Question

Why is co2 is more dissolve in water than O2

Answer 1

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.

Answer 2

Hii..
The dissolving of a gas in water depends on the interaction between the molecules of the gas and the water molecules. O2 has reduced solubility in water as compared to CO2. The reason of poor solubility of O2 in water is that they just occupy the intermolecular spaces and stays there by interaction with its surrounding molecules by weak van der Waals forces or weak interactions between lone pairs of oxygen with water. CO2 when dissolves in water it interacts with surrounding H2O molecules to hydrate itself, i.e. the electronegative oxygen atoms of CO2forms strong H-bond with H atoms of water molecules, This interaction is very strong to dissolve more and more CO2 molecules. Some of them (H2O bound to CO2) release protons to increase H+ ions in water and CO2converted into HCO3-.
Equilibrium is established between the dissolved CO2 and H2CO3, carbonic acid.
CO2 (aq) + H2O = H2CO3 (aq)

This reaction is kinetically slow. At equilibrium, only a small fraction (ca. 0.2 - 1%) of the dissolved CO2 is actually converted to H2CO3. Most of the CO2remains as dissolved molecular CO2.

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