Is water an acid or a base according to the arrhenius theory?
water can be both an acid and a base.
H2O + H+ = H3O+
H2O + HCO3-= H2CO3 +OH-
H2O + H+ = H3O+
H2O + HCO3-= H2CO3 +OH-
Why water is called an amphoteric substance?
According to Bronsted concept
Water can act as an acid by losing a proton as
H2O-------->OH- + H+
Water can act as a base by gaining a proton as
H2O+ H+---------------->H3O+
Water can act as an acid by losing a proton as
H2O-------->OH- + H+
Water can act as a base by gaining a proton as
H2O+ H+---------------->H3O+
Why/How is
Hydronium (H3O) positively charged?
H2O + H+ --> H3O+
I see that due to the conversation of charge, both sides should have a net charge of +1, but I don't see how is the hydronium positively charged.
The H+ has a dative covalent bond with the H2O so hydrogen's s-orbital should be complete, hence the charge should be zero.
Is this due to the electronegativity of the H2O molecule?
I will appreciate it if you could explain to me what I am missing here
I see that due to the conversation of charge, both sides should have a net charge of +1, but I don't see how is the hydronium positively charged.
The H+ has a dative covalent bond with the H2O so hydrogen's s-orbital should be complete, hence the charge should be zero.
Is this due to the electronegativity of the H2O molecule?
I will appreciate it if you could explain to me what I am missing here
well H20 has a charge of 0
Two H's give you a +2 Charge and then you have one O (oxide has a charge of -2) therefore H20 has a zero charge
your adding something that has a charge of 0 to something that has a charge of 1(H)
thats why the result is H3O+
Two H's give you a +2 Charge and then you have one O (oxide has a charge of -2) therefore H20 has a zero charge
your adding something that has a charge of 0 to something that has a charge of 1(H)
thats why the result is H3O+
Hydronium
In chemistry,
a hydronium ion
is the cation
H3O+, a type of oxonium ion
produced by protonation of water and isoelectronic with ammonia.
This cation is often used to represent the nature of the proton in
aqueous solution, where the proton is highly solvated
(bound to a solvent). The reality is far more complicated, and a proton is
bound to several molecules of water, such that other descriptions such as H5O2+,
H7O3+ and H9O4+
are increasingly accurate descriptions of the environment of a proton in water.[3]
The ion H3O+ has been detected
in the gas phase.
Determination of pH
It is
the presence of hydronium ion relative to hydroxide that
determines a solution's pH. Water molecules
auto-dissociate into hydronium and hydroxide ions in the
following equilibrium:
2 H2O OH− + H3O+
In pure water, there is an equal number of hydroxide and
hydronium ions. At 25 °C and atmospheric pressure their concentrations are
approximately equal to 1.0 × 10−7 mol∙dm−3.
For these conditions, [H3O+] = 10−pH
so pH = 7 is defined as neutral. A pH value less than 7 indicates an
acidic solution, and a pH value more than 7 indicates a basic solution. Note
that [H3O+]×[OH−], the ionic product of
water, strongly increases with temperature so [H3O+]
is not equal to 10−pH for temperatures other than 25 °C.
Structure
Since O+ and N have the same number of electrons, H3O+ is isoelectronic
with ammonia.
As shown in the images above, H3O+
has a trigonal pyramid geometry with the oxygen atom at its apex. The H-O-H
bond angle is approximately 113°,[6]
and the center of mass is very close to the oxygen atom. Because the base of
the pyramid is made up of three identical hydrogen atoms, the H3O+ molecule's symmetric top
configuration is such that it belongs to the C3v point group. Because of
this symmetry and the fact that it has a dipole moment, the rotational
selection rules are ΔJ = ±1 and ΔK = 0. The transition
dipole lies along the c axis and, because the negative charge is localized near
the oxygen atom, the dipole moment points to the apex, perpendicular to the
base plane.
Acids and acidity
Hydronium
is the cation that forms from water in the presence of hydrogen ions.
These hydrons do not exist in a
free state: they are extremely reactive and are solvated
by water. An acidic
solute is generally the source of these hydrons; however, hydroniums exist even
in pure water. This special case of water reacting with water to produce
hydronium (and hydroxide) ions is commonly known as the self-ionization of water. The resulting
hydronium ions are few and short-lived. pH is a measure of the relative
activity of hydronium and hydroxide ions in aqueous solutions. In acidic
solutions, hydronium is the more active, its excess proton being readily
available for reaction with basic species.
Hydronium
is very acidic: at 25 °C, its pKa is -1.74. It is also the most acidic species that can
exist in water (assuming sufficient water for dissolution)(see leveling
effect): any stronger acid will ionize and protonate a water
molecule to form hydronium. The acidity of hydronium is the implicit standard
used to judge the strength of an acid in water: strong acids
must be better proton donors than hydronium, otherwise a significant portion of
acid will exist in a non-ionized state. Unlike hydronium in neutral solutions
that result from water's autodissociation, hydronium ions in acidic solutions
are long-lasting and concentrated, in proportion to the strength of the
dissolved acid.
pH was
originally conceived to be a measure of the hydrogen ion
concentration of aqueous solution.[7]
We now know that virtually all such free protons quickly react with water to
form hydronium; acidity of an aqueous solution is therefore more accurately
characterized by its hydronium concentration. In organic syntheses, such as
acid catalyzed reactions, the hydronium ion (H3O+)
can be used interchangeably with the H+ ion; choosing one over the
other has no significant effect on the mechanism of reaction.
Solvation
Researchers
have yet to fully characterize the solvation
of hydronium ion in water, in part because many different meanings of solvation
exist. A freezing-point depression study determined
that the mean hydration ion in cold water is approximately H3O+(H2O)6:[8]
on average, each hydronium ion is solvated by 6 water molecules which are
unable to solvate other solute molecules.
Some
hydration structures are quite large: the H3O+(H2O)20
magic ion number structure (called magic because of its increased
stability with respect to hydration structures involving a comparable number of
water molecules) might place the hydronium inside a dodecahedral
cage.[9]
However, more recent ab initio method molecular
dynamics simulations have shown that, on average, the hydrated proton resides
on the surface of the H3O+(H2O)20
cluster.[10]
Further, several disparate features of these simulations agree with their
experimental counterparts suggesting an alternative interpretation of the
experimental results.
Zundel cation
Two
other well-known structures are the Zundel cations and Eigen cations.
The Eigen solvation structure has the hydronium ion at the center of an H9O+4 complex in which the hydronium is strongly hydrogen-bonded
to three neighbouring water molecules. In the Zundel H5O+ complex the proton is shared equally by two water molecules in a symmetric hydrogen bond. Recent work
indicates that both of these complexes represent ideal structures in a more
general hydrogen bond network defect.
Isolation
of the hydronium ion monomer in liquid phase was achieved in a nonaqueous, low
nucleophilicity superacid solution (HF-SbF5SO2).
The ion was characterized by high resolution O-17 nuclear magnetic resonance.
A 2007
calculation of the enthalpies and free energies of the various hydrogen
bonds around the hydronium cation in liquid protonated water at room
temperature and a study of the proton hopping mechanism using molecular dynamics showed that the
hydrogen-bonds around the hydronium ion (formed with the three water ligands in the
first solvation shell of the hydronium) are quite strong compared to those of
bulk water.
A new
model was proposed by Stoyanov based on infrared spectroscopy in which the proton exists as an H13O+6 ion. The positive charge is thus delocalized over
six water molecules.
Solid hydronium salts
For
many strong acids,
it is possible to form crystals of their hydronium salt that are relatively
stable. Sometimes these salts are called acid monohydrates. As a rule,
any acid with an ionization constant of 109 or higher
may do this. Acids whose ionization constant is below 109 generally
cannot form stable H3O+ salts.
For example, hydrochloric acid has an ionization constant of
107, and mixtures with water at all proportions are liquid at room
temperature. However, perchloric acid has an ionization constant of
1010, and if liquid anhydrous perchloric acid and water are combined
in a 1:1 molar ratio, solid hydronium perchlorate forms.
The
hydronium ion also forms stable compounds with the carborane superacid H(CB11H(CH3)5B6).
X-ray crystallography shows a C3v
symmetry
for the hydronium ion with each proton interacting with a bromine atom each
from three carborane anions 320 pm apart on average. The [H3O][H(CB11HCl)]11 salt is also soluble in benzene.
In crystals grown from a benzene solution the solvent co-crystallizes and a H3O·(benzene)3 cation is completely
separated from the anion. In the cation three benzene molecules surround
hydronium forming pi-cation
interactions with the hydrogen atoms. The closest (non-bonding) approach of the
anion at chlorine to the cation at oxygen is 348 pm.
There
are also many examples of hydrated hydronium ions known, such as the H5O+2 ion in HCl·2H2O,
the H7O+3 and H9O+4 ions both found in HBr·4H2O.
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