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 waterSodium saltsPotassium salts Ammonium salts
All dissolves in water
Nitrate salts All dissolves in water
Chloride salts
All dissolves in water, Except: Lead(II) chloride, PbCl2
Silver chloride, AgCl Mercury chloride, HgCl
Sulphate salts
All dissolves in water Except: Lead(II) sulphate, PbSO4
Barium sulfat, BaSO4
Calcium sulfat, CaSO4
Carbonate All did not dissolves in water, Except: Sodium 1
Salt is an ionic compound formed when the hydrogen ion, H+ from acid is replaced by a metal ion or
ammonium ion, NH4+
salts
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 waterbut dissolve in hot water.
Use of salts;
Item Use Example
Food preparation Flavor Monosodium glutamate (MSG)
Sodium chloridePreservatives Sodium chloride - salted fish
Sodium benzoate - sauce
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White precipitate of PbCl2
White precipitate dissolves in hot water
White precipitate formed when the water is cooled down.
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.
PbCl2 are soluble in hot water.
Sodium nitrite - processed meat, burger
Baking powder Sodium hydrogen carbonateAgriculture Nitrogen
fertilizersPotassium nitrateSodium nitrate
Pesticide Copper(II) sulphateIron(II) sulphate
Medicine
Reduce stomach acidic (gastric)
Calcium carbonateCalcium hydrogen carbonate
Sniff salt (fainted)
Ammonium carbonate
Plaster 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
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;
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- 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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Anion(Non-m etal ion)
Cation(M etal ion) nn mm
Chemical and ionic equations
Chemical equation : MX(aq) + NY(aq) → MY(s) + NX(aq)
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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
Glass rod
Residue/precipitate (Insoluble salt)
Filtrate (Soluble salt)
Mixture of solutions
Filter funnel
Filter paper
Retort stand
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
ii. Preparation and purification of insoluble salts
Preparation of Plumbum(II) iodide
Chemical equation : Pb(NO3)2 (aq) + 2KI (aq) → PbI2 (s) + 2KNO3 (aq)
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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.
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+ →
20 cm3
Lead(II) nitrat
0.1 mol dm-3
20 cm3
potassium iodide
0.1 mol dm-3
Glass rod
Precipitate of lead(II) iodide(yellow)
Sodium nitrate solution
Mixture of solutions
Filter funnel
Filter paper
Retort stand Beaker
4. The mixture is filtered to obtain the yellow solids of lead(II)iodide as the residue.
Step 2: Purification
5. The residue is rinsed with distilled water to remove other ionsin 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 alkalireaction.
Salt Alkali Acid Chemical equation
NaCl NaOH HCl NaOH + HCl → NaCl + H2O
K2SO4 KOH H2SO4 2KOH + H2SO4 → K2SO4 + 2H2O
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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 Salt Acid that mustbe used
Substance that can be use to react withacid
Metal Metal oxide Metal carbonateZnCl2 HCl Zn ZnO ZnCO3
Mg(NO)3 HNO3 Mg MgO MgCO3
CuSO4 H2SO4 × CuO CuCO3
Pb(NO3)2 HNO3 × PbO PbCO3
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 salts10
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.
Example: Preparing sodium chloride
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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)
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Retortstand
Burette
Hydrochloric acid
Conical flask
25 cm3 NaOH + phenolphthalein indicator
8. The mixture is transferred into a evaporating dish.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.
Step 3: Purification
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.
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Bunsen burner
Evaporating dishSalt solution
Glass rodDistilled water
Copper(II) sulphateFilter funnel
However experiment is repeated without using phenolphthalein so that the salt prepared will not contaminated by the indicator.
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 pouredinto 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 nolonger dissolve anymore. (the solid is excess and all the acid is completely neutralised by the solid)
14Heating
Acid Powderof :
M etal oxideM etal carbonateM etal
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.
Example: Preparing copper(II) sulphate (Sulphuric acid and copper(II) oxide powder) Step 1: Preparation
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Excess of solid powder
Filtrate (Salt solution)
Heating
Saturated solutionCrystals
Filtrate
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 withglass 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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Copper(II) oxide
Glass rodBeaker
Wire gauze
50 cm3 sulphuric acid 0.1 mol dm-3
Tripod Bunsen burner
SpatulaStir
Glass rodReactant 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.
Step 3: Purification
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
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Bunsen burner
Evaporating dish×××××××××××
×
Copper(II) sulphate solution
Glass rodDistilled water
Copper(II) sulphate
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 orcarbonate powder only.
Example: CuO + H2SO4 CuSO4 + H2O (ok)
CuCO3 + H2SO4 CuSO4 + H2O + CO2 (ok)
Cu + H2SO4 no reaction (not ok)
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.
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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 anionspresent.
C. QualitativeAnalysis ofSaltsWhat is Qualitative analysis?
In the qualitative analysis of salts, we need to identify the ionsthat 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 solid
Solubilityin water
Colour in Aqueous solution
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Salt Solubility in waterSodium, 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 (SO4
2-) All sulphate salts are soluble in
water except PbSO4, BaSO4 and CaSO4
Carbonate salt (CO3
2-) 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.
1. Ammonium chloride NH4Cl white soluble colourless2. Ammonium nitrateNH4(NO3)3 white soluble colourless3. Calcium carbonate CaCO3 white insoluble -4. Calcium nitrate Ca(NO3)2 white soluble colourless5. Magnesium sulphate MgSO4 white soluble colourless6. Magnesium carbonate MgCO3 white insoluble -7. Zinc sulphate Zn SO4 white soluble colourless8. Zinc nitrate Zn(NO3)2 white soluble colourless9. 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
brown17. Sodium nitrate , NaNO3 white soluble colourless18, Sodium carbonate , Na2CO3 white soluble colourless19. 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
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Brown solid Hydrated Fe 3+ salt
White solid Salts 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 salts All are soluble
Chloride salts All are soluble except AgCl, HgCl and PbCl2 (soluble in hot water)
Sulphate salts All are soluble except BaSO4, PbSO4 and CaSO4
Carbonate salts All are insoluble except sodium carbonate, potassiumcarbonate 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
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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 ,CO2
Bubble 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, HCl
Test 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
Nitrogen dioxide gas , NO2
Test with moist blue litmus paper
moist blue litmus paper turns red
3. Action of heat on salts
Effect of heat on carbonate salts
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Carbonaate salt Colour of salt before heating
Colour of residue Effect on lime water
Hot cold
Copper (II) carbonate, CuCO3
Green powder Black powder
Black powder
The gas liberated turns lime water milky/chalky
Zinc carbonate , ZnCO3
White solid Yelow solid White solid
The gas liberated turns lime water milky/chalky
Lead(II) carbonate, PbCO3
White solid Brown sold Yelow solid
The 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 solid
The 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 solid
The 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
Copper (II) nitrate, Cu(NO3)2
Blue solid Blackpowder
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 solid Yellowsolid
White solid
A browan gas that turns bluelitmus paper red is liberated.The gas liberated also ignites a glowing splinter
Lead(II) nitrate, Pb(NO3)2
White solid Brown solid
Yellowsolid
A browan gas that turns bluelitmus paper red is liberated.The gas liberated also ignites a glowing splinter
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Sodium nitrate,NaNO3
White solid White solid
White solid
A colourless gas that rekindles a glowing splinteris liberated
Calcium nitrate, Ca(NO3)2
White solid White solid
White solid
A browan gas that turns bluelitmus paper red is liberated.The gas liberated also ignites a glowing splinter
Potassium nitrate, KNO3
White solid White solid
White solid
A colourless gas that rekindles a glowing splinteris liberated
Magnesium nitrate, Mg(NO3)2
White solid White solid
White solid
A browan gas that turns bluelitmus paper red is liberated.The gas liberated also ignites a glowing splinter
Iron(II) nitrate, Fe(NO3)2
Pale Green solid
Pale Green solid
Pale Green solid
A browan gas that turns bluelitmus paper red is liberated.The gas liberated also ignites a glowing splinter
Iron(III) nitrate, Fe(NO3)3
Brown solidReddish-Brown solid
Reddish-Brown solid
A browan gas that turns bluelitmus paper red is liberated.The gas liberated also ignites a glowing splinter
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.
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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.
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 / sulphuricacid 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 White precipitate SO42- ion Ba2+ + SO4
2 - BaSO4
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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
is formed.
2 cm3 of the unknown solution pour into atest tube 2 cm3 of dilute sulphuric acid + 2 cm3 of iron(II) sulphate solution shake well.Then drop carefully andslowly a few drops of concentrated sulphuric acid along the side of a slanting test tube into the mixture without shaking it.
Brown ring is formed at the boundary between the concentrated H2SO4 (top layer) and aqueous solution of the mixture (bottom layer)
NO3- ion -
Tests for cations
Confirmatory Test for Fe 2+ , Fe 3+ , Pb 2+ , NH 4+ Ions
Confirmatory Test for Fe 2+ 26
Reagent Observation ConclusionPotassium hexacyanoferrate(II) solution
Pale blue precipitate Fe2+ ion is present
Dark blue precipitate Fe3+ ion is present
Potassium hexacyanoferrate(III) solution
Dark blue precipitate Fe2+ ion is presentGreenish-brown solution Fe3+ ion is present
Potassium thiocyanate solution
Pale red colouration Fe2+ ion is presentBlood 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 coolto room temperature using runningwater 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 coolto room temperature using runningwater from the tap
- A yellow precipitate is formed
When heated – dissolve in water to form colourless solution
When cooled – yellow precipitate reappear
Pb2+ + 2I- PbI2
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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 redlitmus paper at the mouth of thetest 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 inexcess NaOH
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Cations
+ NaOH (aq)
Precipitate produced
No precipitate
White precipitate
Coloured precipitate
Green
Blue BrownFe2+ 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
Ca2+ Mg2+ : White precipitate insoluble/tidak larut in excess NaOH
Reaction of Cations With NH3
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Cations
Precipitate produced
No precipitate
White precipitate
Coloured precipitate
Green
Blue BrownFe2+ 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+ : White precipitate dissolves/larut in excess NH3
Pb2+ Al3+ Mg2+ : White precipitate insoluble/tidak larut in excess NH3
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.
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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).
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.
Example 1:
Describe chemical tests that can be carried out in the laboratory to differentiatebetween
(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.
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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.
(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.
If no change occurs, then the solution tested is iron(II) 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.
If no change occurs, then the solution tested is iron(II) chloride.
(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.
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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 gasthat changed moist blue litmus paper to red and colourless gas that lighted up a glowing wooden splinter are produced.
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D. Numerical problem involving stoichiometric reaction in the preparation of salt
Example 1;
Ammonium phosphate, (NH4)3PO4 is use as a fertilizer. 29.8g of thissalt is prepared by neutralizing phosphoric acid, H3PO4 with ammoniumgas, NH3. Calculate the volume of ammonium gas, NH3 reacted at roomconditions.( 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)
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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 1
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;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]
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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. 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?
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No. of mol K =mass
Molar mass
=3.9 g
39 gmol-1
0.1 mol=
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
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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
FBCE; 2HNO3 + CaCO3 → Ca(NO3)2 + CO2 + H2O 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
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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
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
FBCE; 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
FBCE; 2Pb(NO3)2 → 2PbO + 4NO2 +O2
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)
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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 Saaim
SMKDBL
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