REFER TEXT BOOK : PAGE 138

EXAMPLE : Metal ions Ammonium ion replace Ammonium chloride Sodium chloride

SALTS CONSIST ANION PART COMES FROM THE ACID WHILE CATION PART COMES FROM BASES Common cations Common anions (parent acids) Na + K+K+K+K+ K+K+K+K+ NH 4 + Ca 2+ Mg 2+ Al 3+ Zn 2+ Pb 2+

Metal ion Sulphate salts + H 2 SO 4 Chloride salts + HCl Carbonate salts + H 2 CO 3 Nitrate salts + H 2 NO 3 Na + Na 2 SO 4 NaClNa 2 CO 3 NaNO 3 Mg 2+ MgSO 4 MgCl 2 MgCO 3 Mg(NO 3 ) 2 Cu 2+ CuSO 4 CuCl 2 CuCO 3 Cu(NO 3 ) 2 Al 3+ Al 2 (SO 4 ) 3 AlCl 3 Al 2 (CO 3 ) 3 Al(NO 3 ) 3

All nitrate salts ; soluble salts Barium nitrate, Ba(NO 3 ) 2 Calcium nitrate, Ca(NO 3 ) 2 Aluminium nitrate, Al(NO 3 ) 3 Silver nitrate, AgNO 3 Lead(II) nitrate, Pb(NO 3 ) 2 Potassium nitrate, KNO 3 Sodium nitrate, NaNO 3 Copper(II) nitrate, Cu(NO 3 ) 2 Iron(III) nitrate, Fe(NO 3 ) 3 NO 3 -

Potassium carbonate, K 2 CO 3 Sodium carbonate, Na 2 CO 3 Ammonium carbonate, (NH 4 ) 2 CO 3 Potassium sulphate, K 2 SO 4 Potassium chloride, KCl Potassium nitrate, KNO 3 Sodium nitrate, NaNO 3 Sodium chloride, NaCl Ammonium sulphate, (NH 4 ) 2 SO 4

All carbonate salts ; insoluble salts Magnesium carbonate MgCO 3 Calcium carbonate CaCO 3 Silver carbonate Ag 2 CO 3 Other names[hide] Silver(I)Carbonate Copper(II) carbonate CuCO 3 Zinc carbonate ZnCO 3 Manganese(II) carbonate MnCO 3 Potassium carbonate K 2 CO 3 Sodium Carbonate Na 2 CO 3 Ammonium carbonate (NH 4 ) 2 CO 3 CO 3 2-

Mercury(II) Chloride HgCl 2 All SO 4 2-, Cl - salts ; soluble salts Silver(I) Chloride AgCl Lead(II) Chloride PbCl 2 Cl - Barium sulphate BaSO 4 Lead(II) sulphate PbSO 4 Calcium(II) sulphate CaSO 4 SO 4 2-

Copper(II) Chloride CuCl 2 Iron(II) Chloride FeCl 2 Magnesium Chloride MgCl 2 Copper(II) sulphate CuSO 4 Aluminium(II) sulphate Al 2 (SO 4 ) 3 Zinc Chloride ZnCl 2 Potassium chloride, KCl Sodium chloride, NaCl

NO 3 - PbSO 4 CaSO 4 BaSO 4 PbCl 2 AgCl CO 3 2- SO 4 2- Cl -

[ SODIUM SALTS / POTASSIUM SALTS / AMMONIUM SALTS ] PREPARATION OF POTASSIUM CHLORIDE EXAMPLE K K OH H H Cl K K

APPARATUS APPARATUS : Pipette 25mL, Burette 50mL, Conical Flask 250 mL MATERIALS MATERIALS : Potassium hydroxide 1.0 M, Hydrochloric acid 1.0 M, Phenolphthalein APPARATUS APPARATUS : Pipette 25mL, Burette 50mL, Conical Flask 250 mL MATERIALS MATERIALS : Potassium hydroxide 1.0 M, Hydrochloric acid 1.0 M, Phenolphthalein Colourless KOH turn to pink. Fill a burette with hydrochloric acid and record the initial burette reading. Record the burette reading in 2d.p Slowly adding the acid into the conical flask and swirls- until the indicator turns from pink to colourless. Record the volume of acid used. (V cm 3 ) Record the final burette reading in 2d.p

Pipette 25.0 cm 3 of the same potassium hydroxide solution into a conical flask. Do not add any indicator. Pipette 25.0 cm 3 of the same potassium hydroxide solution into a conical flask. Do not add any indicator. From the burette, add exactly V cm 3 of hydrochloric acid to the alkali and swirls and shake well. START OVER AGAIN BUT WITHOUT INDICATOR : To get the pure and neutral salt solution START OVER AGAIN BUT WITHOUT INDICATOR : To get the pure and neutral salt solution HEATING/EVAPORATE COOLING FILTRATION DRY Solution salt contains impurities continuous with recrystallisation process

[ OTHER SALTS EXCEPT Na +, K +, NH 4 + ] Pour 50 cm 3 of sulphuric acid into a beaker. Warm the acid Use a spatula to add copper(II) oxide powder bit by bit into the acid. Stir the mixture well. Continue adding copper(II) oxide until some of it no longer dissolves(excess unreacted metal Pour 50 cm 3 of sulphuric acid into a beaker. Warm the acid Use a spatula to add copper(II) oxide powder bit by bit into the acid. Stir the mixture well. Continue adding copper(II) oxide until some of it no longer dissolves(excess unreacted metal See the change of metal solid colour and dissolve Solution salt contains impurities continuous with recrystallisation process Glass rod Acid Metal/ metal oxide/ metal carbonate Excess unreacted metal (residue) Evaporating basin with salt solution (filtrate)

HEATING/EVAPORATE COOLING Evaporating basin Salt solution

FILTRATION DRY The crystals are filtered and rinsed with a little cold distilled water. Rinse with distilled water Glass rod Salt Cystals Filter Paper These physical characteristics : Regulars geometry shapes, such as cubic or hexagonal. Flat faces, straight edges and sharp angles. Same angle between adjacent faces.

DISSOLVE SOLUTE IN ACID HEATING DISSOLVE METAL IN ACID HEATING DISSOLVE METAL IN ACID EXCESS METAL NOT DISSOLVE COMPLETE REACT EXCESS METAL NOT DISSOLVE COMPLETE REACT NEUTRALISATION REACTION 1 ST TITRATION WITH INDICATOR FIND VOLUME OF ACID 1 ST TITRATION WITH INDICATOR FIND VOLUME OF ACID 2 ND TITRATION NO INDICATOR GET PURE SALT 2 ND TITRATION NO INDICATOR GET PURE SALT PREPARATION OF SOLUBLE SALTS TRANSFER TO EVAPORATING BASIN HEATING/EVAPORATEHEATING/EVAPORATE COOLING FILTRATION DRY

[ ALL CARBONATE SALTS except Na + /K + /NH 4 + ] PbSO 4 / CaSO 4 / BaSO 4 /PbCl 2 / AgCl ] [ ALL CARBONATE SALTS except Na + /K + /NH 4 + ] PbSO 4 / CaSO 4 / BaSO 4 /PbCl 2 / AgCl ] PREPARATION OF LEAD(II) CHLORIDEEXAMPLE Na Cl Pb NO 3 Na DOUBLE DECOMPOSITION METHOD DOUBLE DECOMPOSITION METHOD – TWO AQUOUES SOLUTIONS/SOLUBLE SALTS WERE MIX TOGETHER INTERCHANGE TO PRODUCE TWO NEW COMPOUND WHICH IS INSOLUBLE SALT OR PRECIPITATE, AND AQUEOUS SOLUTION/SOLUBLE SALTS Cl 2 Pb

the ions of the two aqueous solutions above interchange to produce two new compound which is insoluble salt or precipitate, and aqueous solution [one of the solutions contains the anions of the insoluble salt] two aquoues solutions/soluble salts were mix together [one of the solutions contains the cations of the insoluble salt]

Mixture solutions Filter paper Retort stand Precipitate (residue) Filter funnel Aqueous Solution (filterate) Glass rod Filtration : Remove solution from precipitate Glas s rod Distilled water Precipitate (residue) Rinse : remove other ions from precipitate

Filter paper Precipitate /Soluble salts Dry : Dry : Dried by pressing between two pieces of filter paper. FLOW CHART : PREPARATION OF INSOLUBLE SALTS MIX - STIR TWO SOLUBLE SALTS MIX - STIR TWO SOLUBLE SALTS FILTRATION REMOVE FILTRATE FILTRATION REMOVE FILTRATE RINSE REMOVE OTHER IONS RINSE REMOVE OTHER IONS DRY PRESS BETWEEN FILTER PAPER DRY PRESS BETWEEN FILTER PAPER

PREPARATION OF SALTS REMEMBER : METAL ION DISPLACE HYDROGEN ION IN ACID TO FORMED SALTS HCl [H + /Cl - ] Hydrochloric acid HCl [H + /Cl - ] Hydrochloric acid HNO 3 [H + /NO 3 - ] Nitric Acid HNO 3 [H + /NO 3 - ] Nitric Acid H 2 SO 4 [2H + /SO 4 2- ] Nitric Acid H 2 SO 4 [2H + /SO 4 2- ] Nitric Acid H 2 CO 3 [2H + /CO 3 2- ] Nitric Acid H 2 CO 3 [2H + /CO 3 2- ] Nitric Acid Na + K+K+K+K+ K+K+K+K+ NH 4 + Ca 2+ Mg 2+ Cu 2+ Fe 2+ Fe 3+ Al 3+ Zn 2+ Pb 2+

Method/ReactionReason Type of Salts (Metal) Neutralisation (Titration method) Alkali + Acid  Salts + Water Most salts of sodium, potassium, and ammonium ions are soluble. Na + K + NH 4 + Metal Displacement Metal + Acid  Salts + Hydrogen More electropositive metal can be displaced hydrogen ion from acid. Ca 2+ Mg 2+ Al 3+ Zn 2+ Metal oxide + Acid  Salts + Hydrogen Less electropositive metal not be displaced hydrogen ion from acid. Mostly Cu 2+ /Pb 2+ /Ag + Metal carbonate + Acid  Salts + Water + Carbon dioxide metal carbonate is a solid that cannot dissolves in water, in reaction that solid must be added excessively All above except Na + /K + /NH 4 +

Reactive metal is magnesium, aluminium, and zinc. Unreactive metal is iron, lead, silver Metal that is less reactive from hydrogen such as copper, lead and silver did not react with dilute acid. Soluble salts of sodium, potassium and ammonium can be prepared by the reaction between an acid and alkali.

Metal, metal oxide and metal carbonate is a solid that cannot dissolves in water, hence during reaction that solid must be added excessively to make sure all hydrogen ions in acid is completely reacted. Excess solid can be expelling through filtration. Unreactive metal such as lead (Pb), copper (Cu), and silver (Ag) cannot react with dilute acid. So to prepare salt contains lead ions (Pb 2+ ), copper ions (Cu 2+ ) or silver ions (Ag + ), we must use either oxide powder or carbonate powder only. Impure soluble salt can be purified through crystallization process

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