2:53 I wouldn't say it really mitigates our impact. The acidification of the ocean is a separate environmental issue to deal with, and the only benefit is ~30% atmospheric CO2, not a very big dent. Would probably be better to have it all in the atmosphere.
I am not quite sure what you are asking. Most tests measure total alkalinity by titrating to a set pH using a strong acid. The amount of each ion present (bicarbonate and carbonate) can then be determined based on the original pH of the solution.
You forgot the NaH(CO3) which makes the water basic when dissolved in water. (Na+aq)... H(CO3) + H20 H2(CO3) + OH-. Therefore it makes sea water alkaline. What matters is the K value of each equation to give the final pH. So what your saying is wrong about the ocean or at least not the bigger picture. And corals use (CO3) to forum their calcium skeleton Ca(CO3). Therefore CO2 in the water is ultimately good for corals.
It is more difficult to generalize about freshwater because it is much more variable. It depends on the composition of the surrounding rock and soil and the ratio between precipitation and evaporation. In general, the same major ions (Ca, Na, Mg, K, HCO, SO4, and Cl) in saltwater also dominate in freshwater, albeit at lower concentrations and with more variability across water bodies.
Thank you for your comment. The carbonate ppt chemistry is over simplified in the diagram. It also does not address how the ppt of CaCO3 results in the formation of CO2. That is something I plan to address in another video.
1:50 I'm still confused about this. It is said CO2 combines with H2O to form H2CO3 which can let loose of 2 hydrogen atoms for 2H+ and CO3 but can then recombine with one of the hydrogen atoms easier than combining with calcium. Why? Nature's creatures have always been forming CaCO3 instead, calcium carbonate. What changed?
Basically what matters here is that by adding H2CO3 to the ocean you lower it's pH, in other words you have more free H+, since you have more of those it makes it more likely for CO3 to combine with one of those to form HCO3 than before. So you decrease the amount of CO3. However in order to have solid CaCO3 (seashells) in water you need to have so much CO3 and Ca that it can't be dissolved anymore (like adding too much salt or sugar to water it won't dissolve at some point if you add too much). But since you are decreasing the amount of CO3 in the water by transforming it to HCO3 then there's now possibility for more CO3 to become soluble, so shells dissolve until solubility is reached. That's why CO2 going into the ocean dissolves carbonate based shells.
Part of the picture is studied by scientists and reported on by IPCC but not well known publicly. Can be googled with ... ocean slowing. 2013: "The oceans as a whole have a large capacity for absorbing CO2, but ocean mixing is too slow to have spread this additional CO2 deep into the ocean. As a result, ocean waters deeper than 500 meters (about 1,600 feet) have a large but still unrealized absorption capacity, said Scripps geochemist Ralph Keeling" 2015: Atlantic Meridional Overturning Circulation "(AMOC) has weakened by 15-20% in 200 years (UCM) 2019: CO2 levels [in the air] rise when Atlantic Circulation is weak and fall when it’s strong (EOS)
i'm not good with chemistry but this video made buffering really easy for me to understand, i think i'll do better on my final now, thank you!
Glad the video helped. Good luck on your exam.
2:53 I wouldn't say it really mitigates our impact. The acidification of the ocean is a separate environmental issue to deal with, and the only benefit is ~30% atmospheric CO2, not a very big dent. Would probably be better to have it all in the atmosphere.
Similar bicarbonate buffering reactions in blood to maintain pH within narrow range.
bicarbonate "can be both an acid and a base depending on what it is reacting with"
Really helpful, thanks!
Glad it was helpful!
Thanks sir ❤
Thanks for the video
You are welcome. Glad you found it useful. Thanks for commenting.
@@SciencePrimer I also like video!!!! Thanks for uploading a nice video!!
at what pH each reaction is triggered since all reactions look to be reversible, which would be the spontaneous reactions at which pH. please help
Question : for Alkalinity, which one is better ? Bicabonate or Carbonate ?
I am not quite sure what you are asking. Most tests measure total alkalinity by titrating to a set pH using a strong acid. The amount of each ion present (bicarbonate and carbonate) can then be determined based on the original pH of the solution.
You forgot the NaH(CO3) which makes the water basic when dissolved in water.
(Na+aq)... H(CO3) + H20 H2(CO3) + OH-. Therefore it makes sea water alkaline. What matters is the K value of each equation to give the final pH. So what your saying is wrong about the ocean or at least not the bigger picture. And corals use (CO3) to forum their calcium skeleton Ca(CO3). Therefore CO2 in the water is ultimately good for corals.
What is the most abundant ion in natural freshwater?
It is more difficult to generalize about freshwater because it is much more variable. It depends on the composition of the surrounding rock and soil and the ratio between precipitation and evaporation. In general, the same major ions (Ca, Na, Mg, K, HCO, SO4, and Cl) in saltwater also dominate in freshwater, albeit at lower concentrations and with more variability across water bodies.
I want to mention a point, that CaCO3 is produced by Ca2+ and HCO32-, not from CO32-.
Hope your video becomes better and better.
Thank you for your comment. The carbonate ppt chemistry is over simplified in the diagram. It also does not address how the ppt of CaCO3 results in the formation of CO2. That is something I plan to address in another video.
1:50 I'm still confused about this. It is said CO2 combines with H2O to form H2CO3 which can let loose of 2 hydrogen atoms for 2H+ and CO3 but can then recombine with one of the hydrogen atoms easier than combining with calcium. Why? Nature's creatures have always been forming CaCO3 instead, calcium carbonate. What changed?
Basically what matters here is that by adding H2CO3 to the ocean you lower it's pH, in other words you have more free H+, since you have more of those it makes it more likely for CO3 to combine with one of those to form HCO3 than before. So you decrease the amount of CO3. However in order to have solid CaCO3 (seashells) in water you need to have so much CO3 and Ca that it can't be dissolved anymore (like adding too much salt or sugar to water it won't dissolve at some point if you add too much). But since you are decreasing the amount of CO3 in the water by transforming it to HCO3 then there's now possibility for more CO3 to become soluble, so shells dissolve until solubility is reached. That's why CO2 going into the ocean dissolves carbonate based shells.
Part of the picture is studied by scientists and reported on by IPCC but not well known publicly. Can be googled with ... ocean slowing.
2013: "The oceans as a whole have a large capacity for absorbing CO2, but ocean mixing is too slow to have spread this additional CO2 deep into the ocean. As a result, ocean waters deeper than 500 meters (about 1,600 feet) have a large but still unrealized absorption capacity, said Scripps geochemist Ralph Keeling"
2015: Atlantic Meridional Overturning Circulation "(AMOC) has weakened by 15-20% in 200 years (UCM)
2019: CO2 levels [in the air] rise when Atlantic Circulation is weak and fall when it’s strong (EOS)