the Arrhenius definitions stated that acids would donate a Hydrogen (H+)in water and a base would donate a hydroxide(OH-) in water, but would limit to substances with those "parts" like ammonia for example because it could do both.....
It had so many limitations which was found out by the later scientists; Bronsted and Lowry, who came up with their theories afterwards
According to Arrhenius, acids produce a proton in aqueous solution, and bases produce a hydroxide ion in aqueous solution. Hydrochloric acid is an Arrhenius acid because it gives up its proton as it dissolves in water. Sodium hydroxide is an Arrhenius base because it gives up its hydroxide as it dissolves in water.
The Arrhenius definition of acids and bases explains a number of things. Arrhenius's theory explains why all acids have similar properties to each other (and, conversely, why all bases are similar): because all acids release H+ into solution (and all bases release OH-). The Arrhenius definition also explains Boyle's observation that acids and bases counteract each other. This idea, that a base can make an acid weaker, and vice versa, is called neutralization. hope that helped
Arrhenius, Bronsted-Lowry, and Lewis theories of acids and bases
Acids were compounds with hydrogen that ionized when aqueous to form H+. Bases were compounds that ionized when aqueous to form OH- (hydroxide).
It had so many limitations which was found out by the later scientists; Bronsted and Lowry, who came up with their theories afterwards
According to Arrhenius, acids produce a proton in aqueous solution, and bases produce a hydroxide ion in aqueous solution. Hydrochloric acid is an Arrhenius acid because it gives up its proton as it dissolves in water. Sodium hydroxide is an Arrhenius base because it gives up its hydroxide as it dissolves in water.
The Arrhenius definition of acids and bases explains a number of things. Arrhenius's theory explains why all acids have similar properties to each other (and, conversely, why all bases are similar): because all acids release H+ into solution (and all bases release OH-). The Arrhenius definition also explains Boyle's observation that acids and bases counteract each other. This idea, that a base can make an acid weaker, and vice versa, is called neutralization. hope that helped
salt and water
Arrhenius, Bronsted-Lowry, and Lewis theories of acids and bases
Acids were compounds with hydrogen that ionized when aqueous to form H+. Bases were compounds that ionized when aqueous to form OH- (hydroxide).
because arrhenius model does not include some elementa as they dont contain hydroxide before the reaction
There are several commonly-used definitions for acids and bases. Prior to the 20th century, acids were largely viewed as substances containing oxygen and hydrogen which would react with metals. Around the turn of the 20th century, Svante Arrhenius defined an acid as a substance which could dissociate to generate positively-charged hydrogen ions ([H+], later recognized to exist as hydronium ions, [H3O+]) in solution, while a base would dissociate to form negatively-charged hydroxide ions ([OH-]). Johannes Brønsted and Martin Lowry later expanded this definition, with an acid as a proton donor and a base as a proton acceptor. This meant that a substance could be an acid without forming hydronium ions in solution. Around the same time, Gilbert Lewis developed a theory suggesting that an acid is a substance which could accept an electron pair and a that a base is a substance which can donate an electron pair.
All acids and bases are electrolytes. Some are more powerful than others, depending on the extent of ionization and dissociation of the solution.
Acids and bases have many definitions, but for your question, these will do: Bases are proton (H+) acceptors. Acids are proton (H+) releasers.
Bronsted and Lowry.
Yes, because all Arrhenius bases contain OH- ions which accept the proton.