How CO2 stripping cause raise in pH in water treatment?
441451
Well, there's a decomposition reaction.\n\nH2CO3 <--> H2O + CO2\n\nCarbonic acid (H2CO3) doesn't not exist much at all, because it decomposes into H2O and CO2. But some of the carbonic acid remains, pushing up the hydronium concentration, which by definition makes water more acidic. Therefore, getting rid of the CO2 in water makes water less acidic (raising the pH).
332502
Yeah, I've actually done this reaction before several times. \n\nTheoretically, this is a metathesis reaction, also called a double-replacement reaction.  Essentially, the ions switch partners.  \n\nCaCO3 + 2HCl ---> CaCl2 + H2CO3\n\nNow, the CaCl2 is a soluble salt, so that's actually just like ions floating around in solution. \nThe H2CO3 is carbonic acid, which is actually just carbon dioxide, CO2, dissolved in water.  The carbon dioxide will immediately come out of solution and bubble out, which is totally observable, just like putting baking soda and vinegar together.  \n\nThe more complete reaction full ionic equation is the following:\nCaCO3 + 2H+ + 2Cl- ---> Ca2+ + 2Cl- + H2O + CO2
1181487
True the higher the pH the lower the concentrations
549228
A rythmic expulsion of carbon dioxide which aids in maintaining the proper pH balance in the bloodstream in order to maintain life.
644041
2.\nBy decreasing the temperature and increasing the pressure. As ussually done in Haber;s process\nAnother way is to keep on removing the ammmonia gas to make reaction go forward\nRead th Le Chatelier's principle for more detail.\n\n13.\n2 HCl + Na2CO3  -----> 2 NaCl + H2CO3\nH2Co3 can exist as water and carbon dioxide.\n\n14.\nBecause acid-base reaction is spontaneous.\n\n11.\nBecause of the formation of copper(II) carbonate which will settle down as precipitate.
835624
CO2. and you can also use vinegar.
829097
i agree with science teacher CO2 is covalently bonded\nthe minerals in the plants water system is dissovled are ions of an aqeous solution. these are (or were formorly) ionic bonded
508304
slightly acidic... that's why the add lime when disinfecting the water.  the addition of lime raises the pH a bit which buffers the natural acidity of the water to help prevent lead and copper leaching from residential plumbing.  the lime helps minimize corrosivity, and if it does that and since acids are corrosive, when they disinfect the water they are making it nuetral by adding a weak base.
169963
Actually, that is a somewhat simplified reaction,\nin reality, the water and Carbon Dioxide dont form directly, they form after a secondary reaction (Carbonic acid decomposing).\n\n3Na2CO3 + 2H3PO4 --> 2Na3PO4 + 3H2CO3\nH2CO3 --> H2O + CO2\n\nSo combining them,\n3Na2CO3 + 2H3PO4 --> 2Na3PO4 + 3H2O + 3CO2
952998
The reductive dissolution of goethite ( -FeOOH) and hematite ( -Fe 2 O 3 ) by phenolic reductants has been examined in order to improve the understanding of iron transformations in soils, sediments and aquifers. Rates of goethite reductive dissolution by hydroquinone increased as the pH was increased from pH 1.8 to 4.65, arid the following reaction stoichiometry was obeyed: 2 - FeOOH + QH 2 = 2 Fe 2+ + Q + 4 OH - . As the pH was increased from pH 4.5 to 6.0, the reductive dissolution rate decreased to below the detection limit. At pH 3.4, the reductive dissolution of hematite was two orders of magnitude slower than goethite. The relationship between structure and reactivity was examined for a series of mono-, di-, and tri-hydroxybenzene reductants. Rates of reductive dissolution decreased in the following order: catechol ~- hydroquinone 〉 3,4-dihydroxybenzoic acid 〉 resorcinol-phenol-4-hydroxybenzoic acid.
701387
the conversion of water (H2O) and Carbon dioxide (CO2) into Glucose((C6H12O6) and oxygen(O2)\n\n             H2O+CO2 -----> C6H12O6 +O2
580198
Alkalinity gets into water as the presence of the OH- ions increase. Remember that Water has a pH of 7... so its equality semi-acidic (as it can have the H ions donating electrons), or semi-basic (as it can accept the electrons). As the OH- ions increases, the mixture has a greater tendency of wanting electrons to keep it stable. The greater affinity / presence of OH- ions, the more basic or alkaline the water becomes.\n(Hope that was of help).
613273
Excess of CO2 along with water forms carbonic acid. the reaction goes this way.\n\nCO2+H2O-H2CO3
318669
The obvious answer "by destillation" is technically challenging. I know of a Danish firm EnvoTech ApS that built systems which concentrate problematic waste water by cyclical destillation with very little energy loss,  which would help concentrate the remaining acid, but only up to a degree where the stainless steel the system is built from begins to corrode, and without removing the discoloration. You'd get quite good water condensate to reuse in the process, which isn't that helpful for your problem...\n\nThe foamy particles might be removable by letting the water go through a flotation trough. The resulting acid will still be weak and brown, though.
282642
actually, pure water does not have a pH of 7.0, it is slightly acidic, around 5.6-5.8 from what i have seen at work.
539761
It because fish produce ammonia which dissolves to form ammonia solution. The ammonia solution is basic thus it increases the pH of water in the aquarium.
804094
dissociation of co2 in water produces produces an acid proton:\n\nCO2 + H2O ⇌ HCO3− + H+\n\nKa = 4.30×10−7 mol/L; pKa = 6.36. \n\nwithout knowing the amount of CO2 or water you used, it is impossible to calculate the pH.\n\nassuming its a 0.1M solution (0.1mol of CO2 dissolved in 1dm³ of water), pH would be around 3.7, whereas strong acids would hit pH 0 at far lower concentrations.