There are several commonly-used definitions for acids and bases. Prior to the 20th century, acids were largely viewed as substances containing oxygen and hydrogen which would react with metals. Around the turn of the 20th century, Svante Arrhenius defined an acid as a substance which could dissociate to generate positively-charged hydrogen ions ([H+], later recognized to exist as hydronium ions, [H3O+]) in solution, while a base would dissociate to form negatively-charged hydroxide ions ([OH-]). Johannes Brønsted and Martin Lowry later expanded this definition, with an acid as a proton donor and a base as a proton acceptor. This meant that a substance could be an acid without forming hydronium ions in solution. Around the same time, Gilbert Lewis developed a theory suggesting that an acid is a substance which could accept an electron pair and a that a base is a substance which can donate an electron pair.
Svante Arrhenius was the first to define acids and bases on a molecular level.
Definitions:
Arrhenius acid- produces H+ in water
Arrhenius base- produces OH- ions in water
There are several definitions give for acids and bases, which are give by various scientists.
Acids produce hydronium ions in solution, and bases produce hydroxide ions in solution.
Svante Arrhenius
By using a ph meter
Each cationic acid HA+, when it donates ONE proton H+, will form its conjugated base A of the acid HA+. (Example: NH4+ ammonium, acid NH3 ammonia, base)Each neutral acid HA, when it donates ONE proton H+, will form its conjugated base A- of the acid HA. (Example: CH3COOH acetic acid CH3COO- acetate, base)Each anionic acid HA-, when it donates ONE proton H+, will form its conjugated base A2- of the acid HA-. (Example: HS- (mono)hydrogen sulfide, acid S2- sulfide, base)Each anionic base HA-, when it adopts ONE proton H+, will form its conjugated acid H2A of the base HA-. (Example: HS- mono-hydrogen sulfide, base H2S di-hydrogen sulfide, acid)Each anionic base A-, when it adopts ONE proton H+, will form its conjugate acid HA of base A-. (Example: CH3COO- acetate, base CH3COOH acetic acid)Each neutral base A, when it adopts ONE proton H+, will form its conjugate acid HA of base A-. (Example: NH3 ammonia, base NH4+ ammonium, acid)
When a strong acid and a strong base neutralize each other the products are a salt and water.
In acid base neutralisation, both the acid and the base react with each other to form salt and water. Ex: hcl+naoh --> nacl + hoh here, acid-hcl base-naoh salt-nacl water-hoh
If an acid and a base completely neutralize each other, their corrosive properties will be nullified and the resulting solution would not be corrosive at all.
An acid base pair which differ from each other by a single proton(H+ ion) is called a conjugate pair. Eg. Acid Base HCl Cl- NH3 NH4+ H2O H3O+
Each cationic acid HA+, when it donates ONE proton H+, will form its conjugated base A of the acid HA+. (Example: NH4+ ammonium, acid NH3 ammonia, base)Each neutral acid HA, when it donates ONE proton H+, will form its conjugated base A- of the acid HA. (Example: CH3COOH acetic acid CH3COO- acetate, base)Each anionic acid HA-, when it donates ONE proton H+, will form its conjugated base A2- of the acid HA-. (Example: HS- (mono)hydrogen sulfide, acid S2- sulfide, base)Each anionic base HA-, when it adopts ONE proton H+, will form its conjugated acid H2A of the base HA-. (Example: HS- mono-hydrogen sulfide, base H2S di-hydrogen sulfide, acid)Each anionic base A-, when it adopts ONE proton H+, will form its conjugate acid HA of base A-. (Example: CH3COO- acetate, base CH3COOH acetic acid)Each neutral base A, when it adopts ONE proton H+, will form its conjugate acid HA of base A-. (Example: NH3 ammonia, base NH4+ ammonium, acid)
When a strong acid and a strong base neutralize each other the products are a salt and water.
They neutralise each other, assuming you neutralise a volume of acid with a base of the same molarity they completely cancel each other out leaving water and a salt. The salt differs depending on the acid and base used.
an acid and a base. also-chemical opposites, for eg. acids and alkalis
A substance
In acid base neutralisation, both the acid and the base react with each other to form salt and water. Ex: hcl+naoh --> nacl + hoh here, acid-hcl base-naoh salt-nacl water-hoh
An acid-base equilibrium is the state in whic the concentrations of acidic and basic ions in a solution neutralize each other.
the kind of base and acid is a chemical bound that go each other.
If an acid and a base completely neutralize each other, their corrosive properties will be nullified and the resulting solution would not be corrosive at all.
Salt
An acid base pair which differ from each other by a single proton(H+ ion) is called a conjugate pair. Eg. Acid Base HCl Cl- NH3 NH4+ H2O H3O+
Answer the answer is when thay are mixed together a chemical reaction happens. Such as explosion occurs. When an acid and a base/alkali are mixed together, a chemical reaction known as neutralization takes place.