0
An arrhenius acid is an bronsted lowry acid bt an arrhenius base is NT a bronsted lowry base?
Wiki User
∙ 14y ago
no, arhenious base is also a bronsted lowry base
Wiki User
∙ 14y ago
Add your answer:
Earn +20 pts
Could a bronsted-lowry acid not be an arrhenius acid?
Since protons are always transferred in the Arrenhius concept, all Arrhenius acid/base reactions are also Bronsted-Lowry acid/base reactions.
What are the three Acid Base Theories?
Arrhenius, Bronsted-Lowry, and Lewis theories of acids and bases
In the reaction co32- H2O -- hco3- oh- the carbonate ion is acting as an a arrhenius base b arrhenius acid c bronsted-lowry base d bronsted-lowry acid?
The Bronsted-Lowry definition describes acids as being proton (H+) donators and bases as being proton acceptors. So the answer would be C, because the carbonate anion is accepting a proton (H+ cation) to become the HCO3-
Is sulfuric acid a bronsted-lowry acid or base?
As the name sulfuric acid might indicate, it is a bronsted-lowry acid.
How does the Bronsted-Lowry definition of an acid differ from the Arrhenius definition of an acid?
Because some acids contribute H+ directly to the base so the H+ will not be found in the solution.
Could a bronsted-lowry acid not be an arrhenius acid?
Since protons are always transferred in the Arrenhius concept, all Arrhenius acid/base reactions are also Bronsted-Lowry acid/base reactions.
What are the three Acid Base Theories?
Arrhenius, Bronsted-Lowry, and Lewis theories of acids and bases
What are the bronsted - lowry definition of acid and base?
Arrhenius: Acid is a proton (H+) donor. Base is a -OH^- (hydroxyl) donor.B-L: Acid is a proton donor. Base is a proton acceptor.
In the reaction co32- H2O -- hco3- oh- the carbonate ion is acting as an a arrhenius base b arrhenius acid c bronsted-lowry base d bronsted-lowry acid?
The Bronsted-Lowry definition describes acids as being proton (H+) donators and bases as being proton acceptors. So the answer would be C, because the carbonate anion is accepting a proton (H+ cation) to become the HCO3-
Is sulfuric acid a bronsted-lowry acid or base?
As the name sulfuric acid might indicate, it is a bronsted-lowry acid.
How does the Bronsted-Lowry definition of an acid differ from the Arrhenius definition of an acid?
Because some acids contribute H+ directly to the base so the H+ will not be found in the solution.
Why is the Brønsted-Lowry definition of acids more general than the Arrhenius definition?
A Brønsted-Lowry base accepts H+ ions.
What is true of the bronsted-lowry base?
A Bronsted-Lowery base accepts H+ ions
What scientists described a base as a compound that accepts a proton?
The Svante Arrhenius definition of an acid is a compound that donates a hydrogen ion (or proton) in an aqueous solution.
In a Bronsted-Lowry acid-base reaction the original acid becomes a what?
The product will be a conjugate base.
What is true about bronsted-lowry base?
A conjugate base is considered the deprotonated acid.
What defines an acid and a base?
Depending on the definition you use. An Arrhenius acid / base is one that gives a H+ / OH- ion when dissociated in water. A Bronsted-Lowry acid is a proton donor (since a hydrogen ion without its valence electron is a proton), while a Bronsted-Lowry base is defined as one which accepts a H+ ion from the acid. This helps explain why substances without OH- (Na2CO3) react with acids. A Lewis acid is one that can accept an electron pair, and a Lewis base is one which can donate an electron pair. As a result, a Lewis base is necessarily a Bronsted-Lowry base, though the converse may not be true
