Solubility of CO2 in water?

Question

What intermolecular force or bond is responsible for the solubility of CO2 in water?
a) London dispersion force
b) Hydrogen Bonding
c) Ionic Bonding
d) Covalent Bonding
e) Dipole/induced dipole force
and WHY?

Answer 1

At standard temperature and pressure, the solubility of CO2 is only about 0.03 moles/L. Most of this is due to the formation of Carbonic acid, which can dissociate:

CO2 + H2O --> H2CO3 --> H+ + (HCO3)-

Although it is this last step which keeps the CO2 in solution (the ionic bonding), it is the (e) Dipole of the water that induces a dipole force in the symmetrical CO2 that allows the first part of the reaction to take place.

Answer 2

Hydrogen Bonding will probably be the largest influence. However, CO2 is not very soluble in water (that's why sodas go flat when you leave them open. The extra pressure that's applied when canned keeps it in). CO2 is a straight shaped molecule with carbon in the middle and oxygen on the outside. There will be a more negative overall charge around the oxygen, but not as much as the water (in other words, there is no dipole moment). London dispersion forces are hapening but they are so weak that they don't have a great affect here. Water has a dipole moment, so the positive end would be attracted to the slightly negative areas of the CO2. This attraction is just very weak. Ionic bonding is a very strong bond and is actually a chemical bond (think salt). You can heat it with a torch and it won't break. Covalent bonding is what holds oxygen and carbon together in CO2. Hope that helps with this question and any others you might have.

Answer 3

Solubility Of Co2

Answer 4

E.

Carbon Dioxide DOES dissolve in water but the solubility rate is not high. If not, there is no carbonic acid in this world. The general equation would be

H2O + CO2 <-> HCO3- + H+

We can generally say that from the ionic equation (w/o symbols) that answer a,b,d are out. Ionic bonding is not the main bond because it does not keep the carbonic acid in water; it just give rise to that HCO3- ion. It is the dipole-dipole form that give rise to the solubility of CO2 in water. The dipole-dipole attraction gave rise to that solute-solvent bond.

Answer 5

Tell Pepsi and CocaCola that CO2 doesn't dissolve in water...

Ionic and covalent bonding are out immediately as they are chemical bonds.

Hydrogen bonding occurs when an electron deficient atom is drawn to an electron rich source. AKA when electron rich oxygen atoms in water are drawn to electron poor hydrogens in neighboring water molecules.

London dispersion forces (AKA van der waals' forces) are non-permanent dipole interactions. They can occur in nonpolar molecules, such as CO2, due to transient charges on the atoms in carbon dioxide (electron density will change periodically). This is most like your culperate.

Answer 6

I would have to say e because the water's dipoles allow other molecule to "side" in between the hydrogen bonds that is why water is the universal solvent.
you might want to look up cabonic acid because that what CO2 in water is

Answer 7

Read my hand to Dana. At least half the CO2 from the industrial period has been uptaken by the oceans. Trying to explain a perfect equilibrium between H2O and CO2 would damn never make a person God. They know it does exist, and can explain why it occurs as a primary reactant--->. But they haven't, and under all likely hood, will never explain the reverse reaction<----. Unfortunately this is one of the many things pending, with man's understanding of natural balances.

Answer 8

i don't know for sure but id say e) Dipole/induced dipole force is because its the weakest and co2 does not dissolve very well and is released easily when it is

Answer 9

CO2 is NOT soluble in water.

O=C=O is a Non-polar molecule and therefore will not dissolve in water. This is why our body uses Sodium Bicarbonate to transport the CO2 from our muscles to our lungs.

Like dissolves like and CO2 only dissolves in a hydrophobic solvent.

Answer 10

richard just got this by googling u could have done the same thing. dont trust him.