CO2 solubility typically decreases with increasing water temperature [0].

[0] https://www.engineeringtoolbox.com/gases-solubility-water-d_...

CO2 solubility in H2O is inversely proportional to temperature but proportional to pressure. Even at 500 atmospheres (~5 km / ~15,000 ft depth), it's still not proportional to temperature. Whether a high-pressure environment precipitates out supercritical CO2 as a "solidish" hydrate or affects solubility is beyond my current laziness to look for. I would guess supercritical CO2 has a density higher than the densest water, but that's only a guess. (Paging Thunderf00t, CodysLab or NileRed to make a video.)

https://pubs.acs.org/doi/pdf/10.1021/ja01861a033

EDIT: I didn't see any replies before commenting, so "eventual consistency" of independent commenters likely led to what looks like piling-on. Sorry, that's not the intention.

That is very incorrect. While heat helps dissolve ionic compounds like salt, it has the opposite effect for CO2.