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Title: Reactions in Aqueous Solutions
Description: These notes are for first semester of general chemistry.
Description: These notes are for first semester of general chemistry.
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Chem
...
Mack/S15
Net Ionic Equations:
Reactions in Aqueous Solutions
One of the most important components of this course is the ability to predict and write the products of
reactions in aqueous solutions
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AX + BY → AY + BX
There are several types of these reactions that you will encounter, they are classified as follows:
• Precipitation Reactions: Reaction where and insoluble solid forms
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• Reduction and Oxidation (RedOx) Reactions: Electron transfer reactions
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The reactants in such reactions are generally strong electrolytes
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If the cation from one reactant can form an insoluble
compound with the anion from the other reactant, precipitation occurs
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It is your responsibility to learn these rules,
there is a chart available to download on the Lab web page for the course
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A white precipitate forms
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AgNO3(aq) + NaCl(aq) → NaNO3(aq) + AgCl(s)
Since all sodium and nitrate containing salts are strong electrolytes, silver chloride must be the ppt
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A base is a substance that produces OH−(aq) or accepts a proton (H+) in solution
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This information is in your
nomenclature handout and in the text
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2HCl(aq) + Ba(OH)2 (aq) → BaCl2 (aq) + 2H2 0(l)
Gas−Forming reactions: When the exchange of cations and anions produce a compound that is an insoluble gas,
often bubbles or an odorous gas will ensue
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Other gases that my form are CO2, SO2 and NH3 for
instance
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Page 1 of 2
Chem
...
Mack/S15
Net Ionic Equations: Writing the molecular, ionic, and net ionic equations for a chemical reaction in aqueous
solution
...
Write the balanced molecular equation which gives the complete chemical formula and the phase (s, l, g or
aq) and products
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2
...
3
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These are the ions that appear as both reactants and products in the ionic
equation
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What remains is the net ionic equation
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Molecular Equation: 2HCl(aq) + Ba(OH)2 (aq) → BaCl2 (aq) + 2H2 0(l)
Ionic Equation: 2H + (aq) + 2Cl − (aq) + Ba2+ (aq) + 2OH − (aq) → Ba2+ (aq) + 2Cl − (aq) + 2H2O(l)
Result: 2H + (aq) + 2OH − (aq) → 2H2O(l)
Net Ionic Equatoin: H + (aq) + OH − (aq) → H2O(l)
Reduction and Oxidation Reactions (RedOx): When a chemical species undergoes oxidation, the change
involves an atom or compound losing electrons
...
Neither process can occur alone… that is, there must be an exchange of electrons in the process
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When a substance loses electrons its charge or oxidation number becomes more positive
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Please refer to your text and class notes for the details on assigning oxidation
numbers
...
KMnO4
K = +1, O = −2
Since the compound must have a charge of zero overall we can write:
(+1) + (?) + 4×(−2) = 0
Mn = +7
Example:
When solid copper is placed in a solution of silver ions, solid silver forms at the surface of the
copper
...
Reduced
Oxidized
+
Cu(s) →
2Ag(s)
+
Cu2+(aq)
2Ag+(aq)
Oxidizing
Reducing
Agent
Agent
Copper is oxidized since its oxidation number increases from 0 to +2 (loss of 2 electrons)
Page 2 of 2
Title: Reactions in Aqueous Solutions
Description: These notes are for first semester of general chemistry.
Description: These notes are for first semester of general chemistry.