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An acid donates an H+, and a base accepts an H+. - Apex
A Bronsted-Lowery base accepts H+ ions
The simplest way to answer this is to say that water can act as an acid or a base - giving up a proton (H+) or taking one. When put with an acid, it acts as a base and therefore accepts the proton from the acid. acid + base <---> acid + base HCl + H2O <---> Cl- + H3O+
A Brønsted-Lowry base accepts H+ ions.
Brønsted-Lowry acid-base theory
A Bronsted-Lowry base is a proton acceptor.
A Bronsted-Lowry base accepts a proton from something else.
A base accept protons.
An acid donates an H+, and a base accepts an H+. - Apex
It is basic, as it accepts a proton (Bronsted-Lowry base). It is the conjugate base of nitric acid.
Ammonia accepts H+ ions to form NH4+ ions. Bases are proton acceptors
Vinegar is dilute acetic acid, which is an acid.
Ammonia NH3 behaves as a base when it reacts with an acid because it accepts a proton and becomes NH4+.
The Svante Arrhenius definition of an acid is a compound that donates a hydrogen ion (or proton) in an aqueous solution.
The base in a chemical reaction is the species that either (a) accepts a proton, (b) produces an OH- ion, or (c) is an electron donor.
A Bronsted-Lowery base accepts H+ ions
The simplest way to answer this is to say that water can act as an acid or a base - giving up a proton (H+) or taking one. When put with an acid, it acts as a base and therefore accepts the proton from the acid. acid + base <---> acid + base HCl + H2O <---> Cl- + H3O+