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How can you justify that NH3 is bronsted Lowry base but not arrhenius base?
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An arrhenius acid is an bronsted lowry acid bt an arrhenius base is NT a bronsted lowry base?
no, arhenious base is also a bronsted lowry base
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-
Why is methylamine a bronsted-lowry base but not an arrhenius base?
Because it may accept the proton but can not donate the 'OH-' ion.
An arrhenius acid is an bronsted lowry acid bt an arrhenius base is NT a bronsted lowry base?
no, arhenious base is also a bronsted lowry base
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-
What is the definition of a bronsted-Lowry base?
A Bronsted-Lowry base is a proton acceptor.
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.
Is ammonium ion NH4 a Bronsted-Lowry base?
Yes, the ammonium ion NH4 is a Bronsted-Lowry base.
Why is methylamine a bronsted-lowry base but not an arrhenius base?
Because it may accept the proton but can not donate the 'OH-' ion.
What is true of a Bronsted -Lowry base?
A Bronsted-Lowery base accepts H+ ions
What is true of the bronsted-lowry base?
A Bronsted-Lowery base accepts H+ ions
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.
