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KCl NaCl AgF

Lösungsvorgang von Salzen. D H L. NaCl(s) Na + (aq) + Cl – (aq). Hydration D H H < 0. Gitter- spaltung D H G > 0. D H (kJ/mol). Gitter-enthalpie. Hydrations-enthalpie. Na + (g) + Cl – (g).

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KCl NaCl AgF

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  1. Lösungsvorgang von Salzen DHL NaCl(s) Na+ (aq) + Cl–(aq) Hydration DHH < 0 Gitter-spaltungDHG > 0 DH (kJ/mol) Gitter-enthalpie Hydrations-enthalpie Na+(g) + Cl–(g) DHG = DHH  temperaturneutral DHG > DHH  endotherm DHG < DHH  exotherm DHG >> DHH  sehr schlecht löslich KCl NaCl AgF Lösungs-enthalpie

  2. Wasserlöslichkeit von Salzen d+

  3. d– d+ d+ d+ d– d+ d– d+ d+ Anlagerung von Wassermolekülen d+

  4. d+ d– d+ d– d+ d+ d+ d+ d– d– d+ d– Ablösung von Ionen

  5. d+ d– d+ d– d+ d+ d+ d+ d– d– d+ d– Ablösung von Ionen

  6. d+ d– d+ d– d+ d+ d+ d+ d– d– d+ d– Salzlösung

  7. d– d+ d+ d+ d– d+ d– d+ d+ Schwer lösliche Salze d+ Salze mit je 2-fach geladenen Ionen sind (meistens) schlecht löslich.

  8. d– d+ d+ d+ d+ Kräfte zwischen Ionen und Molekülen Ion d– d– d– d+ d+ Dipol Ion-Dipol-Kräfte Ion-Dipol-Kräfte

  9. d– d+ d+ d+ d+ stabilerAbstand kleiner weniger stabilAbstand grösser Aquakomplexe Zentralteilchen d– d– d– d+ d+ Liganden Aquakomplex Aquakomplex

  10. Kräfte zwischen den Stoffteilchen Van der Waals- Dipol-Dipol- Wasserstoff- Ion-DipolKräfte Kräfte brücken Kräfte + d++d-- d+d- d-- d++ d++d-- d+d- am schwächsten am stärksten

  11. Salzhydrate CoCl2 CoCl2. 6H2O [Co(H2O)6]Cl2

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