Bronsted Base
It is a Bronsted base.
A Bronsted-Lowry base is a proton acceptor.
A Bronsted-Lowry Acid Donates H+ ions
Depending on the type of acid/base (Arrhenius, Bronsted, Lewis), the acid donates protons and a base doesn't but accepts protons, or the base donates OH- and the acid doesn't, or the acid accepts a pair of electrons and the base donates a pair of electrons. They are just different, that's why.
Yes, the ammonium ion NH4 is a Bronsted-Lowry base.
It is a Bronsted base.
Sulfuric acid is a Bronsted acid because it donates a proton (H+) in an acid-base reaction. It can act as a proton donor but not as a proton acceptor, which is the characteristic of a Bronsted base.
A Bronsted-Lowry acid is a substance that donates a proton (H) in a chemical reaction, while a Bronsted-Lowry base is a substance that accepts a proton. To determine if a substance is a Bronsted-Lowry acid or base, you can look at its behavior in a reaction - if it donates a proton, it is an acid, and if it accepts a proton, it is a base.
ClO2- is a Brønsted base as it can accept a proton (H+ ion) to form HClO2.
Phosphate ion (PO4 3-) acts as a base in the Bronsted-Lowry acid-base theory by accepting a proton (H+).
Yes, that's correct. An Arrhenius acid releases H+ ions in water, making it a Bronsted-Lowry acid. On the other hand, an Arrhenius base releases OH- ions in water but may not necessarily donate or accept protons in other reactions, so it is not always considered a Bronsted-Lowry base.
As the name sulfuric acid might indicate, it is a bronsted-lowry acid.
NH4+ is a Bronsted acid because it can donate a proton (H+) to another molecule or ion.
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.
Theophylline can act as a Bronsted base because it can accept a proton (H+) to form a conjugate acid. In its basic form, theophylline has a lone pair of electrons on the nitrogen atom that can readily accept a proton, making it a base.
NH3 is a bronsted base. It has a lone pair.
An acid donates an H+, and a base accepts an H+. (apex).