The Bronsted-Lowry definition of an acid is a species which can give up an H+ ion, and HSO4- can deprotonate to give SO42- and H+. This is where the second hydrogen ion from sulfuric acid comes from.
H2O can act as both a Bronsted acid and a Bronsted base. As an acid, it can donate a proton (H+) to another species, and as a base, it can accept a proton. The role it plays depends on the context of the reaction.
Hydrochloric acid (HCl) is an example of a Bronsted-Lowry acid. It donates a proton (H+) in solution.
Water can act as both a Brønsted-Lowry acid and base. As an acid, it donates a proton (H+) to a base; as a base, it accepts a proton from an acid. This ability is due to its amphiprotic nature.
Yes, bicarbonate (HCO3-) can act as both a Bronsted-Lowry acid and a base. As an acid, it donates a proton (H+) to another substance, while as a base, it accepts a proton. This ability to both donate and accept protons makes it amphiprotic.
It is a Bronsted base.
The Bronsted-Lowry definition of an acid is a species which can give up an H+ ion, and HSO4- can deprotonate to give SO42- and H+. This is where the second hydrogen ion from sulfuric acid comes from.
H2O can act as both a Bronsted acid and a Bronsted base. As an acid, it can donate a proton (H+) to another species, and as a base, it can accept a proton. The role it plays depends on the context of the reaction.
Hydrochloric acid (HCl) is an example of a Bronsted-Lowry acid. It donates a proton (H+) in solution.
Yes, ephedrine sulfate is a salt formed by the reaction between the weak base ephedrine and the strong acid sulfuric acid. This results in a salt that has properties of both an acid and a base.
Water can act as both a Brønsted-Lowry acid and base. As an acid, it donates a proton (H+) to a base; as a base, it accepts a proton from an acid. This ability is due to its amphiprotic nature.
Yes, bicarbonate (HCO3-) can act as both a Bronsted-Lowry acid and a base. As an acid, it donates a proton (H+) to another substance, while as a base, it accepts a proton. This ability to both donate and accept protons makes it amphiprotic.
Bronsted and Lowry expanded the definition of an acid from just donating a proton to also include the ability to accept a pair of electrons. This broader definition includes reactions where molecules can both donate and accept protons, leading to a more comprehensive understanding of acid-base reactions.
Sulfuric acid reacts easily with sodium hydroxide to form sodium sulfate and water because sulfuric acid is a strong acid and sodium hydroxide is a strong base. This reaction occurs because both acids and bases react to form water and a salt. Hydrochloric acid may not react in the same way because it is a weaker acid compared to sulfuric acid.
Water can act as both an acid and a base in a Brønsted-Lowry reaction due to its ability to donate a proton (H+) to another species, making it an acid, or accept a proton from another species, making it a base. This dual nature of water is due to the presence of both a hydrogen ion (H+) and a hydroxide ion (OH-) within its structure.
Sulfuric acid and calcium hydroxide react to form calcium sulfate and water in a neutralization reaction.
Yes, a Brønsted-Lowry acid can be a different concept from an Arrhenius acid. While both concepts define acids based on their ability to donate protons, the Arrhenius definition is limited to substances that produce H+ ions in aqueous solutions, whereas the Brønsted-Lowry definition extends to reactions that occur in non-aqueous solvents.