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Swaeligsuur: Verskil tussen weergawes

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Lyn 3:
:: <math>SO_2 +H_2O \to H_2SO_3</math>
 
Die ekwilibruimreaksie word soos volg voorgestel:
::<chem>SO_2 + H_2O <=> HSO_3^− + H^+ </chem> {{spaces|10}}''K''<sub>a</sub> = 1.54{{e|−2}}; p''K''<sub>a</sub> = 1.81.▼
 
▲::<chem>SO_2 + H_2O <=> HSO_3^−- + H^+ </chem> {{spaces|10}} ''K''<sub>a</sub> = 1.54{{e|−2}}; p''K''<sub>a</sub> = 1.81.
::<chem>SO_2 </chem>
 
As ons probeer om die oplossing te konsentreer deur verdamping om waterlose swaeligsuur te produseer, sal dit ontbind (die vormingsreaksie sal omgekeer word).
''K''<sub>a</sub> = 1.54{{e|−2}}; p''K''<sub>a</sub> = 1.81.
 
Wanneer dit afgekoel word sal <chem>SO_2 \cdot 5.75 H_2O</chem> kristalliseer wat weer by 7 °C sal ontbind. Dus kan swaeligsuur H<sub>2</sub>SO<sub>3</sub> nie geïsoleer word nie.
: [H–OSO<sub>2</sub>]<sup>−</sup> ⇌ [H–SO<sub>3</sub>]<sup>−</sup>
 
When trying to concentrate the solution by evaporation to produce waterless sulfurous acid it will decompose (reversing the forming reaction). In cooling down a [[clathrate]] SO<sub>2</sub> · 5.75 H<sub>2</sub>O will crystallise which decomposes again at 7 °C. Dus kan swaeligsuur H<sub>2</sub>SO<sub>3</sub> nie geïsoleer word nie.
 
== Kyk ook ==
Ontsluit van "https://af.wikipedia.org/wiki/Swaeligsuur"