4.1 acids and bases

define alkali

aqueous solutions of bases

describe the properties of acids

turn litmus indicator red, corrosive, sour, low pH, conducts electricity

describe the properties f bases

turn litmus indicator blue, caustic and slippery, bitter, high pH, conduct electricity

summarise the bronsted Lowry theory of acids and bases

acids are proton donors, bases are proton acceptors and acid base rxns involve the exchange of protons from an acid to a base.

define hydrolysis reaction

a reaction that occurs when a molecule or ion in an aq solution, reacts with water & either accepting or donating a proton.

what is one advantage and one disadvantage of the bronsted lowry theory

adv: not restricted to only aqueous solns
disadvantage: cannot be applied to the reaction between acidic and basic oxides

define conjugate acid

when a base in a rxn contains one more hydrogen ion. e.g HCl is the conjugate acid of Cl-

define conjugate base

when an acid in a run has one less hydrogen ion. e.g Cl- is the conjugate base of HCl

define conjugate acid-base pair

an acid and its conjugate base/ vice versa.

define amphiprotic substances

substance that can donate and accept protons. e.g h20

examples of monoprotic acids:

hcl, ch3cooh, hf, hno3

examples of diprotic acids

h2so4, h2co3

examples of triprotic acids

h3po4, h3bo3