5. Acids & Bases

because you know i'm all about that base

arrhenius acid

a substance that dissociates in water to produce H+ ions

arrhenius monobasic acid

dissociates in water to give one H+ ion

arrhenius dibasic acid

dissociates in water to give two H+ ions

arrhenius strong acid

a substance that almost completely dissociates in water to give hydrogen ions

arrhenius weak acid

a substance that only slightly dissociates in water to give hydrogen ions

arrhenius base

a substance that dissociates in water to produce OH- ions

arrhenius strong base

a substance that almost completely dissociates in water to produce OH- ions

arrhenius weak base

a substance that only slightly dissociates in water to give OH- ions

arrhenius theory limitations

only applies in aqueous solutions, h+ ions do not exist independently in solution, does not explain amphiprotic substances

bronsted-lowry mnemonic device

aciD - Donor, basE - accEptor

bronsted-lowry acid

proton donor

bronsted-lowry strong acid

good proton donor

bronsted-lowry weak acid

poor proton donor

bronsted-lowry base

proton acceptor

bronsted-lowry strong base

good proton acceptor

bronsted-lowry weak base

poor proton acceptor

amphoteric/amphiprotic substance

a substance that can donate or accept protons

conjugate acid-base pair

any pair consisting of an acid and a base that differ by one proton

conjugate base

an acid changes into a conjugate base when it donates a proton

conjugate acid

a base changes into a conjugate acid when it accepts a proton

neutralisation

the reaction between an acid and a base to form a salt and water

a salt

the substance formed when the hydrogen ion from an acid is replaced by a metal or an ammonium ion

everyday examples of neutralisation

alka seltzer to neutralise excess HCl in stomach, toothpaste contains a base to neutralise the acids in food

everyday acids

lemon juice, vinegar

everyday bases

soap, baking soda