Slide 1
Examples of Crystal
(Solubility, Structure, and Manufacture)
Candra Aditya Wiguna(6512010005)
Agenda
INTRODUCTION
IntroductionAcrystalorcrystalline solidis asolidmaterial whose
constituentatoms,molecules, orionsare arranged in anordered pattern
extending in all threespatial dimensions. In addition to their
microscopic structure, large crystals are usually identifiable by
their macroscopic geometrical shape, consisting of flat faces with
specific, characteristic orientations.
IntroductionCrystallizationis the (natural or artificial)
process of formation of solidcrystalsprecipitatingfrom
asolution,meltor more rarelydeposited directly from agas.
Crystallization is also a chemical solidliquid separation
technique, in which mass transfer of a solute from the liquid
solution to a pure solid crystalline phase occurs. Inchemical
engineeringcrystallization occurs in a crystallizer.
Crystallization is therefore an aspect ofprecipitation, obtained
through a variation of thesolubilityconditions of thesolutein
thesolvent, as compared to precipitation due to chemical
reaction.
Introduction
PyramidalDipyramidalDisphenoidal
TrapezohedralScalenohedralDipyramidalPyramidalDisphenoidalDomaticPrismaticSphenoidalPedialPinacodial
Tetartoidal
Diploidal
Rhombohedral
Cubic
Trigonal
Hexagonal
TetragonalOrthohombic
Monoclinic
Triclinic
Dipyramidal
Pyramidal
Trapezohedral
Pyramidal
Trapezohedral
Seven Crystall Structure System
Gyroidal6
EXAMPLES OF CRYSTALL
Examples of CrystallChesium Chlorida (CsCl)
Potassium Allum (KAl(SO4)2.12H2O)
Silica Dioxide (SiO2)
Sucrose (C12H22O11)
Calcite (CaCO3)
Caesium chlorideProperties
Widely used in:
Caesium chloride
Solubility Graph
Gram / 100 gram H2OTemperature (Co)Caesium chloride
Crystall Structure
Body Centered Cubic
Caesium chloride
PolluciteExctraction ProcessHydroclhoric AcidMixing
ProcessMixing ProcessAntimony chloride, iodine monochlorideHydrogen
sulfide
Manufacture
Heat
Crystalization Process
Caesium ChloridePotassium AlumProperties
Widely used in:
Potassium Alum
Solubility Graph
Potassium Alum
Crystall Structure
OrthorhombicPotassium AlumFrom alunite[edit]In order to obtain
alum fromalunite, it iscalcinedand then exposed to the action of
air for a considerable time. During this exposure it is kept
continually moistened with water, so that it ultimately falls to a
very fine powder. This powder is then lixiviated with hot water and
sulfuric acid, the liquor decanted, and the alum allowed to
crystallize. The alum schists employed in the manufacture of alum
are mixtures of ironpyrite, aluminiumsilicateand various bituminous
substances, and are found in upperBavaria,Bohemia,Belgium,
andScotland. These are either roasted or exposed to
theweatheringaction of the air. In the roasting process, sulfuric
acid is formed and acts on the clay to form aluminium sulfate, a
similar condition of affairs being produced during weathering. The
mass is now systematically extracted with water, and a solution of
aluminium sulfate ofspecific gravity1.16 is prepared. This solution
is allowed to stand for some time (in order that anycalcium
sulfateand basic ferric sulfate may separate), and is then
evaporated until ferrous sulfate crystallizes on cooling; it is
then drawn off and evaporated until it attains a specific gravity
of 1.40. It is now allowed to stand for some time, decanted from
any sediment, and finally mixed with the calculated quantity of
potassium sulfate, well agitated, and the alum is thrown down as a
finely divided precipitate of alum meal. If much iron should be
present in the shale then it is preferable to use potassium
chloride in place of potassium sulfate.From clays or
bauxite[edit]In the preparation of alum fromclaysor frombauxite,
the material is gently calcined, then mixed with sulfuric acid and
heated gradually to boiling; it is allowed to stand for some time,
the clear solution drawn off and mixed with acid potassium sulfate
and allowed to crystallize. Whencryoliteis used for the preparation
of alum, it is mixed withcalcium carbonateand heated. By this
means, sodium aluminate is formed; it is then extracted with water
andprecipitatedeither bysodium bicarbonateor by passing a current
ofcarbon dioxidethrough the solution. The precipitate is then
dissolved in sulfuric acid, the requisite amount of potassium
sulfate added and the solution allowed to crystallize.[citation
needed]AluniteCalcination ProcessExposure ProcessAir +
WaterLixiviated ProcessHot Water + Sulphuric
acidLiquorBauxiteCalcination ProcessMixing and Heating
ProcessSulphuric acidMixing ProcessAcid Potassium
SulfateLiquorLiquor
Manufacture
Crystalization Process
Potassium AlumCrystalization ProcessSilica DioxideProperties
Widely used in:
Silica Dioxide
Solubility Graph
Silica DioxideCrystall Structure
Trigonal
Hexagonal
Na2Si3O7+ H2SO4 3 SiO2+ Na2SO4+ H2OSilica DioxideSilica
QuadchloridaBurning processOxygenHydrocarbonSmoke SilicaSodium
QuadchloridaAcidification ProcessSulphuric acidWashing
ProcessDehydrated ProcessSiCl4+ 2 H2+ O2 SiO2+ 4 HCl
Manufacture
Crystalization ProcessSilica DioxideSucroseProperties
Widely used in:
Sucrose
Solubility Graph
Sucrose
Crystall Structure
Hexagonal
SucroseSugar CaneExtraction ProcessBoiling ProcessCentrifugal
SeparationRaw SugarWashing ProcesFilterSyrupPressureSugar
BeetsWashing and Slicing ProcessPurification
processFilterSugarBeets fiber
Manufacture
Crystalization ProcessCrystalization ProcessSoaking ProcessHot
WaterCalcium CarbonateProperties
Widely used in:Calcium Carbonat
Solubility Graph
Calcium Carbonat
Crystall Structure
Hexagonal
Calcium CarbonatLimestoneCalcination Process1000-3000oCMixing
processWaterCalcite
Manufacture
CONCLUSION
Conclucion
