An acid donates an H+, and a base accepts an H+. (apex).
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.
An acid donates an H+, and a base accepts an H+. (apex).
A Bronsted-Lowery base accepts H+ ions
A Bronsted-Lowry base is a substance that is a proton acceptor. This means it can accept a proton (H+) from another substance in a chemical reaction. Examples of Bronsted-Lowry bases include hydroxide ions (OH-) and ammonia (NH3).
A Bronsted-Lowry base is a substance that accepts a proton in a chemical reaction. It can donate a pair of electrons to form a new bond with a proton. In water, Bronsted-Lowry bases can form hydroxide ions (OH-) when they accept a proton.
No, PbI2 is not a Bronsted-Lowry acid. Bronsted-Lowry acids are substances that donate a proton (H+ ion) in a reaction, whereas PbI2 is lead iodide, which does not contain any hydrogen ions to donate.
A Bronsted-Lowry Acid Donates H+ ions
A Bronsted-Lowry Acid Donates H+ ions
A Bronsted-Lowry base is a substance that can accept a proton or donate an electron pair. It is a proton acceptor in a chemical reaction.
A Bronsted-Lowry base is a proton acceptor.
A Bronsted-Lowery base accepts H+ ions
Yes, the ammonium ion NH4 is a Bronsted-Lowry base.