Why co2 more soluble in water than o2 explain the process?
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The reason for poor solubility of O2 or H2 in water is because they just occupy the inter molecular spaces & stay there by interaction with its surrounding molecules by weak Vander waals forces or very weak electronic interaction by use of its pi electrons or lone pairs.
CO2 when dissolves in water, interacts with surrounding h2o molecules to hydrate itself, i.e. the electro negative atoms of CO2 forms strong H-bond with H atoms of water molecules. This interaction is very strong to dissolve more & more CO2 molecules.
Some of them (H2O BOUND TO CO2) release protons to increase H+ ions in water
Equilibrium is established between the dissolved CO2 and H2CO3.
CO2(aq)+ H20 = H2CO3 (aq)
The reaction is kinetically slow. At equilibrium, only a small fraction (ca. 0.2% - 1%) of dissolved CO2 is actually converted to H2CO3. Most of CO2 remains as dissolved molecule of CO2.
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The reason for poor solubility of O2 or H2 in water is because they just occupy the inter molecular spaces & stay there by interaction with its surrounding molecules by weak Vander waals forces or very weak electronic interaction by use of its pi electrons or lone pairs.
CO2 when dissolves in water, interacts with surrounding h2o molecules to hydrate itself, i.e. the electro negative atoms of CO2 forms strong H-bond with H atoms of water molecules. This interaction is very strong to dissolve more & more CO2 molecules.
Some of them (H2O BOUND TO CO2) release protons to increase H+ ions in water
Equilibrium is established between the dissolved CO2 and H2CO3.
CO2(aq)+ H20 = H2CO3 (aq)
The reaction is kinetically slow. At equilibrium, only a small fraction (ca. 0.2% - 1%) of dissolved CO2 is actually converted to H2CO3. Most of CO2 remains as dissolved molecule of CO2.
hope ull get the answer and mark as brainliest one
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