Analysis of information sources in references of the Wikipedia article "Teoria ácido-base de Brønsted-Lowry" in Portuguese language version.
The self-ionization of water is another example of water being able to react either as an acid or a base. [...] One water molecule can transfer a proton to another water molecule. One water molecule acts as an acid and the other acts as a base. [...] Equal quantities of H3O+ and OH- are made.
In the reaction of boric acid with water, [...] B(OH)3 is an electron receptor and a Lewis acid, but in this case, the water molecule is the proton donor.
The Lux/Flood definition defines an acid as an oxide ion acceptor and a base as an oxide ion donor.
If the reaction is viewed in reverse a new acid and base can be identified. The substances on the right side of the equation are called conjugate acid and conjugate base compared to those on the left. Also note that the original acid turns in the conjugate base after the reaction is over.
This definition encompasses the Brønsted-Lowry definition, in that H+ is an electron pair acceptor (when interacting with a base), and a base is an electron pair donor in its interaction with H+.
An acid–base reaction forms an adduct, which is a compound with a coordinate covalent bond in which both electrons are provided by only one of the atom, [...] such as ammonia to form an acid–base adduct, as shown here for boron trifluoride (BF3).
Other molecules can also act as either an acid or a base. For example, Al(OH)3+3H+→Al3++3H2O where Al(OH)3 is acting as a Lewis Base. Al(OH)3+OH−→Al(OH)−4 where Al(OH)3 is acting as an Lewis Acid.
In a strongly acidic solution, [...] consider the reaction of Al(OH)3 with HCl. [...] This is a classic acid-base neutralization reaction. [...] Now consider aluminum hydroxide’s reaction in a strongly basic solution. [...] Here, aluminum hydroxide picks up an hydroxide ion out of solution, thereby acting as a Lewis acid.
According to Brønsted-Lowry definition, acidity of [...] acid HA [...] in solvent S is defined using equation 2.1.
If the reaction is viewed in reverse a new acid and base can be identified. The substances on the right side of the equation are called conjugate acid and conjugate base compared to those on the left. Also note that the original acid turns in the conjugate base after the reaction is over.
The self-ionization of water is another example of water being able to react either as an acid or a base. [...] One water molecule can transfer a proton to another water molecule. One water molecule acts as an acid and the other acts as a base. [...] Equal quantities of H3O+ and OH- are made.
According to Brønsted-Lowry definition, acidity of [...] acid HA [...] in solvent S is defined using equation 2.1.
This definition encompasses the Brønsted-Lowry definition, in that H+ is an electron pair acceptor (when interacting with a base), and a base is an electron pair donor in its interaction with H+.
An acid–base reaction forms an adduct, which is a compound with a coordinate covalent bond in which both electrons are provided by only one of the atom, [...] such as ammonia to form an acid–base adduct, as shown here for boron trifluoride (BF3).
In the reaction of boric acid with water, [...] B(OH)3 is an electron receptor and a Lewis acid, but in this case, the water molecule is the proton donor.
Other molecules can also act as either an acid or a base. For example, Al(OH)3+3H+→Al3++3H2O where Al(OH)3 is acting as a Lewis Base. Al(OH)3+OH−→Al(OH)−4 where Al(OH)3 is acting as an Lewis Acid.
In a strongly acidic solution, [...] consider the reaction of Al(OH)3 with HCl. [...] This is a classic acid-base neutralization reaction. [...] Now consider aluminum hydroxide’s reaction in a strongly basic solution. [...] Here, aluminum hydroxide picks up an hydroxide ion out of solution, thereby acting as a Lewis acid.
The Lux/Flood definition defines an acid as an oxide ion acceptor and a base as an oxide ion donor.
According to Brønsted-Lowry definition, acidity of [...] acid HA [...] in solvent S is defined using equation 2.1.
