Réaksi asam-basa: Béda antarrépisi

'''Réaksi asam-basa''' hartina [[réaksi kimia]] antara [[asam]] jeung [[basa (kimia)|basa]].

 

 

=== Definisi Lavoisier ===

[[Svante Arrhenius]] menyediakan definisi modérn munggaran ngeunaan asam jeung basa ditahun[[1884]]. Dina [[cai]], lumangsung prosés [[konstanta disosiasi|disosiasi]]:

 

 

Sanyawa nu ngabalukarkeun ngaronjatna kadar H⁺ sarta nurunkeun kadar OH^- disebut '''asam''', mun sabalikna, disebut '''basa'''.

 

 

 

Ion positif ti hiji basa bisa ngahasilkeun [[uyah (kimia)|uyah]] jeung ion négatif ti hiji asam. Pikeun conto, dua [[mol]] basa [[natrium hidroksida]] (NaOH) bisa ngagabung jeung sa-mol asam sulfat (H₂SO₄) ngahasilkeun dua mol cai jeung sa-mol natrium [[sulfat]].

 

 

=== Definisi proton (Brønsted-Lowry) ===

Basa hartina akséptor [[proton]]. Dina réaksi asam-basa Brønsted-Lowry, aya kompetisi antara dua basa marebutkeun hiji proton, sahingga mun '''X''' jeung '''Y''' mangrupa dua spésiés, bakal lumangsung kasatimbangan

 

 

Boh HX jeung HY duanana mangrupakeun asam Brønsted-Lowry; boh X^- jeung Y^- duanana mangrupakeun basa Brønsted-Lowry. Mun réaksina leuwih loba lumangsung ka kénca, HY mangrupa asam nu leuwih kuat, sedengkeun X^- basa nu leuwih kuat; mun réaksina géséh ka katuhu, mangka HX asam leuwih kuat, sedengkeun Y^- basa leuwih kuat.

 

If these reactions have equilibrium constants K_X and K_Y respectively, then:

:[X^-][HZ] / [HX][Z^-]=K_X

Acids and bases in the Brønsted-Lowry system occur in '''conjugate pairs'''; in the reaction

 

 

 

 

Stronger acids typically oxidize metals, forming salts and releasing hydrogen.

 

 

=== Definisi pangleyur-sistim ===

This definition is based on a generalization of the earlier Arrhenius definition. If we consider a solvent which can be dissociated into a positive species '''X''' and a negative species '''Y''':

 

or

or

 

 

In this more general sense, aprotic compounds (those which do not donate protons), can still react with bases, and the terms "acid" and "base" can still be used for reactions in aprotic or non-aqueous environments.

The Lewis definition is one of the most broad definitions and is necessary for an understanding of acid-base reaction, although the Brønsted-Lowry definition is sufficient and more practical for most cases in everyday use.

 

 

=== Definisi Usanovich ===

The most general definition is that of the Russian chemist Usanovich, and can basically be summarized as defining an acid as anything that accepts negative species or donates positive ones, and a base as the reverse. This tends to overlap the concept of [[redox]] ([[oxidation]]-[[reduction]]), and so is not highly favored by chemists. This is because redox reactions focus more on physical electron transfer processes, rather than bond making/bond breaking processes, although the distinction between these two processes is somewhat ambiguous.

 

 

* [[Konsép HSAB]]

* [[Konfigurasi éléktron]]

 

 

[[ar:تفاعل حمض-قاعدة]]

[[ca:Reacció àcid-base]]