U2- Acids + Bases

a species that donates a proton, H+, during an acid-base reaction

change colour of some indicators (exception eg is phenolphthalein indicator) tend to be corrosive sour react w bases pH<7 solutions can conduct electric current (bc covalent molecules can ionise and ions are free to move and carry e charge)

a species that accepts a proton, H+, during an acid-base reaction

soluble base that dissociates (splits up) hydroxide ions

red litmus -> blue slippery bitter caustic (react w living tissue) react w acids pH>7 (alkali only) solutions can conduct electric current (alkali only)

process by which a chemical species gains or loses an electric charge

process by which a molecule separates into smaller particles

[BAWS] salt (aq) + water (l)

[MASH] salt (aq) + hydrogen gas (g)

[CAWCS] salt (aq) + carbon dioxide (g) + water (l)

NH3 (aq) + H2O (l) –> NH4+(aq) + OH-(aq) base. acid. conj acid. conj base.

can either donate or accept a proton, H+ eg H2O, HSO4-

species that donates one/two/three/multiple protons, H+, during ionisation

how readily an acid or base donates or accepts a proton, H+

undergo almost complete ionisation when added to water. Almost all acid molecules in solution will donate proton to form aqueous H+ ions good conductors eg sulfuric acid hydrochloric acid nitric acid

does not readily donate a proton, H+, in a solution. More reactant acid molecules present I'm solution that product of H+ ions hence <--> poor conductors eg ammonium ethanoic acid carbonic acid

readily accepts a proton, H+ and dissociates to form OH- ions and a basic solution in an acid-base reaction eg O2- OH- HPO4 2- H- S2-

doesn’t readily accept H+ ions. More reactant base molecules present in solution than product of OH- ions hence <–> eg ammonia sulphate ethanoate

strength of an acid/base relates to what proportion of its molecules will donate/accept a proton, H+ w/a acid/base concentration depends on how many of those acid/base molecules were in the solution to begin with

measure of the concentration of H3O+ ions in solution values of pH arranged on a logarithmic scale [OH-][H3O+] = 10^-14 M^2

a soluble base

(dilute a solution by factor of 10 to increase/decrease pH by 1) pH = -log [H3O+] pH = 14 + log [OH-]

[H3O+] = 10 ^-pH [OH-] = 10 ^pH-14 or C1V1 = C2V2

Kw = [H3O+] x [OH-] = 1 x 10^-14 constant value tf as [H3O+] increases, [OH-] must decrease to maintain constant and vice versa