CBMS107 Lecture 7: Acid and Bases
3 Aug 2018
School
Department
Course
Professor
Document Summary
21st march 2018: lecture 11 and 12 acids and bases: Hydrogen ion, h+ = proton because the h+ cation is a proton with no surrounding valence electrons. Brackets [ ] indicate the concentration of a species. Can be characterised as either strong or weak acids/bases: arrhenius model: Acids/bases are substances that can/cannot dissociate in water: measure of strength: A substance that dissociates into ions when it is in a solution = electrolyte: equilibrium: Dynamic equilibrium: reversible (forward and reverse reaction can occur) If a system at equilibrium is disturbed (e. g. conc. Of a species changes), then the system reacts to counteract the disturbance (cid:523)le chatelier(cid:495)s principles(cid:524) The change in reactant and product concentrations is constant. The relationship between reactant and product concentration at equilibrium can be expressed by using an equilibrium constant expression keq: bronsted-lowry model: Ab reactions involve the transfer of h+ between substances. Acid = donates h+ to another substance.
