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Write a balanced ionic equation for the acid base reaction of an oxide ion with...

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Write a balanced ionic equation for the acid base reaction of an oxide ion with water...

with water acting as the acid. Label the conjugate acid and the conjugate base and state how many protons are transferred between water and the oxide ion as a base.

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Posted (Answer #1)

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5.1 Exchange Reactions:
Precipitation and Net
Ionic Equations 136
5.2 Acids, Bases, and
Acid-Base Exchange
Reactions 143
5.3 Oxidation-Reduction
Reactions 151
5.4 Oxidation Numbers
and Redox Reactions 155
5.5 Displacement
Reactions, Redox, and
the Activity Series 159
5.6 Solution
Concentration 161
5.7 Molarity and Reactions
in Aqueous Solutions 166
5.8 Aqueous Solution
Titrations 168

hemistry is concerned with how substances react and what products are
formed when they react. A chemical compound can consist of molecules or
oppositely charged ions, and often the compound’s properties can be deduced
from the behavior of these molecules or ions. The chemical properties of a compound
are the transformations that the molecules or ions can undergo when the substance
reacts. A central focus of chemistry is providing answers to questions such as these:
When two substances are mixed, will a chemical reaction occur? If a chemical reaction occurs, what will the products be?

As you saw in Chapter 4 ( p. 101), most reactions of simple ionic and molecular compounds can be assigned to a few general categories: combination, decomposition, displacement, and exchange. In this chapter we discuss chemical reactions in
more detail, including oxidation-reduction reactions. The ability to recognize which
type of reaction occurs for a particular set of reactants will allow you to predict the
Chemical reactions involving exchange of ions to form precipitates are discussed
first, followed by net ionic equations, which focus on the active participants in such
reactions. We then consider acid-base reactions, neutralization reactions, and reactions
that form gases as products. Next comes a discussion of oxidation-reduction (redox)
reactions, oxidation numbers as a means to organize our understanding of redox reactions, and the activity series of metals.
A great deal of chemistry—perhaps most—occurs in solution, and we introduce
the means for quantitatively describing the concentrations of solutes in solutions. This
discussion is followed by explorations of solution stoichiometry and finally aqueous
titration, an analytical technique that is used to measure solute concentrations.

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Many of the ionic compounds that you frequently encounter, such as table salt, baking
soda, and household plant fertilizers, are soluble in water. It is therefore tempting to
conclude that all ionic compounds are soluble in water, but such is not the case.
Although many ionic compounds are water-soluble, some are only slightly soluble, and
others dissolve hardly at all.
When an ionic compound dissolves in water, its ions separate and become surrounded by water molecules, as illustrated in Figure 5.1a. The process in which ions
separate is called dissociation. Soluble ionic compounds are one type of strong electrolyte. Recall that an electrolyte is a substance whose aqueous solution contains ions

Group 1A: Li

, Na

, All Group 1A (alkali metal) and ammonium salts are soluble.

, Rb

, Cs

ammonium NH4

Nitrates: NO3

All nitrates are soluble.
Chlorides, bromides, All common chlorides, bromides, and iodides are soluble except
iodides: Cl

, Br

, I

AgCl, Hg2
, PbCl2
, AgBr, Hg2
, PbBr2
, AgI, Hg2
, PbI2
Sulfates: SO4
Most sulfates are soluble; exceptions include CaSO4
, SrSO4
, and PbSO4
Chlorates, ClO3

All chlorates are soluble.
Perchlorates, ClO4

All perchlorates are soluble.
Acetates, CH3

All acetates are soluble.
Usually Insoluble
Phosphates, PO4
All phosphates are insoluble except those of NH4

and Group 1A
elements (alkali metal cations).
Carbonates, CO3
All carbonates are insoluble except those of NH4

and Group 1A
elements (alkali metal cations).
Hydroxides, OH

All hydroxides are insoluble except those of NH4

and Group 1A
(alkali metal cations). Sr(OH)2
, Ba(OH)2
, and Ca(OH)2
are slightly
Oxalates, C2O4
All oxalates are insoluble except those of NH4

and Group 1A
(alkali metal cations).
Suldes, S
All suldes are insoluble except those of NH4

, Group 1A (alkali
metal cations) and Group 2A (MgS, CaS, and BaS are sparingly

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Posted (Answer #3)

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and therefore conducts electricity. A strong electrolyte is completely converted to
ions when it forms an aqueous solution. By contrast, most water-soluble molecular
compounds do not ionize when they dissolve. This is illustrated in Figure 5.1b.
The solubility rules given in Table 5.1 are general guidelines for predicting the
water solubilities of ionic compounds based on the ions they contain. If a compound
contains at least one of the ions indicated for soluble compounds in Table 5.1, then
the compound is at least moderately soluble.
Figure 5.2 shows examples illustrating the solubility rules for a few nitrates,
hydroxides, and suldes. Suppose you want to know whether NiSO4
is soluble in
water. NiSO4
contains Ni
and SO4
ions. Although Ni
is not mentioned in Table 5.1,
substances containing SO4
are described as soluble (except for SrSO4
, BaSO4
, and
). Because NiSO4
contains an ion, SO4
, that indicates solubility and NiSO4
is not
one of the sulfate exceptions, it is predicted to be soluble.

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Posted (Answer #4)

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^^she is right

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