notes updates salts

SALTSWhat is salt?

In the preparation of salts, we must identify the type of salt. This can be done by analysing the cations and the anions that are present in salts.

Two types of salts Soluble salt – salts that can be dissolve in water at room temperature

Insoluble salt – salts cannot be dissolve in water at room temperature

Type of salt Solubility in water

Sodium saltsPotassium salts Ammonium salts

All dissolves in water

Nitrate salts All dissolves in water

Chloride saltsAll dissolves in water, Except: Lead(II) chloride, PbCl2

Silver chloride, AgCl Mercury chloride, HgCl

Sulphate saltsAll dissolves in water Except: Lead(II) sulphate, PbSO4

Barium sulfat, BaSO4

Calcium sulfat, CaSO4

Carbonate saltsAll did not dissolves in water, Except: Sodium carbonate, Na2CO3 Potassium carbonate, K2CO3

Ammonium carbonate, (NH4)2CO3

Special Properties of lead(II) chloride and lead(II) iodide NOTES: Lead halide such as lead(II) chloride (PbCl2), lead(II) bromide (PbBr2), and lead(II) iodide (PbI2) did not dissolve in cold water but dissolve in hot water.

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White precipitate of PbCl2

White precipitate dissolves in hot water

White precipitate formed when the water is cooled down.

Salt is an ionic compound formed when the hydrogen ion, H+ from acid is replaced by a metal ion or ammonium ion, NH4

+

PbCl2 are soluble in hot water.

Use of salts;

Item Use Example

Food preparation

FlavorMonosodium glutamate (MSG)Sodium chloride

PreservativesSodium chloride - salted fishSodium benzoate - sauceSodium nitrite - processed meat, burger

Baking powder Sodium hydrogen carbonateAgriculture

Nitrogen fertilizersPotassium nitrateSodium nitrate

PesticideCopper(II) sulphateIron(II) sulphate

Medicine

Reduce stomach acidic (gastric)

Calcium carbonateCalcium hydrogen carbonate

Sniff salt (fainted) Ammonium carbonatePlaster of Paris (cement to support broken bone)

Calcium sulphate

A. Preparation of SaltThe procedure of preparation salt depends to the type of salt.

a. Insoluble salt is prepared through precipitation reaction.

b. Soluble salt is prepared by one of these reactions; i. Acid and alkali ii. Acid and metal oxide

iii. Acid and metal carbonateiv. Acid and reactive metal

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Yellow precipitate of PbI2

Yellow crystals formed when the water is cooled down.

Yellow precipitate dissolves in hot water

PbI2 are also soluble

in hot water.

a. Insoluble Saltsi. Preparing Insoluble Salts 1. Insoluble salts can be prepared through precipitation reactions or double decomposition reactions.2. Precipitation or double decomposition reaction involves;

- two aquoues solutions/soluble salts were mix together- one of the solutions contains the cations of the insoluble salt. - one of the solutions contains the anions of the insoluble salt.- the ions of the two aqueous solutions above interchange to produce two new compound which is insoluble salt or precipitate, and aqueous solution. - the precipitate produced is obtained by filtration. The residue left in the filter paper is the insoluble salt. The filtrate is soluble salt. - the residue/precipitate (insoluble salt) then rinsed with distilled water to remove any other ions as impurities.

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Na+ Na+

NO3-NO3

-

PbCl2

Pb2+ ions combined with Cl- ions to form white precipitate

Na+ ions and NO3- ions do not

take part in the reaction and are free to move in the solution

Ionic equation: Pb2+ + 2Cl- PbCl2

Anion(Non-metal ion)

Cation(Metal ion) nn mm

Chemical and ionic equations

Chemical equation : MX(aq) + NY(aq) → MY(s) + NX(aq) solution solution precipitate solution

Ionic equation : M+(aq) + Y-(aq) → MY(s)

Study this reaction carefullyIn the formation of the precipitate of barium sulphate, BaSO4, the chemical equation can be written:

BaCl2(aq) + Na2SO4 (aq) BaSO4(s) + 2NaCl (aq)

Ions Ba 2+ + Cl - + Na + + SO42- BaSO4 + Na + + Cl -

Ionic equation : Ba2+ + SO42- BaSO4

(shows the ions that take part in the reaction to form precipitate/insoluble salts)

More examples;Insoluble Salt Ions Ionic equation

ZnCO3 Zn2+ , CO32- Zn2+ + CO3

2- ZnCO3

AgCl Ag+ , Cl- Ag+ + Cl- AgCl

BaSO4 Ba2+ , SO42- Ba2+ + SO4

2 BaSO4

PbCl2 Pb2+ , Cl- Pb2+ + Cl- PbCl2

PbSO4 Pb2+ , SO42- Pb2+ + SO4

2- PbSO4

CaCO3 Ca2+ , CO32- Ca2+ + CO3

2- CaCO3

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Glass rod

Residue/precipitate (Insoluble salt)

Filtrate (Soluble salt)

Mixture of solutions

Filter funnel

Filter paper

Retort stand

ii. Preparation and purification of insoluble salts

Preparation of Plumbum(II) iodide

Chemical equation : Pb(NO3)2 (aq) + 2KI (aq) → PbI2 (s) + 2KNO3 (aq)

Ionic equation : Pb2+ (aq) + 2I- (aq) → PbI2 (s)

Step 1: Preparation

1. 20 cm3 lead(II) nitrate 0.1 mol dm-3 solution is measured with measuring cylinder 50 ml,and poured into a beaker.

2. 20 cm3 potassium iodide 0.1 mol dm-3 solution is measured with measuring cylinder 50 ml and poured into a beaker contains lead(II) nitrate solution.3. The mixture is stirred with a glass rod. A yellow precipitate is formed.

4. The mixture is filtered to obtain the yellow solids of lead(II) iodide as the residue.5

+ →

20 cm3

Lead(II) nitrat0.1 mol dm-3

20 cm3

potassium iodide0.1 mol dm-3

Glass rod

Precipitate of lead(II) iodide(yellow)

Sodium nitrate solution

Mixture of solutions

Filter funnel

Filter paper

Retort standBeaker

Step 2: Purification

5. The residue is rinsed with distilled water to remove other ions in it.

6. The yellow solid is dried by pressing between two pieces of filter paper.

EASY LAH !

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Glass rodDistilled water

Precipitate of lead(II) iodide

Precipitate of lead(II) iodide

Filter paper

b. Soluble Salti. Preparaing Soluble Salt

- Sodium salts

- Potassium salts Acid + alkali salts + water

- Ammonium salts

Soluble Salts

Acid + metal oxide salts + water

- Others salts Acid + reactive metal salts + hydrogen gas

Acid + metal carbonate salt + water + carbon dioxide

Notes: Reactive metal is magnesium, aluminium, and zinc Unreactive metal is iron, lead, silver

a. Sodium, potassium or ammonium salts prepared from acid and alkali reaction.

Salt Alkali Acid Chemical equation

NaCl NaOH HCl NaOH + HCl → NaCl + H2O

K2SO4 KOH H2SO4 2KOH + H2SO4 → K2SO4 + 2H2O

NH4NO3 NH3/NH4OH HNO3 NH3 + HNO3 → NH4NO3 + H2O

CH3COONa NaOH CH3COOH NaOH + CH3COOH → CH3COONa + H2O

Note: To prepare the above salts, titration technique is use.

b. Soluble salt (except sodium, potassium and ammonium salt) is prepared using these methods - Acid and metal - Acid and metal oxide - Acid and metal carbonate

Name of SaltAcid that must be

used

Substance that can be use to react with acid

Metal Metal oxide Metal carbonate

ZnCl2 HCl Zn ZnO ZnCO3

Mg(NO)3 HNO3 Mg MgO MgCO3

CuSO4 H2SO4 × CuO CuCO3

Pb(NO3)2 HNO3 × PbO PbCO3

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Write a chemical equation for each experiment above.

Remember this notes ok1. Metal that is less reactive from hydrogen such as copper, lead and silver/argentum did not react with dilute acid. 2. Metal, metal oxide and metal carbonate above 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. 3. Impure soluble salt can be purified through crystallization process.

ii. Preparation and purification of soluble salts

A. Preparing soluble salt through reaction between acid and alkali.

Preparation of Soluble Sodium, Potassium and ammonium Salts Soluble salts of sodium, potassium and ammonium can be prepared by the reaction between an

acid and alkali.

Acid (aq) + alkali (aq) Salt (aq) + Water (l)

Procedure : Using pipette, 25 cm3 of alkali solution is measured and transferred into a conical flask. Two drops of phenolphthalein are added to the alkali solution. Dilute acid is place in a burette. The initial reading is recorded. Acid is added slowly into the alkali solution while shaking the conical flaks, until the pink solution turn colourless. The final reading of the burette is recorded. The volume of acid added, V cm3 is calculated. The experiment is repeated by adding V cm3 of acid to 25 cm3 of alkali solution in a beaker without using phenolphthalein as an indicator. The mixture is transferred into a evaporating dish. The mixture is heated until saturated and the saturated solution is allowed to cool at room temperature. Salt crystals formed are filtered and rinsed with a little of cold distilled water. Salt crystals are dried by pressing it between filter papers (or in oven)

The reaction between acid and alkali is known as what process?Refer to acids and bases notes ok. Don’t worry I’ll help you.!Kita bukan along kita cuma nak tolong.

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Example: Preparing sodium chloride

Step 1: Preparation (Titration)

1. 25.0 cm3 sodium hydroxide solutions is pipette into conical flask. 2. Two drops of phenolphthalein indicator are added into conical flask. The colour of solution is

recorded.3. A 50 cm3 burette is filled with hydrochloric acid. The initial burette reading is recorded. 4. Hydrochloric acid is added gradually from a burette into conical flask and swirling the conical

flask. 5. Titration is stopped when phenolphthalein changes from pink to colourless. The final burette

reading is recorded. 6. The volume of hydrochloric acid used is calculated. 7. The experiment is repeated by adding hydrochloric acid (known volume) to 25.0 cm3 sodium

hydroxide in a beaker without using phenolphthalein.

Step 2: Preparation (Crystallization)

8. The mixture is transferred into a evaporating dish.

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Retortstand

Burette

Hydrochloric acid

Conical flask

25 cm3 NaOH + phenolphthalein indicator

Bunsen burner

Evaporating dishSalt solution

9. The colourless solution is slowly heated/evaporated until its saturated or to about one-third (1/3) of the original volume.

10. The saturated solution is then cooled to allow crystallization to occur.


10. The white crystals formed are then filtered, rinsed with a little distilled water and dried by pressing between filter paper.

Note: Phenolphthalein indicator is used at the beginning of the experiment to determine the volume of hydrochloric acid that is required to react completely with 25 cm3 of sodium hydroxide. However experiment is repeated without using phenolphthalein so that the salt prepared will not contaminated by the indicator.

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Glass rodDistilled water

Copper(II) sulphate

Filter funnel

B. Preparing soluble salt through reaction between acid i. Metal oxide. ii. Metal iii. Metal carbonate

Procedure To Prepare a Soluble Salt (not Na, K or NH4+)

50 cm3 of acid is measured using a measuring cylinder and poured into a beaker. The acid is heated slowly.

Using a spatula, metal / metal oxide / metal carbonate powder is added a little at a time while stirring the mixture with a glass rod.

The addition of the solid powder is stopped when some solids no longer dissolve anymore. (the solid is excess and all the acid is completely neutralised by the solid)

The mixture is filtered to remove the excess solid powder.

The filtrate is transferred to an evaporating dish. The filtrate is heated until saturated. (The filtrate is evaporated to about one-third (1/3) of the

original volume) The saturated solution is then allowed to cool to room temperature and the salt crystals are

formed. The crystals are filtered and rinsed with a little cold distilled water. Salt crystals are then dried by pressing it between filter papers.

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Heating

AcidPowderof :

Metal oxideMetal carbonateMetal

Excess of solid powder

Filtrate (Salt solution)

Heating

Saturated solution

Crystals

Filtrate

Example: Preparing copper(II) sulphate (Sulphuric acid and copper(II) oxide powder) Step 1: Preparation

1. 50 cm3 sulphuric acid 0.1 mol dm-3 is put in a beaker and is heated. 2. Using spatula copper(II) oxide powder is added a little at a time to the hot sulphuric acid while

stirring continuously with glass rod. 3. The addition of copper(II) oxide is stopped when solids powder remain undissolved.

4. The mixture is filtered to remove the excess copper(II) oxide.5. The filtrate is transferred to an evaporating dish.

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xxxxxxxxxxxxxxxx

Copper(II) oxide

Glass rod

Beaker

Wire gauze

50 cm3 sulphuric acid 0.1 mol dm-3

TripodBunsen burner

Spatula

Stir

Glass rod

Reactant mixture

Excess copper(II) oxide

Copper(II) sulphate solution

6. The filtrate is slowly heated/evaporated until its saturated, or to about one-third (1/3) of the original volume.

7. The saturated solution is then allowed to cool to room temperature.


8. The crystals are filtered and rinsed with a little cold distilled water.9. Salt crystals are then dried by pressing it between filter papers.

REMEMBER…. THIS NOTES OK

Unreactive metal such as lead (Pb), copper (Cu), and silver (Ag) cannot react with dilute asid. So to prepare salt contains lead ions (Pb2+), copper ions (Cu2+) or silver ions (Ag+), we must use either oxide powder or carbonate powder only.

Example: CuO + H2SO4 CuSO4 + H2O (ok)

CuCO3 + H2SO4 CuSO4 + H2O + CO2 (ok)

Cu + H2SO4 no reaction (not ok)

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Bunsen burner

Evaporating dish

××××××××××××Copper(II) sulphate solution

Glass rod

Distilled water

Copper(II) sulphate

B. Physical Characteristics of Crystals.

A salt is made up of positive and negative ions. When these ions are packed closely with a regular and repeated arrangement in an orderly manner, a solid with definite geometry known as crystal lattice is formed.

All crystals have these physical characteristics:a) Reqular geometry shapes, such as cubic or hexagonal.b) Flat faces, straight edges and sharp angles.c) Same angle between adjacent faces.d) All crystals of the same salt have the same shape although the sizes may be different.

Start to memorize the solubility of a salt in water OK.It will help you a lot to better understand this chapter.

KNOWLEDGE IS POWER

The solubility of a salt in water depends on the types of cations and anions present.

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What is Qualitative analysis?

In the qualitative analysis of salts, we need to identify the ions that are present in salts. This can be done by analysing their physical and chemical properties.

Observations on the physical properties of salts

1. Colour and solubility in water

Certain physical properties of salts such colour and solubitity in water are observed to help us infer certain cations and anions that are present in salts. The table shows the colour of salts in solid , in aqueous solution and the solubility of salts in water

Salt Colour in solidSolubility in water

Colour in Aqueous solution

1. Ammonium chloride NH4Cl white soluble colourless

2. Ammonium nitrateNH4(NO3)3 white soluble colourless

3. Calcium carbonate CaCO3 white insoluble -

4. Calcium nitrate Ca(NO3)2 white soluble colourless

5. Magnesium sulphate MgSO4 white soluble colourless

6. Magnesium carbonate MgCO3 white insoluble -

7. Zinc sulphate Zn SO4 white soluble colourless

8. Zinc nitrate Zn(NO3)2 white soluble colourless

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Salt Solubility in water

Sodium, potassium and ammonium salts (Na+, K+, NH4

+) All are soluble

Nitrate salt (NO3-) All are soluble

Chloride salt (Cl -) All chloride salts are soluble in water except

PbCl2, AgCl and HgCl2

Sulphate salt (SO42-)

All sulphate salts are soluble in water except

PbSO4, BaSO4 and CaSO4

Carbonate salt (CO32-)

All carbonate salts are insoluble except Na2CO3,

K2CO3 and (NH4)2CO3

Qualitative analysis is a chemical technique used to determine what substances are present in a mixture but not their quantities.

9. Lead(II) chloride , PbCl2 white insoluble -

10. Lead(II) sulphate , PbSO4 white insoluble -

11. Lead(II) carbonate , PbCO3 white insoluble -

12. Copper(II) chloride , CuCl2 Blue soluble Blue

13 Copper(II) sulphate , PbSO4 Blue soluble Blue

14. Copper(II) carbonate , PbCO3 Green insoluble -

15. Iron(II) sulphate , FeSO4 Green soluble Pale green

16. Iron(III) chloride , FeCl3 Brown / Yellow soluble Brown/Yellow/ Yellowish brown

17. Sodium nitrate , NaNO3 white soluble colourless

18, Sodium carbonate , Na2CO3 white soluble colourless

19. Potassium nitrate , KNO3 white soluble colourless

20. Potassium carbonate , K2CO3 white soluble colourless

The table shows the colour of different cations in the solid form or in aqueous solution

Observation Inference

Blue solution Ion copper (Cu2+ ) present

Pale green solution Ion Iron(II) Fe2+ present

Yellow/Yellowish-brown/brown solution

Ion Iron (III) Fe3+ present

Green solid Hydrated Fe 2+, CuCO3

Brown solid Hydrated Fe 3+ salt

White solidSalts of Na+ , K+ ,NH4

+, Mg 2+, Ca 2+ Al 3+ , Zn 2+, Pb 2+ (If the anions are colourless

Colourless solution Na+ , K+ ,NH4+, Mg 2+, Ca 2+ , Al 3+ , Zn 2+, Pb 2+

The table shows the solubility of different types of salts in water

Compounds Solubility in water

Sodium saltsPotassium saltsAmmonium salts

All are soluble

Nitrate saltsAll are soluble

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Chloride saltsAll are soluble except AgCl, HgCl and PbCl2 (soluble in hot water)

Sulphate saltsAll are soluble except BaSO4, PbSO4 and CaSO4

Carbonate salts All are insoluble except sodium carbonate, potassium carbonate and ammonium carbonate

2. Tests for gases

Gases are often produced from reactions carried out during laboratory tests on salts. By identifying the gases evolved,it is possible to infer the types of cations and anions that are present in a salt.

The table shows the test and the result of different gases

Gas Test Result

Oxygen gas, O2Test with a glowing wooden splinter

Wooden splinter is rekindled /lighted

Hydrogen gas , H2Test with a lighted wooden splinter

Gas explodes with a pop sound

Carbon dioxide gas , CO2Bubble the gas produced into lime water

Lime water turns milky

Ammonia gas, NH3Test with moist red litmus paper

Moist red litmus paper turns blue

Chlorine gas, Cl2Test with moist blue litmus paper

Moist blue litmus paper turns red and then turns white

Hydrogen chlorine gas , HClTest with a drop of concentrated ammonia NH3 solution

Dense white fumes

Sulphur dioxide gas , SO2

Bubble the gas produced into purple acidified potassium manganate (VII), KMnO4 solution

Purple acidified potassium manganate (VII),KMnO4 solution decolourises

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Nitrogen dioxide gas , NO2Test with moist blue litmus paper

moist blue litmus paper turns red

3. Action of heat on salts

Effect of heat on carbonate salts

Carbonaate saltColour of salt before heating

Colour of residueEffect on lime water

Hot cold

Copper (II) carbonate, CuCO3

Green powder Black powder Black powderThe gas liberated turns lime water milky/chalky

Zinc carbonate , ZnCO3

White solid Yelow solid White solidThe gas liberated turns lime water milky/chalky

Lead(II) carbonate, PbCO3

White solid Brown sold Yelow solidThe gas liberated turns lime water milky/chalky

Sodium carbonate, Na2CO3

White solid White solid White solid No change

Calcium carbonate, CaCO3

White solid White solid White solidThe gas liberated turns lime water milky/chalky

Potassium carbonate, K2CO3

White solid White solid White solid No change

Magnesium carbonate, MgCO3

White solid White solid White solidThe gas liberated turns lime water milky/chalky

Effect of heat on nitrate salts

Nitrate SaltColour of salt before heating

Colour of residue Test on gases liberated

Hot cold

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Copper (II) nitrate, Cu(NO3)2

Blue solidBlackpowder

Blackpowder

A brown gas that turns blue litmus paper red is liberated.The gas liberated also ignites a glowing splinter

Zinc nitrate, Zn(NO3)2

White solidYellowsolid

White solid

A browan gas that turns blue litmus paper red is liberated.The gas liberated also ignites a glowing splinter

Lead(II) nitrate, Pb(NO3)2

White solid Brown solidYellowsolid


Sodium nitrate, NaNO3

White solid White solid White solidA colourless gas that rekindles a glowing splinter is liberated

Calcium nitrate, Ca(NO3)2

White solid White solid White solid


Potassium nitrate, KNO3

White solid White solid White solidA colourless gas that rekindles a glowing splinter is liberated

Magnesium nitrate, Mg(NO3)2

White solid White solid White solid


Iron(II) nitrate, Fe(NO3)2

Pale Green solid

Pale Green solid

Pale Green solid


Iron(III) nitrate, Fe(NO3)3

Brown solidReddish-Brown solid

Reddish-Brown solid


The table shows the comparison of the effect of heat on carbonate and nitrate salts

Metal Effect of heat on carbonate salt Effect of heat on nitrate salt

PotassiumSodium

Are not decomposed by heat Decompose to nitrite salt and oxygen gas.

CalciumMagnesiumAluminiumZincIronTinLeadCopper

Decompose to metal oxide and carbon dioxide gas.

Decompose to metal oxide, nitrogen dioxide gas and oxygen gas.

MercurySilverGold

Decompose to metal, carbon dioxide gas and oxygen gas.

Decompose to metal , nitrogen dioxide gas and oxygen gas.

Most sulphate salts are not decomposed by heat. Only a few sulphate such as iron(II) sulphate,zinc sulphate and copper sulphate decompose to sulphur dioxide or sulphur trioxide gas when heated.

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All chloride salts are stable when heated except ammonium chloride. Ammonium chloride sublimes and decomposes to produce ammonia gas and hydrogen chloride gas.

The table shows the deduction of the types of ion present based on the gas produced

Type of gas produced Type of ion present(anion)

CO2 Carbonate ion (CO3 2- ) present except Na2CO3 and K2CO3

O2 Nitrate ion (NO3-) present

NO2 Nitrate ion (NO3-) present except NaNO3 and KNO3

SO2 Sulphate ion (SO4 2- ) present

NH3 Ammonim ion (NH4+) present

Tests for anions

Reagent / Condition Observation Anion Ionic Equation (if any)

2 cm3 the unknown solution + dilute hydrochloric acid / nitric acid / sulphuric acid pour into a test tube gas liberated is immediately bubbled through lime water.

Effervescence. Colourless gas turns lime water milky.

CO32- ion CO3

2- + 2H+ CO2 + H2O

2 cm3 of nitric acid + 2 cm3 of the unknown solution pour into a test tube + 2 cm3 silver nitrate solution

White precipitate is formed.

Cl- ion Ag+ + Cl- AgCl

2 cm3 of dilute hydrochloric acid / nitric acid + 2 cm3 of the unknown solution pour into a test tube + 2 cm3 of barium chloride / barium nitrate solution shake well

White precipitate is formed.

SO42- ion Ba2+ + SO4

2 - BaSO4

2 cm3 of the unknown solution pour into a test tube 2 cm3 of dilute sulphuric acid + 2 cm3 of iron(II) sulphate solution shake well. Then drop carefully and slowly a few drops of concentrated sulphuric acid along the side of a slanting test tube into the

Brown ring is formed at the boundary between the concentrated H2SO4 (top layer) and aqueous solution of the mixture (bottom

NO3- ion -

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mixture without shaking it.

layer)

Tests for cations

Confirmatory Test for Fe 2+ , Fe 3+ , Pb 2+ , NH 4+ Ions

Confirmatory Test for Fe 2+ Reagent Observation Conclusion

Potassium hexacyanoferrate(II) solution

Pale blue precipitate Fe2+ ion is present

Dark blue precipitate Fe3+ ion is presentPotassium hexacyanoferrate(III) solution

Dark blue precipitate Fe2+ ion is present

Greenish-brown solution Fe3+ ion is presentPotassium thiocyanate solution

Pale red colouration Fe2+ ion is present

Blood red colouration Fe3+ ion is present

Confirmatory Test for Pb2+

Method Observation Ionic Equation

Using aqueous solution of chloride - 2 cm3 of any solution of Cl- + 2 cm3 of any solution of Pb2+ dilute with 5 cm3 of distilled water heat until no further change occurs allow the content to cool to room temperature using running water from the tap

- A white precipitate is formed

When heated – dissolve in water to form colourless solution

When cooled – white precipitate reappear

Pb2+ + 2Cl- PbCl2

Using aqueous solution of iodide - 2 cm3 of any solution of I- + 2 cm3 of any solution of Pb2+ dilute with 5 cm3 of distilled water heat until no further change occurs allow the content to cool to room temperature using running water from

- A yellow precipitate is formed

When heated – dissolve in water to form colourless solution

Pb2+ + 2I- PbI2

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the tap When cooled – yellow precipitate reappear

Confirmatory Test for NH4+

Method Observation

2 cm3 of any solution of NH4+ + 2 cm3 of

NaOH / KOH / Ca(OH)2 heat put a piece of moist red litmus paper at the mouth of the test tube

- Moist red litmus paper turns blue

Reaction with Nessler’s Reagent 2 cm3 of any solution of NH4

+ + 2 cm3 of Nessler’s Reagent shake well

- A brown precipitate is formed

Reaction of Cations With NaOH

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Pb2+ Zn2+ Al3+ : White precipitate dissolves/larut in excess NaOH

Ca2+ Mg2+ : White precipitate insoluble/tidak larut in excess NaOH

Reaction of Cations With NH3

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Cations

+ NaOH (aq)

Precipitate producedNo precipitate

White precipitate Coloured precipitate

Green Blue Brown

Fe2+ Cu2+ Fe2+NH4

+ K+ Na+

Dissolve in excess NaOH (aq) to form colourless solution

Sodium hydroxide solution is poured slowly into 2 cm3 of the solution to be tested in a test tube, until in excess.

Insoluble in excess NaOH (aq)

NH3 gas produced

warm

Zn2+ Al3+Pb2+ Ca2+ Mg2+

Easylah

Zn2+ : White precipitate dissolves/larut in excess NH3

Pb2+ Al3+ Mg2+ : White precipitate insoluble/tidak larut in excess NH3

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Cations

Precipitate producedNo precipitate

White precipitate Coloured precipitate

Green Blue Brown

Fe2+ Cu2+ Fe2+NH4

+ K+ Na+

Aqueous ammonia solution is poured slowly into 2 cm3 of the solution to be tested in a test tube until in excess.

NH3 gas produced

warm

Zn2+ Al3+Pb2+

Ca2+

Mg2+

Easylah

+ NH3 (aq)

+ excess NH3 (aq)

Dark blue solution

Dissolve in excess NH3 (aq) to form colourless solution

Insoluble in excess NH3 (aq)

Zn2+ ion is the only cation that form white precipitate and dissolves in both excess NaOH and NH3 solutions.

Mg2+ ion is the only cation that form white precipitate and insoluble in both excess NaOH and NH3 solutions.

Ca2+ ion in the only cation that form white precipitate in NaOH solutions, but no precipitate in NH3 solution.

Fe2+ , Fe3+ and Cu2+ ions is easy to spot because the ions shows coloured precipitate.

Pb2+ ion and Al3+ ion form white precipitate and dissolves in excess NaOH

solution, but insoluble in excess NH3 solutions.

Example: lead(II) nitrate solution and aluminium nitrate solution

Sodium sulphate solution is added slowly into 2 cm3 of the solution to be tested in a test tube. If a white precipitate is formed, then then the solution tested is lead(II) nitrate. If no change occurs, then the solution tested is aluminium nitrate.

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Based from the observation, I can conclude that

How to differentiate between Pb2+ and Al3+?

A chemical tests can be carried out in the laboratory to differentiate between Pb2+ and Al3+. (Please refer to Confirmatory Test for Pb2+, in ealier notes).

Now let see some questions about salt. Try to solve it by yourself first and then compare with the answers provided.

Example 1:

Describe chemical tests that can be carried out in the laboratory to differentiate between

(a) lead(II) nitrate solution and aluminium nitrate solution

Sodium sulphate solution is added slowly into 2 cm3 of the solution to be tested in a test tube. If a white precipitate is formed, then then the solution tested is lead(II) nitrate. If no change occurs, then the solution tested is aluminium nitrate.

(b) aluminium nitrate solution and zinc nitrate solution

Aqueous ammonia solution is poured slowly into 2 cm3 of the solution to be tested in a test tube until in excess. If a white precipitate that dissolves in excess aqueous ammonia solution is formed, than the solution tested is zinc nitrate. If a white precipitate that is insoluble in excess aqueous ammonia solution is formed, than the solution tested is aluminium nitrate.

(c) ammonium chloride solution and potassium chloride solution

Nessler’s Reagent is added to 2 cm3 of the solution to be tested in a test tube. If a brown precipitate is formed, then the solution tested is ammonium chloride.If no change occurs, then the solution tested is potassium chloride

(d) iron(II) sulphate solution and iron(III) sulphate solution

Potassium hexacyanoferrate(II) solution is poured into 2 cm3 of the solution to be tested in a test tube.If a dark blue precipitate is formed, then the solution tested is iron(III) chloride.

If no change occurs, then the solution tested is iron(II) chloride.

Or

Potassium hexacyanoferrate(III) solution is poured into 2 cm3 of the solution to be tested in a test tube.If a greenish-brown solution is formed, then the solution tested is iron(III) chloride.


Or

Potassium thiocyanate solution is poured into 2 cm3 of the solution to be tested in a test tube.If a blood red colouration is formed, then the solution tested is iron(III) chloride.

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(e) sodium chloride and sodium sulphate

Silver nitrate solution is poured into 2 cm3 of the solution to be tested in a test tube.If a white precipitate is formed, then the solution tested is sodium chloride.If no change occurs, then the solution tested is sodium sulphate.

Or

Barium chloride solution is poured into 2 cm3 of the solution to be tested in a test tube.If a white precipitate is formed, then the solution tested is sodium sulphate.If no change occurs, then the solution tested is sodium chloride.

Example 2:

1. State three examples ofa) soluble salts b) insoluble salts

Potassium carbonate Magnesium carbonate Lead(II) nitrate Lead(II) sulphate Ammonium chloride Argentum chloride

2. Which of the following salts is soluble

3. Identify the gas that turns moist red litmus paper blue

Ammonia gas

4. Gas X has the following properties

Gas X is carbon dioxide gas

5. Heat +

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Lead(II) chloride Sodium carbonate

Calcium sulphate Barium sulphate

Colourless Acidic gas Turns lime water milky

Salt P Metal oxide X Gas Y

Colour of metal oxide X is yellow when hot and white when cold. Gas Y turns lime water milky.

a) Name gas Y : carbon dioxide gas

b) Name metal oxide X : zinc oxide

c) Name salt P : zinc carbonate

d) Write an equation to represent the action of heat on salt P

ZnCO3 (s) ZnO (s) + CO2 (g)

6. A sample of copper(II) nitrate, Cu(NO3)2 was heated strongly. Write down the expected observation.

Copper(II) nitrate decompose to produce black colour of residue when hot and cold. A brown gas that changed moist blue litmus paper to red and colourless gas that lighted up a glowing wooden splinter are produced.

D. Numerical problem involving stoichiometric reaction in the

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preparation of salt

Example 1;

Ammonium phosphate, (NH4)3PO4 is use as a fertilizer. 29.8g of this salt is prepared by neutralizing phosphoric acid, H3PO4 with ammonium gas, NH3. Calculate the volume of ammonium gas, NH3

reacted at room conditions.( Relative atomic mass; H, 1: N, 14: P, 31; O, 16; Molar volume; 24 dm3 mol-1 at room conditions)

Solutions;

a. Calculate the number of moles

2.88 g

[3(14) + 12(1) + 31 + 4(16)

= 0.2 mol

b. Write a balanced chemical equation Compare the mole ratio of NH3 and (NH4)3PO4

H3PO4(aq) + 3NH3(aq) (NH4)3PO4(aq)

c. Calculate the number of moles of NH3 base on the mole ratio

= 3 X 0.2 mol

= 0.6 mol

d. Calculate the volume of NH3

Volume = number of mole X volume

= 0.6 mol X 24 dm3 mol -1

= 14.4 dm3

Example 2:3.9 g of potassium is burnt completely in the air as shown in the following equation;

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A balanced chemical equation for a reaction in preparation of a salt can be used to calculate the stoichiometric quantities of the followingMasses of reactantsVolumes and concentrations of reactantsMasses of productsVolumes of products

=

3 mol 1 mol

4K(s) + O2(g) → 2K2O(s)What is the mass of potassium oxide produced?[Relative atomic mass: K, 39; O, 16]

SolutionsTip: Solve the question step by step

Step 1: Write Chemical Equation

4K(s) + O2(g) → 2K2O(s)

4 mol of K react with 1 mol of O2 produce 2 mol K2O

Step 2: Calculate the number of mole [Get the information from the question]

Step 3: Find the coefficient From Balance Chemical EquationFBCE;4 mol of K produce 2 mol K2OThus; 0.1 mol of K produce 2/4 mol K2O = 0.2 mol K2O

FBCE;[Sebelah kiri] [Sebelah kanan]Bil. mol yang telah dikira Bil. Mol yang hendak ditentukan

4 mol K = 2 mol K2O

0.1mol K = 2/4 x 0.1mol K2O = 0.05 mol K2O

No. of mol of K2O = 0.05 mol

Step 4: Solve the questionsThus; Mass of K2O = 0.05 mol × Molar mass

= 0.05 mol× 55 g mol-1

= 2.75 g

Example 3:Acids reacts with calcium carbonate, CaCO3 in limestone to form a salt and carbon dioxide, CO2.

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No. of mol K =mass

Molar mass

=3.9 g

39 gmol-1

0.1 mol=

A piece of limestone reacted completely with 100 cm3 of 31.5 g dm-3 nitric acid, HNO3. [Relative atomic mass: H, 1; C, 12; N, 14; O, 16; Ca, 40. Molar volume: 24 dm3 mol-1 at room conditions]a. Calculate the mass of salt produced. b. What is the volume of carbon dioxide, CO2 liberated at room conditions?

Step 1: Write Chemical EquationChemical Equation: 2HNO3 + CaCO3 → Ca(NO3)2 + CO2 + H2O

Step 2: Calculate the number of mole Get the information from the question;

FBCE; 2HNO3 + CaCO3 → Ca(NO3)2 + CO2 + H2O

2 mol HNO3 = 1 mol Ca(NO3)2

0.05 mol HNO3 = ½ x 0.05 mol Ca(NO3)2 = 0.025 mol Ca(NO3)2

No. of mol of Ca(NO3)2 = 0.025 mol

Mass of Ca(NO3)2 = 0.025 mol × 40 + 2[14 + 3(16)] g mol-1 = 4.1 g

FBCE; 2HNO3 + CaCO3 → Ca(NO3)2 + CO2 + H2O 31

No. of mole of HNO3 =Molarity × Volume

1000

=0.5 mol dm-3 × 100 cm3

1000

= 0.05 mol

Concentration of HNO3 = 31.5 g dm3

=Molar mass of HNO3

31.5 g dm3

= 0.5 mol dm-3

=31.5 g dm3

1 + 14 + 48 g mol-1

Change the concentration given in g dm-3 to mol dm-3 first

2 mol HNO3 = 1 mol CO2

0.05 mol HNO3 = ½ x 0.05 mol CO2 = 0.025 mol CO2

No. of mol of CO2 = 0.025 mol

Volume of CO2 = 0.025 mol × 12 + 2(16) dm3 mol-1 = 1.1 dm3

Example 4:Pb(NO3)2 compound decomposes when heated as shown in the following equation.If 6.62 g of Pb(NO3)2 compound is heated, calculate;[Relative atomic mass: N, 14; O, 16; Pb, 207; 1 mol of gas occupies 22.4 dm3 at s.t.p.] (i) mass of PbO that is produced (ii) volume of nitrogen dioxide produced at s.t.p (ii) volume of oxygen produced at s.t.p

Solution:

FBCE; 2Pb(NO3)2 → 2PbO + 4NO2 + O2

2 mol Pb(NO3)2 = 2 mol PbO

0.02 mol Pb(NO3)2 = 0.02 mol PbO

No of mol PbO = 0.02 mol

Mass of PbO = 0.02 x 223 = 4.46 g

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No of mol Pb(NO3)2 =mass

Molar mass

=6.62 g

331 gmol-1

0.02 mol=

2Pb(NO3)2 → 2PbO + 4NO2 + O2


2 mol Pb(NO3)2 = 4 mol NO2

0.02 mol Pb(NO3)2 = 4/2 x 0.02 mol O2 = 0.04 mol O2

No of mol O2 = 0.04 mol

Volume of O2 = 0.04 x 22.4 dm3 = 0.896 dm3 // 896 cm3


2 mol Pb(NO3)2 = 1 mol O2

0.02 mol Pb(NO3)2 = ½ x 0.02 mol O2 = 0.01 mol O2

No of mol O2 = 0.01 mol

Volume of O2 = 0.01 x 22.4 dm3 = 0.224 dm3 // 224 cm3

Numerical Problems involving stoichiometric reactions in the precipitation of salts

Question 1:A student prepare copper(II) nitrate, Cu(NO3)2 by reacting copper(II) oxide, CuO with 200 cm3 of 2.0 moldm-3 nitric acid, HNO3. Calculate the mass of copper(II) oxide, CuO needed to react completely with the acid. [Relative atomic mass: Cu, 64 ; O, 16]

Question 2:X cm3 of 0.5 moldm-3 sulphuric acid, H2SO4 is added to 100 cm3 of 1.0 moldm-3 lead(II) nitrate solution to produce lead(II) sulphate, PbSO4.[Relative atomic mass: Pb, 20; O, 16; S, 32]

a. Calculate the value of X.b. Calculate the mass of lead(II) sulphate obtained.

Start to do exercises from any book. I will help and guide you to master this topic.

Prepared by;Kamal Ariffin Bin SaaimSMKDBL

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notes updates salts

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