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lime

lime. objectives. To get information history of lime To learn about types of lime To get information properties of lime. HISTORY of LIME. One of the oldest binding materials Babylon , Egypt , Persian , Hittite Roman, Turks , Byzantine. PROPERTIES OF LIME.

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lime

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  1. lime

  2. objectives • Togetinformationhistory of lime • Tolearnabouttypes of lime • Togetinformationproperties of lime

  3. HISTORY of LIME • One of theoldestbindingmaterials • Babylon, Egypt, Persian, Hittite • Roman, Turks, Byzantine

  4. PROPERTIES OF LIME • General termforcalcium-containinginorganicmaterials • Generallyknown as calciumoxideorcalciumhydroxide • Source: quarriesormines Limestonequarry in ChesterCounty

  5. APPEREANCE OF LIME • White, andlargestone • Bindingagent • Can be solidify in air, orwater (depends on thetype of lime)

  6. TYPES OF LIME • Hydraulic Lime • Slaked Lime (CalciumHydroxide) • Unslaked Lime (CalciumOxide) • Marble, Calcite, Limestone (CalciumCarbonate)

  7. HYDRAULIC LIME • Producedbyheatingcalcininglimestone (clay, otherimpurities) • Usages: 1) usefulbuildingmaterial • -lesspolluting • -does not trap moisture in thewall • -no needforexpansionjoints

  8. SLAKED LIME (calciumhydroxide) • Ca(OH)2 • Colourlesscrystalorwhitepowder • Producedbymixingcalciumoxideandwater • Usages: - in themanufacture of foodandliquors • -refiningpetroleum • - purification of water • - fillingtherootcanal (firststage of therapy)

  9. Warning ! • Calciumhydroxidemaycausedangerousillnessesif it is in excess in the body. • 1) Skin irritation • 2) Blindless • 3) LungDamage • 4) InternalBleeding • 5) HighBloodPressure • 6) Dyspnea

  10. Ifyouheatcalciumhydroxideuntil it reaches 512°C, it decomposesintocalciumoxideandwater.

  11. UNSLAKED LIME (Calciumoxide) • White, corrosive, alkaline solid • Producedfromheatingimpurelimestones at 825°C. (calcination) • Leavingcarbondioxide (CO2) • Usages: - additive in whitepaints • - substanceformakingcementandpulp • - mostlyproduced in China

  12. Calciumoxidereactswithwatervigorously.

  13. WARNING ! • Calciumoxide can causediseasesif it is usedincorrectly. • 1) Inhalingcalciumoxide : coughing, sneezing • 2) Touching : nasal septum, abdominal pain, nausea and vomiting

  14. CALCIUM CARBONATE • Exists on thenature (marble,chalk) • veryreactive alkaline • Tounderstandwhether a materialcontainscalciumcarbonate, weusesulphuricacidorhydrochloricacid.

  15. USAGES • - purification of ironore • - component of blackboardchalk • - in constructions ( not onlycalciumcarbonate) • - unreactive filler fortablets • - substance in toothpastes • - helpsexcretionsystem

  16. Chemicalreactions • CaCO3 → CaO + CO2 (decomposition of calciumcarbonate) • Heatingabove 840°C • Ca(OH)2 + CO2 → CaCO3 + H2O (producingcalciumcarbonate)

  17. Burak YILDIRIM 9/D - 222 THANKS FOR LISTENING.

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