Chemistry: acids and bases

• 1887 - year when the Arrhenius theory is made
• Neutralization reaction - acid + base = salt + water
• Swedish - The nationality of Arrhenius
• Svante Arrhenius - the full name of the scientist that made the theory in 1887
• Arrhenius Theory - states that an acid is any compound that produces H+ ions in aqueous solution, while a base is any compound that produces OH- ions in aqueous solution.
• Arrhenius acid - a substance which has a hydrogen atom and can easily give hydrogen ion or proton in its aqueous solution is called as
• Arrhenius acid - any species that increases the concentration of H+ in aqueous solution.
• Basicity - termed as the number of replaceable hydrogen ions present in an acid
• Monobasic acid - acid with a basicity of 1
• Dibasic acid - an acid with a basicity of 2
• Tribasic acid - an acid with a basicity of 3
• Arrhenius base - substances that dissolve in water to release hydroxide ions (OH-)
• Salt - is any ionic compound made by combining an acid with a base
• 1923 - bronsted lowry proposed this new set of definition for acid and base
• Johannes bronsted - bronsted's full name
• Thomas lowry - lowry's full name
• Bronsted lowry acid - any substance that can donate a proton (H+) to another molecule
• Bronsted lowry base - is any substance that can accept a proton from another molecule.
• Water - H+ ion would combine with the OH- ion to make the molecule what?
• Monoprotic acid - are acids that can donate one hydrogen ion per molecule.
• Diprotic acid - are acids that can donate two hydrogen ions per molecule.
• Triprotic acid - are acids that can donate three hydrogen ions per molecule.
• Amphoteric - A compound that can act as either an acid or a base is called as
• Hydrogen carbonate - ion is also an example of amphoteric compound.
• Water - act as an acid by donating a proton, and can act as a base by accepting a proton
• Conjugate acid - formed when a base accepts a proton.
• Conjugate base - are formed when an acid donates a proton.
• Ammonium ion - is the conjugate acid
• OH - ion is the conjugate base.
• pH - potential of hydrogen
• Acidic - pH of a solution ranging from 1-7 are usuall
• Basic - pH of a solution ranging from 7-14 are usually
• Neutral - pH of a solution which is 7 are
• Buffer solution - one which resists changes in pH when small quantities of an acid or an alkali are added to it.
• Acidic buffer - solution is the one which has a pH less than 7. Acidic buffer solutions are commonly made from a weak acid and one of its salts often a sodium salt.