spc561_chapter 3 salts

7/28/2019 SPC561_Chapter 3 Salts

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REF


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EXAMPLE :

Metal ions

Ammonium ion

replace

replace

Ammo

Sodiu


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SALTS CONSIST ANION PART COMES FROM THE ACID

CATION PART COMES FROM BASES

Common cations

Com

anio(parent

Na+

K+

NH4+

Ca2+ Mg2+

Al3+ Zn2+

Pb2+


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Metal

ion

Sulphate

salts

+ H2SO4

Chloride

salts

+ HCl

Carbonate

salts

+ H2CO3 +

Na+

Na2SO4 NaCl Na2CO3Mg 2+ MgSO4 MgCl2 MgCO3 M

Cu 2+ CuSO4 CuCl2 CuCO3

Al 3+ Al2(SO4)3 AlCl3 Al2(CO3)3


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All nitrate salts ; soluble saltBarium

nitrate,

Ba(NO3)2

Calcium

nitrate,

Ca(NO3)2

Aluminium

nitrate,

Al(NO3)3

Silver

nitrate,

AgNO3

Lead(II)

nitrate,

Pb(NO3)2

Potassium

nitrate,

KNO3Sodium

nitrate,

NaNO3Copper(II)

nitrate,

Cu(NO3)2


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All salts ; soluble Potassium

carbonate,

K2CO3

Sodium

carbonate,

Na2CO3

Ammonium

carbonate,

(NH4)2CO3

Potassium

sulphate,

K2SO4

Potassium

chloride,

KCl

Potassium

nitrate,

KNO3

Sodium

nitrate,

NaNO3

Sodium

chloride,

NaCl


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All carbonate salts ; insoluble sMagnesium

carbonate

MgCO3

Calcium

carbonate

CaCO3

Silver

carbonate

Ag2CO

3

Other names[hide]

Silver(I)Carbonate

Copper(II)carbonate

CuCO3Zinccarbonate

ZnCO3Manganese(II)

carbonate

MnCO3

Potassium

carbonate

K2CO3

Ammonium

carbonate

(NH4)2CO3

2


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Mercury(II)

Chloride

HgCl2

All SO42-, Cl- salts ; soluble salt

Silver(I)

ChlorideAgCl

Lead(II)

ChloridePbCl2

Cl-

Bariumsulphate

BaSO4

Lead(II)

sulphate

PbSO4


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Copper(II)

Chloride

CuCl2

Iron(II)

Chloride

FeCl2

Magnesium

Chloride

MgCl2

Copper(II)

sulphate

CuSO4

Aluminium(II)

sulphate

Al2(SO4)3

Zinc

Chloride

ZnCl2

P

c

c


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NO3-

CLASSIFICATION OF SA

PbSO4CaSO4BaSO4

PbCl2AgCl

SO42-

Cl-


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PREPARATION OF SALTS

odium ,Na+ salts

otassium, K+ salts

mmonium, NH4+ salts


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PREPARATION OF SOLUBLE SALT

[ SODIUM SALTS / POTASSIUM SALTS / AMMONIUM

PREPARATION OF POTASSIUM CHLORIDEEXAMPLE

K OHH Cl ClK

.


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LET DO THIS:

PREPARATION OF POTASSIUM CHLORIDE

APPARATUS : Pipette 25mL, Burette 50mL, Conical Flask 250 mLMATERIALS : Potassium hydroxide 1.0 M, Hydrochloric acid 1.0 M, Ph

Use a pipette to

transfer 25.0 cm3 of

potassium

hydroxide solutionto a conical flask.

Add 2 to 3 drops of

Colourless KOH

turn to pink.

Fill a burette

with

hydrochloric

acid and

record theinitial

burette

reading.

Record the burette

reading in 2d.p

Slowl

acid i

flask

until t

turns colou

the vo

used.

Reco


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Pipette 25.0 cm3

of the same

potassium

hydroxide solution

into a conical

flask.

Do not add anyindicator.

From the

burette, add

exactly V cm3

of hydrochloric

acid to the

alkali and

swirls andshake well.

PREPARATION OF POTASSIUM CHLORIDE

START OVER AGAIN BUT WITHOUT INDICATOR :To get the pure and neutral salt solution

HEATING

CO

FIL

Solution salt contains

impurities continuous with

recrystallisation process


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PREPARATION OF SOLUBLE SALT

[ OTHER SALTS EXCEPT Na+, K+, NH4+]

Pour 50 cm3of sulphuric acid

into a beaker. Warm the acid

Use a spatula to add

copper(II) oxide powder bit by

bit into the acid. Stirthe

mixture well. Continue addingcopper(II) oxide until some of

it no longer dissolves(excessunreacted metal

See the change of metal solid

colour and dissolve

Solu

impurit

recrys

Glass rod

Acid

Metal/ metal oxide/

metal carbonate

Ex

un

(re


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HEATING/EVAPORATE COOL

Evaporating

basin

Saltsolution


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FILTRATION DRY

The crystals are filtered

and rinsed with a little

cold distilled water.

Rinse

with

distilled

water

Glass rod

Salt Cystals FilterPaper

These physic

Regulars ge

such as cub

Flat faces, s

sharp angle

Same angle

faces.


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DISSOLVE ACHEATDISSOLVE M

EXCESS MECOMPLET

NEUTRALISATIONREACTION1ST TITRATION WITH INDICATORFIND VOLUME OF ACID2ND TITRATION NO INDICATORGET PURE SALT

PREPARATIONOF SOLUBLESALTS

TRANSFER TOEVAPORATING

BASIN

HEATING/EVAPORATECOOLINGFILTRATION

DRY

PREPARATION OF INSOLUBLE SAL


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PREPARATION OF INSOLUBLE SAL

[ ALL CARBONATE SALTS except Na+/K+/N

PbSO4 / CaSO4/ BaSO4/PbCl2/ AgCl]

PREPARATION OF LEAD(II) CHLORIDEEXAMPLENa ClPb NO3

DOUBLE DECOMPOSITION METHOD TWO AQUOUES SOLUTIONS/SOLUBLMIX TOGETHER INTERCHANGE TO PRODUCE TWO NEW COMPOUND WHICSALT OR PRECIPITATE, AND AQUEOUS SOLUTION/SOLUBLE SALTS

Cl2b

/


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the ions of the two aqueous solutions above interchang

two new compound which is insoluble salt or pre

aqueous solution

[onesolucontaanioninsolu

two aquoues solutions/soluble salts were mix

[one of thesolutionscontains thecations of theinsoluble salt]


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Mixture solutions

Filter paper

Retort

stand

Precipitate

(residue)

Filter

funnel

Aqueous

Solution

(filterate)

Glass

rod

Filtration : Remove solution fromprecipitate

Distilled

water

Rinse : remove


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Filter paperPrecipitate

/Soluble

salts

Dry : Dried by pressing between twopieces of filter paper.

FLOW CPREPARAINSOLUBLMIX -

TWO SOLUBFILTRAREMOVE F

RINREMOVE OT

DRPRESS BETWEEN

PREPARATION OF SALT


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PREPARATION OF SALTREMEMBER : METAL ION DISPLACE

HYDROGEN ION IN ACID TO FORMED SAL

HCl [H+/Cl-]

Hydrochloric acid

HNO3 [H+/NO3

Nitric Acid

H2SO4 [2H+/SO4

Nitric Acid

H2CO3 [2H+/CO3

Nitric Acid

Na+

K+

NH4+

Ca2+

Mg2+ Cu2+

Fe2+Fe3+

Al3+

Zn2+

Pb2+


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Method/Reaction Reason

Neutralisation

(Titration method)

Alkali + Acid Salts + Water

Most salts of sodium,

potassium, and ammonium

ions are soluble.Metal Displacement

Metal + Acid Salts + HydrogenMore electropositive metal

can be displaced hydrogen

ion from acid.

Metal oxide + Acid Salts + Hydrogen Less electropositive metalnot be displaced hydrogen

ion from acid.

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


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Reactive metal is magnesium, aluminium, and zinc. Unrea

metal is iron, lead, silver

Metal that is less reactive from hydrogen such as copper, l

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.


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Metal, metal oxide and metal carbonate is a solid that cannot

dissolves in water, hence during reaction that solid must be add

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) cann

react with dilute acid. So to prepare salt contains lead ions (Pb2+

), copions (Cu2+) or silver ions (Ag+), we must use either oxide powder or

carbonate powder only.

Impure soluble salt can be purified through crystallization proce

spc561_chapter 3 salts

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