It is important to be able to test for certain chemical groups in a compound. One of those important groups are ions.
Ions are charged particles Cations are positive (in the words of JD paws-ative) anions are negative (A N-egative- Ion).
Chemical tests are simply reactions whose products give visual clues as to the reactants. for example if universal indicator is turned red it means there is an H+ ion in the substance being tested or if a gas turns limewater milky then a calcium carbonate precipitate has been produced we use this reaction to show that the gas was carbon dioxide.
the tests that you should know are…
Tests for cations
Hydrogen ion H+*
add universal indicator
indicator turns red if hydrogen is present
or
add calcium carbonate
carbon dioxide is given off if hydrogen is present
or
any other typical reaction of an acid
H+ is effectively an acid and so you can expect it to produce Hydrogen in a reaction with a metal, a salt with an alkali, carbon dioxide with a carbonateFor Hydrogen gas see the common tests page
Copper (commonly Cu2+)*
Add drop of ammonium hydroxide
light blue ppt formsExcess ammonium hydroxide
deep blue solution forms (this takes a large quantity of water to dilute down)
Iron (II)*
Add aqueous sodium hydroxide
Green ppt forms
Iron (III)*
Add drop aqueous sodium hydroxide
Brown ppt forms
Zinc (II)*
Add aqueous sodium hydroxide
White ppt formsExcess sodium hydroxide
White ppt re-dissolve
or
Add drop of ammonium hydroxide
White ppt formsExcess ammonium hydroxide
White ppt re-dissolve
Ammonium (NH4+)*
Add 5cm3 of sodium hydroxide and warm
Ammonia detected
Aluminium (commonly 3+)
Add aqueous sodium hydroxide
White ppt formsExcess sodium hydroxide
White ppt re-dissolve
Calcium (Ca2+)
Add aqueous sodium hydroxide
Fine white ppt formsExcess sodium hydroxide
White ppt does not re-dissolve
Tests for anions
Hydroxide OH–*
Add universal indicator
Indicator turns blue
or
Add ammonium compound and warm
Ammonia detected
Carbonate CO32-*
Add a little dilute acid
Carbon dioxide given off (see common molecules page)
Sulfate SO42-*
Add dilute hydrochloric acid then a few drops of aqueous barium chloride
White precipitate formed
Sulfite SO32-
Add a little dilute hydrochloric acid, warm
Sulfur dioxide detected (see the common molecules tests page)
Nitrate*
Add sodium hydroxide and add aluminium foil
Warm Carefully
Ammonia detected
Chloride Cl–*
Add dilute nitric acid then a few drops of silver nitrate
White precipitate forms
Will dissolve in dilute ammonia
Bromide Br–
Add dilute nitric acid then a few drops of silver nitrate
Cream precipitate forms
Will only dissolve in conc ammonia
Iodide I–
Add dilute nitric acid then a few drops of silver nitrate
Yellow precipitate forms
Will not dissolve in ammonia
* denotes that these are CIE GCSE tests for ions