipitation

Example 2 - Precipitation

Write balanced molecular, complete ionic,

and net ionic equations for the reactions

you would expect to occur when the

following reagents are combined. If no

reaction occurs, just write NO REACTION

after the arrow.

a. Li2SO4(aq) + Pb(NO3)2(aq) 

b. K3PO4(aq) + NaBr(aq) 


Example 3 neutralization

Example 3 - Neutralization

Write balanced molecular, complete ionic,

and net ionic equations for the reactions

you would expect to occur when the

following reagents are combined. If no

reaction occurs, just write NO REACTION

after the arrow.

a. HI(aq) + NaOH(aq) 

b. H2SO4(aq) + Sr(OH)2(aq) 


Example 4 gas formation

Example 4 – Gas Formation

Write balanced molecular, complete ionic,

and net ionic equations for the reactions you

would expect to occur when the following reagents

are combined. If no reaction occurs, just write NO

REACTION after the arrow.

a. HCl(aq) + Na2CO3(aq) 

b. HNO3(aq) + KHSO4(aq) 

c. NH4Cl(aq) + KOH(aq) 


Chapter 7 reactions in aqueous solution

Activity Series for Metals(and Hydrogen)


Example 5 single displacement

Example 5 – Single Displacement

Write balanced molecular equations for the

reactions you would expect to occur when

the following reagents are combined. If no

reaction occurs, just write NO REACTION

after the arrow.

a. Fe(s) + Ni(NO3)2(aq) 

b. Au(s) + ZnCl2(aq) 

c. Ca(s) + HCl(aq) 


Example 6 classifying reactions

Example 6 – Classifying Reactions

Classify each of the following reactions. Note that

a reaction may fall into more than one category.

  • Ca(s) + 2 H2O(l)  Ca(OH)2(aq) + H2(g)

  • Ba(NO3)2(aq) + K2S04(aq)  BaSO4(s) + 2KNO3(aq)

  • 2 C2H6(g) + 7 O2(g)  4 CO2(g) + 6 H2O(g)

  • 2 KClO3(s)  2 KCl(s) + 3 O2(g)

  • 2 HBr(aq) + Ca(OH)2(aq)  2 H2O(l) + CaBr2(aq)

  • 2 H2(g) + O2(g)  2 H2O(g)


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