What are the effects of a high or low pH level on freshwater ecosystems?
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At higher or lower pH levels, Dissolved oxyegn (DO) level can be changed and start redox reactions that may lose DO in the water.
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Absolutely not. But there have been cases where subtherapeutic levels of fluoride have been added to the water, too little to do any good. Happened in my town.
1159169
The pH of distilled water is lower than we expect, because the CO2 from atmosphere dissolves in it, to form an acidic compound. These are the reactions that take place:\nCO2 + H2O ----------> H2CO3\nH2CO3 + H2O ----------> HCO3- + H3O+\nHCO3- + H2O ----------> CO3 2-  + H3O+\nThe ions H3O+ give an acidic character to the distilled water
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water food oxygen environment
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Lack of nutrients like dissolved nitrates prevent algae and plankton that feed on the algae from growing. Thus, clear water.\n\nLack of sediments carried from large land masses, and lack of dust falling from air that has been moving over large land masses also contribute to the clarity of that water.
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plants use N, K and P to live. the more phosphorus(phosphate) in the water the more plants it can support. the more plants the less oxygen for fish.\nso high phosphate levels can cause low oxygen levels.
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1) Bi carbonate buffer system will contain HCO3- ion\n\nwhen a base is added it will liberate the H+ and produce water combining with OH- ion of the base there for reducing the effect of the base\n\nand when an acid is added it will accept the H+ ion and for H2CO3 therefor the effect of the acid will be nullified!!!\n\n2)phosphates are H2O4- or HPO42-\n\nand it will also have the functions as mentioned in the above!!\n\n3)proteins have an NH2 group and well as a COOH group both attached to the same molecule!!!\n\ntherefor when acid is added the NH2 group will neutralize it\n\nand when a base is added COOH group will neutralize it  reducing the alkalinity!\n\nthere for all these chemicals found in the blood and other body tissue will maintain the blood pH level at a constant level acting as natural buffers!!\n\nhope you understood!!!!!\n\ncheers!!
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Water... its got a pH=7
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yes there are certain chemicals that when placed in a bay can effect salinity levels in that bay, which will actually vary the temperature of the water causing native fish and sea life to leave.
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It's not C.  An increase in pH makes a solution more alkaline, meaning less H+ in the fluids.\n\nI'm going to say A here because a rise in pH is associated with increased O2 binding to hemoglobin.
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Invite a bunch of kids into your hottub, they should raise the PH level! jk\n\n"sodium bicarbonate or baking soda raises the kH and pH as mentioned by Goldy. As mentioned, at low pH, the good bugs do not thrive well and the filtration suffers. A pH level between 7.0 to 8.0 would be good. pH should not be raised suddenly to prevent pH shock. Therefore baking soda should be added little by little over a few days. A dosage of 25-50g per 1000L per day until the desired pH is achieved should be OK. As it is easily soluble in water, dissolve it in a pail of water and distribute evenly over the pond. It may need to be replenished after sometime depending on the stocking level as it is being used up by the filter. A more permanent solution of maintaining alkaline pH is to use shells (oyster, cockle) as pH buffers. They act by releasing carbonates slowly. \nIf the ammonia level in the pond is very low, there shouldn't be much danger in raising the pH slightly. As for the location of the UV, I would prefer to place it at the last stage of filtration, that is after the biomedia, and in a separate chamber."
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Nothing.  Except have a lower water volume due to warmer water molecules converting to gas.  However, the warmer water may have an efffect on the plants you are studying.  If you water a plant with hot water it may kill the plant.
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NaCl is the salt of a strong acid and a strong base. So when put in water it does not disturb the pH. On the other hand if you put the salt of a strong base and weak acid(CH3COONa for eg) the pH would increase and if you put a salt of weak base and strong acid(NH4Cl) pH would decrease, due to anionic and cationic hydrolysis respectively.
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Fresh water evaporates faster than the solutions will.  Between the solutions it would depend on the number of particles dissolved in the water.
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Ph is A measure of the acidity or alkalinity of a solution, numerically equal to 7 for neutral solutions, increasing with increasing alkalinity and decreasing with increasing acidity. The pH scale commonly in use ranges from 0 to 14.
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each of these are salts.  A high salt level is a deterant to microbial growth, basically all the water inside the microbial cell wants to rush out into the salt to equilibrize concentrations.  Basically that kills the cell.   There are some bacteria however that are halophiles (salt-loving) that can live in high salt concentrations, most of those however exist in nature in very harsh environments such as sea basins which have dried and left a large amount of salt in the surrounding soil
111444
Do you mean pH?  It is a term stating the concentration of Hydronium Ions H+ in a solution.  Water, when broken apart, can become H+ and OH- (hydroxide).  For example, when hydrogen chloride is mixed in water, the HCL breaks down into H+ (hydronium) and CL- (chloride ion).  That's what makes hydrochloric acid.  When there are high concentrations of H+ the pH number goes down.  Water (filled with hydronium) with a pH of 1 is highly acidic.  Water with a pH of 14 is highly basic (filled with hydroxide).  Household vinegar is probably around pH6.  Chlorox is basic, and is higher than pH7.  Things like alcohohl and gasoline, while volitile, are non-polar, and have few or no hydronium or hydroxide ions, so the pH would be neutral.  See the website describing ion concentration as a ratio of molecular elements logarithmically (powers of 10).