Ions in aqueous solution
No description yet. This curated deck is ready for daily study.
Card preview (12)
State the colour of Fe2+ in aqueous solution
Green
State the colour of Cu2+ in aqueous solution
Blue
State the colour of Fe3+ in aqueous solution
Purple Appears yellow due to [Fe(H2O)5(OH)]2+
State the colour of Al3+ in aqueous solution
Colourless
Describe why some aqueous compound ions are acidic e.g. [Fe(H2O)6]3+
Fe3+ ion strongly polarising Weakens O-H bonds in water ligands Releases H+ ion, producing an acidic solution
Give the equation for an M 3+ ion being acidic
[M(H2O)6]3+ + H2O -> [M(H2O)5(OH)]2+ + H3O+
Describe why a solution of [M(H2O)6]3+ is much more acidic than a solution of [M(H2O)6]2+
M 3+ has a higher charge density than M 2+ M 3+ causes more O-H bonds to break so more H+ ions are produced The concentration of H+ ions is higher so the solution is more acidic
State how [M(H2O)6]3+ can form a precipitate in aqueous solution
[M(H2O)5(OH)]2+ + H2O -> [M(H2O)4(OH)2]+ + H3O+ [M(H2O)4(OH)2]+ + H2O -> M(H2O)3(OH)3 + H3O+ Uncharged complex is not soluble so a precipitate forms
Give the equations for a 2+ metal aqua ion reacting with a base to form a precipitate
[M(H2O)6]2+ + OH- -> [M(H2O)5(OH)]+ + H2O [M(H2O)5(OH)]+ + OH- -> M(H2O)4(OH)2 + H2O Can swap OH- for NH3 and form NH4+
Give the equations for a 3+ metal aqua ion reacting with a base to form a precipitate
[M(H2O)6]3+ + OH- -> [M(H2O)5(OH)]2+ + H2O [M(H2O)5(OH)]2+ + OH- -> [M(H2O)4(OH)2]+ + H2O [M(H2O)4(OH)2]+ + OH- -> M(H2O)3(OH)3 + H2O Can swap OH- for NH3 and form NH4+
Give the equations for a 2+ metal aqua ion reacting with a carbonate ion
[M(H2O)6]2+ + CO3 2- -> MCO3 + 6H2O
Give the equations for a 3+ metal aqua ion reacting with a carbonate ion
2[M(H2O)6]3+ + 3CO3 2- -> M(H2O)3(OH)3 + 3CO2 + 3H2O