The concentration of dissolved CO₂ in the ocean water increases proportionally to the partial pressure of CO₂ in the air.

x_co2 = (1/H_co2) x P_co2

with

x_co2 : mole fraction of CO₂ in ocean water

P_co2 : CO₂ partial pressure in air

H_co2 : Henry's law constant which depends on temperature

The reaction between dissolved CO2 and H₂O is reversible and rapid:

CO₂(aq) + H₂O <-> HCO₃^- + H⁺

HCO₃^- <-> CO₃^2- + H⁺

With the concentration of dissolved CO₂ set by Henry's Law, and with the known equilibrium constants of the above dissociation reactions, the concentration of protons and bicarbonate ions in the liquid phase can be determined as these ions have their roles in the reactions that take place in ocean water.

Oceans are thus CO₂ sinks, absorbing more CO₂ when cold, but are also sources of CO₂ when hot.  Marine life decomposition and certain type of sea-dwelling bacteria also emit CO₂.

The equilibrium between air CO₂ ppm and ocean water CO₂ concentration is thus governed by physical laws and biochemical reactions, making it not easy to reduce air CO₂ ppm by just capturing air CO₂ or by limiting human generated CO₂ emissions.

Our technique for atmosphere CO₂ & energy capture and sequestration addresses this problem of Mass and Energy Releases to the atmosphere caused by human activities and that is the source of climate disasters. 

Further, ocean water is free and abundant, we adjust it to simultaneously capture energy and CO₂.  Also, its alkaline-earth ions are free and abundant; we use these ions for CO₂ sequestration.