An empirical correction function that describes this trend is applied to the basic model. Solubility … kilometers, or 360 trillion sq. A change of temperature of one degree for cold water changes the solubility … Temperature: The variation of solubility for a gas with temperature can be determined by examining the graphic on the left. Related: Total Alkalinity vs. pH and their roles in water chemistry. However, the effect is difficult to predict and varies widely from one solute to another. And the loss of CO 2 is where Henry's Law of physics comes into play. As CO 2 leaves the water–via aeration or algae consumption–pH will naturally rise. More gas is present in a solution with a lower temperature compared to a solution with a higher temperature. The water can obviously not hold the dissolved air with increased temperature. Above 20C the solubility drops by half to about 0.04g/kg/°C. Figure 3 is CO2 solubility in water: 0.08g/kg/degree C below 20C. I'm still curious to where this question came from, OP. The ocean surface area is 360 million sq. If the water is cooled down and then again reheated, bubbles will not appear until the water starts to boil. It states: Henry's Law of the Solubility of Gases. It was found that the solubility decreases with decreasing temperature in the hydrate formation region. The solubility of carbon dioxide in pure water in the presence of CO 2 gas hydrate has been measured at temperatures between 273 and 284 K and pressures ranging from 20 to 60 bar. Henry's Law is a law of physics formulated by William Henry in 1803. The top meter is 360 trillion tons of water. The solubility of the majority of solid substances increases as the temperature increases. Solubility of Gases vs. meters. The water is deaerated. At 100 o C (212 o F) water starts to boil - the bubbles are formed by evaporated water or steam. We will consider solubility of material in water as solvent. Solubility of CO 2 in water from −1.5 to 100 °C and from 0.1 to 100 MPa: ... At higher solubilities the activity coefficients show a systematic trend from values greater than unity at low temperatures, to values progressively lower than unity at high temperatures. As the temperature increases, the solubility of a gas decrease as shown by the downward trend in the graph . [CO2] in water is affected by A) pressure, B) temperature, and C) pH, I would now dismiss my initial assumption and believe the question is written to refer to [CO2] as solubility, as well explained by @aldol16.