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Transcript of Double-Replacement Reactions in Water. Objectives: Describe aqueous solutions Write complete ionic...
![Page 1: Double-Replacement Reactions in Water. Objectives: Describe aqueous solutions Write complete ionic and net ionic equations for reactions in aqueous solutions.](https://reader036.fdocuments.in/reader036/viewer/2022062511/5519ca4d550346443e8b4808/html5/thumbnails/1.jpg)
Reactions in Aqueous SolutionsDouble-Replacement Reactions in Water
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Objectives:Describe aqueous solutionsWrite complete ionic and net ionic equations
for reactions in aqueous solutionsPredict whether reactions in aqueous
solutions will produce a precipitate, water, or a gas
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Reactions in Water are Vital…70% of Earth covered by H2O
Your body is 60-70% H2O
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Aqueous SolutionsAqueous from “Aqua” (Latin for water)Aqueous Solution = Water with stuff
dissolved in itSolute = The stuff that is dissolvedSolvent = The most plentiful substance in the
solutionWater = The solvent in an aqueous solution
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SolutesThere are many
possible solutes—sugar and alcohol are molecular compounds that exist as molecules in aqueous solutions.
Compounds that produce hydrogen ions in aqueous solutions are acids.
Ionic compounds can also be solutes in aqueous solutions.
When ionic compounds dissolve in water, their ions separate in a process called dissociation.
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Types of Reactions in aqueous solutionsWhen two solutions
that contain ions as solutes are combined, the ions might react.
If they react, it is always a double replacement reaction.
Three products can form: precipitates, water, or gases
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Reactions that form solid precipitatesAqueous solutions of
sodium hydroxide and copper(II) chloride react to form the precipitate copper(II) hydroxide.
2NaOH(aq) + CuCl2(aq) →
2NaCl(aq) + Cu(OH)2(s)
Ionic equations that show all of the particles in a solution as they actually exist are called complete ionic equations.
2Na+(aq) + 2OH–(aq) + Cu2+ (aq)+ 2Cl–(aq) →
2Na+(aq) + 2Cl–(aq) + Cu(OH)2(s)
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Ions that do not participate in a reaction are called spectator ions and are not usually written in ionic equations.
Formulas that include only the particles that participate in reactions are called net ionic equations:
2OH–(aq) + Cu2+(aq) → Cu(OH)2(s)
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Reactions that produce WaterSome reactions
produce more water molecules.
No evidence of a chemical reaction is observable.
HBr(aq) + NaOH(aq) → H2O(l) + NaBr(aq)
Without spectator ions:H+(aq) + OH–(aq) → H2O(l)
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Reactions that form gasesGases that are
commonly produced are carbon dioxide, hydrogen cyanide, and hydrogen sulfide.
2HI(aq) + Li2S(aq)→ H2S(g) + 2LiI(aq)
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Reactions that form gasesAnother example is mixing an acid and
baking soda, which produces carbon dioxide gas:
HCl(aq) + NaHCO3(aq) → H2CO3(aq) + NaCl(aq)
H2CO3(aq) (carbonic acid) decomposes immediately:H2CO3(aq) → H2O(l) + CO2(g)
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Combining ReactionsTwo reactions can be combined and
represented by a single chemical reaction.
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Combining ReactionsReaction 1
HCl(aq) + NaHCO3(aq) → H2CO3(aq) + NaCl(aq)
Reaction 2 H2CO3(aq) → H2O(l) + CO2(g)
Combined equationHCl(aq) + NaHCO3(aq) + H2CO3(aq) → H2CO3(aq)
+ NaCl(aq) + H2O(l) + CO2(g)
Overall equationHCl(aq) + NaHCO3(aq) → H2O(l) + CO2(g) +
NaCl(aq)
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Baking Soda + Acid
This is what makes cakes rise!
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ReviewReactions between ionic compounds in water
produce a gas, a solid precipitate, or a liquid (H2O, usually)
These reactions are double replacement reactionsChemists write aqueous reactions as ionic
equations – these show the ions dissolved in water and their interactions
A net ionic equation shows only those ions that interact to produce a solid, liquid or gaseous product
You can combine reactions and cancel out the ions and compounds that appear as both reactants and products.