Acids And Bases Flashcards
Brønsted-Lowry definition of acid
BrØnsted-Lowry definition of an acid is a species that donates a proton, H+, during an acid-base reaction.
BrØnsted-Lowry definition of a base
BrØnsted-Lowry definition of a base is a species that accepts a proton, H+, during an acid-base reaction.
Define Alkali
An alkali is a soluble base that dissociates hydroxide ions.
Common bases
Sodium Hydroxide NaOH Ammonia NH3 Magnesium hydroxide Mg(OH)2 Potassium Hydroxide KOH Sodium Hydroxide NaOH Oxide O2- Calcium Hydroxide Ca(OH)2
Common acids
Hydrochloric acid HCl Sulfuric acid H2SO4 Nitric acid HNO3 Phosphoric acid H3PO4 Ethanoic acid CH3COOH Carbonic acid H2CO3 Ammonium NH4+
Define Amphiprotic species
When acid-base reactions happen between an acid or base and water then either a hydronium or hydroxide ion is produced.
Eg: H2O can become H30+ or OH-
Ion equation
Ionic equations are simplified equations not including spectator ions.
Spectator ions are aqueous ions which do not react and remain dissolved in solution throughout a reaction
Strong acids
A strong acid is one that will undergo almost complete ionisation when added to water.
Almost all acid molecules in solution will donate proton to form aqueous H+ ions.
eg: H2SO4, HCl, HNO3
Weak acids
A weak acid does not readily give up its H+ ion in solution or does not completely ionise.
Must use double arrow
eg NH4+, CH3COOH
Strong base
A strong base readily accepts a proton, H+ during an acid-base reaction.
A strong base is one that readily dissociates to form OH- ions and a basic solution.
Eg: O2-, OH-, S2-
Weak bases
A weak base does not readily accept a H+ ions + small portion of a weak base will accept the proton so small portion of OH- ions
NH3, SO4^2-, F-
Describe Strength
Strength of an acid relates to what proportion of its molecules will donate a proton, H+
Describe Concentration
An acids concentration depends on how many of those acid molecules were in the solution to begin with, that is, how many acid molecules there are per volume
Sections of pH scale
The stronger the acid the lower the pH value.
Neutral solutions have a pH of 7.
The stronger the base the higher the pH value.
Ionic product of water (Kw)
Kw = [H3O+] x [OH-] = 1.00 x 10^-14
