AS Revision Lessons Identification tests.

Name: AS Revision Lessons Identification tests.
Uploaded: 2017-08-02T11:01:23+00:00
Duration: PTM12S20
Channel: Barnaby Blankenship
Description: AS Revision Lessons Identification tests.

AS Revision Lessons Identification tests

Which ion gives a lilac flame test?
sodium potassium calcium carbonate

Which ion gives a white precipitate when added to aqueous barium chloride and hydrochloric acid?
sulfate chloride aluminium hydroxide

sulfide ammonia sulfate ammonium
Which ion, when added to a warm solution of sodium hydroxide, will produce a gas that will turn damp indicator paper blue? sulfide ammonia sulfate ammonium

hydrogen chloride sulfur dioxide carbon dioxide oxygen
Which gas will turn damp indicator paper red and, when dissolved in water, will produce a white precipitate with silver nitrate solution hydrogen chloride sulfur dioxide carbon dioxide oxygen

Aluminium chloride Calcium sulfate Aluminium sulfate
A colourless solution reacts with a few drops of dilute sodium hydroxide solution to make a white precipitate. If the original solution is added to acidified barium chloride solution a different white precipitate forms. The solid will give a brick red flame test. The solution could be: Aluminium chloride Calcium sulfate Aluminium sulfate Copper (II) chloride

Copper (II) iodide Sodium chloride Calcium bromide Iron (III) sulfate
A white solid gives a brick red flame colour. When it is dissolved in water a colourless solution forms. If a mixture of silver nitrate and nitric acid are added to the solution a cream precipitate, that is soluble in concentrated ammonia, forms. The compound might be: Copper (II) iodide Sodium chloride Calcium bromide Iron (III) sulfate

A white solid gives a yellow flame colour & dissolves in water
A white solid gives a yellow flame colour & dissolves in water. The solution reacts with barium chloride to give a thick white precipitate. If dilute nitric acid is added to the precipitate most of it dissolves and a choking gas is produced. The solid might be: Sodium sulphate Potassium nitrate Sodium carbonate Sodium sulphite

Sodium Magnesium Calcium Ammonium
A solid chloride is white. It gives no flame colour. When dissolved in water it will produce a white precipitate on addition of sodium hydroxide or ammonia solution. The cation might be: Sodium Magnesium Calcium Ammonium

Chlorine Bromine Nitrogen dioxide Sulfur dioxide
A pale green gas turns universal indicator red and then bleaches it. The gas might be: Chlorine Bromine Nitrogen dioxide Sulfur dioxide

Sodium hydrogen carbonate
A white solid dissolves in water. The pH of the solution is found to be 8. The solution is boiled vigourously for 5 minutes and the pH is found to be 13. A flame test performed on the solid produces a yellow colour but when viewed through blue glass lilac can be seen. The solid could be: Sodium carbonate Potassium carbonate Sodium hydrogen carbonate Potassium hydrogen carbonate

Tests for cations Hydrogen ions (H+) Solution acidic, tests:Indicator paper, e.g., universal indicator or litmus Indicator solution, e.g., universal indicator, methyl red Reacts with reactive metal (e.g. magnesium) to produce hydrogen gas (H2) Reacts with metal carbonates to give carbon dioxide gas Lithium (Li+) Scarlet flame test. Produces white precipitate with NaOH Sodium ions (Na+) Orangey yellow flame test Potassium ion (K+) Lilac flame test Magnesium ion (Mg2+) Produces white precipitate with NaOH or NH3 solution Calcium ion (Ca2+) Brick red flame test. Produces white precipitate with NaOH Strontium ion (Sr2+) Scarlet flame test. Produces white precipitate with NaOH Barium ion (Ba2+) Apple green flame test. Produces white precipitate with NaOH Ammonium ion (NH4+) When mixed with sodium hydroxide and heated gently it produces an alkaline gas (fumes turn universal indicator paper blue)

Tests for anions Hydroxide ion (OH-) Alkaline solution tests. When mixed with an ammonium salt and heated gently it produces an alkaline gas (fumes turn universal indicator paper blue) Sulphate ion (SO42-) Add hydrochloric acid followed by barium chloride solution Produces a thick white precipitate of barium sulphate. Sulphite ion (SO32-) Produces SO2 (g) with dilute acid. Add barium chloride solution. Produces a thick white precipitate of barium sulphite, that dissolves on addition of acid (some sulphate impurities will remain) Halide ion (X-) Add nitric acid followed by silver nitrate. Chloride (Cl-) Produces a white precipitate of AgCl, that turns purple-gray in sunlight and is soluble in dilute ammonia, with Cl-. Bromide (Br-) Produces a pale yellow/cream precipitate of AgBr, that is soluble in concentrated ammonia, with Br-. Iodide (I-) Produces a yellow precipitate of AgI

Further tests for anions
Carbonate ion (CO32-) Produces carbon dioxide on addition of a dilute acid Solution pH = 12-14, remains constant if boiled. Produces immediate white precipitate with cold Ca2+ or Mg2+ salt. Hydrogen carbonate (HCO3-) Produces carbon dioxide on addition of a dilute acid Solution pH = 7-8, rising to with CO2 production if boiled. Produces white precipitate with Ca2+ or Mg2+ salt only if boiled. Nitrate (NO3-) Heat with sodium hydroxide (to remove ammonium) add aluminium to produce NH3 (g). Addition of FeSO4 (aq) to solution of nitrate followed by a few drops of concentrated sulphuric acid will produce a brown ring.

Tests for gases Oxygen (O2) Relights glowing splint
Hydrogen (H2) Lit splint produces a ‘squeaky’ pop Carbon dioxide (CO2) Turns lime water cloudy (also, will extinguish a lit splint, but this is not a positive test) Ammonia (NH3) Turns moist universal indicator paper blue Chlorine (Cl2) Bleaches indicator paper Sulphur dioxide (SO2) Pass through acidified potassium manganate (VII), produces colour change (purple  brown) Nitrogen dioxide (NO2) Brown, choking & acidic. Pass through acidified potassium manganate (VII), produces colour change (purple  brown)