How does driftwood and peat moss effect the pH level of water?
927156
drift wood will lower pH as it releases tannic acid as it soaks.\n\npeat moss will have the same effect , but will release humic acids.
901202
Buffers are used to regulate pH in living things. Since living things are water-based, they need to keep a constant pH to make their enzymes perform at the proper level. \n\nI attached a link to a really good description of why and how this happens
1104733
BOTH lowering of ph in lakes or removing mineral.\n\n http://healthandenergy.com/acid_rain.htm
966389
Because it is quite a mild solution. There's plenty more water than acid, therefore you may assume that the properties of the water haven't changed much.
1180992
depends on the strength of the base actually.  water is amphoteric which means it can act like an acid or a base.  if a weak base is put in water the water can neutralize it, but water is quickly overrun yielding the below equation.\n\nB + H2O yields HO- +BH\n\nthis makes the water basic.
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Urine pH as measured by urinalysis has a normal range of about 4.5-8 with a pH of 6 being the average. Neutral pH is 7. Anything having a lower pH is acidic and anything with a higher pH is basic. \nUrine is actually a fairly good growth medium for bacteria and is sometimes used in labs for this pupose. However urine with a lower pH (more acidic) has been found to inhibit the growth of bacteria. \nUrine that is high in ammonia on the other hand with its higher pH (more alkaline or basic) has been found to impede the bodies immune responce to a UTI. In fact Proteus species of bacteria which is a common cause of UTIs produces a substance called urease which breaks down uric acid (an end product of nitrogen metabolism found in urine) into ammonia and carbon dioxide, thus causing the urine to become more basic. The ability of Proteus of produce urease increases its ability to cause pylonephritis (infection of the kidney as opposed to the blatter or ureters).\nTaking substances that will alter the pH of your urine however may have unforseen side effects. The pH of the urine helps determine what is and what is not filtered out of the blood by the kidney. Also altering the pH will have an effect of the formation of kidney stones. Certain particles will become "un-dissolved" at a higher pH and some at a lower pH. If enough of the particles come out of solution, you will get kidney stones. In fact the Proteus bacteria that cause the urine to become more basic are associated with an increase in kidney stones.\nI general however pH has very little to do with get or not getting a UTI. The urinary tract from the distal urethra up is mostly sterile and the few bacteria that do get into the urinary tract are usually flushed out when you urinate. Some bacteria however such as E. coli have molecules on thier outer membrane that can adhere to the urinary tract lining. It can do this reguardless of pH and pH in general has little effect on E. coli which is what causes about 85% of UTIs not contracted in a hospital. E. coli is found in the digestive tract and most UTIs are caused when the E. coli finds its way into the urinary tract. While in the digestive tract the E. coli has had to endure the extremely acidic pH of the stomach and the very basic pH of the small intestine.\nMost bacteria that cause UTIs are from the digestive tract. Often they are aided in migration to the urethra by sexual intercourse. The use of spermicides is associated with an increase in UTIs because the protective bacteria of the vagina are killed by the spermicide and this leave the vagina vulnerable to colinization by UTI causing bacteria.\nAlso some women are genetically predisposed to UTI because they have more adhesion molecules on their vaginal walls.\nCranberry juice is helpful in preventing UTI. Studies have shown that cranberry juice inhibits the ability of bacteria to adhere to the urinary tract.\nIf recurrent UTIs are a problem you may want to speak to you doctor about methanamine. It is used to prevent UTIs especially those caused by E. coli which is the most common cause of UTIs.
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Some plants thrive in a low pH-leveled soil (such as rhododendrons and azaleas), and other kinds of plants thrive in a high pH-leveled soil.  Give the plants the opposite of what they need, and they will mostly likely die.
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Alkalinity is usually measured by the presence of bicarbonate (HCO3-) and carbonates (CO3=) and acts to buffer water from acidic inputs, thus is a measure of the buffering capacity of water. Water with high alkalinity have high pH values while water with low alkalinity have low pH values. The hardness of the water is usually determined by the amount of calcium and magnesium salts present in water and is associated with the presence of carbonates. Hard water is generally more productive than soft water waters and can accept more input of salts, nutrients, and acids to their system without change than can soft water waters. So basically, it’s because of the presence of the magnesium. \n\nHope this helps and hope I didn’t confuse you.
313595
Water... its got a pH=7
1181487
True the higher the pH the lower the concentrations
318259
soil pH typically varies on a much smaller scale than country or climate zone.  Here in the Blue Ridge Mountains, some valleys have acid soil ("sour" to the old-school farmers who didn't have a meter fancier than their tongue) while over the next hill it may be "sweet," that is, neutral to basic.  Here it depends on the kind of rock under the soil.
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it depends on the properties of water extracted at that place,it could be any thing for obvious reasons.it depends on H+ ions..it depends on acidic property of soil, pollution, type of pollutio,wher that water is coming from like upstream properties.its hard to say.
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http://www.ebroadcast.com.au/lookup/encyclopedia/so/Soil_pH.html\n\nSoil pH\n\nSoil pH is an indication of the alkalinity or acidity of soil. It is based on the measurement of pH, which is based in turn on the concentration of hydrogen ions (H+) in a water or salt solution.\n\n\nWhen in balance (pH 7) the soil is said to be neutral. The pH scale covers a continuum ranging from 0 (very acidic) to 14 (very alkaline or basic). It is however uncommon to find soils at either extreme of this range. Under many conditions soils tend to become more acid or alkaline over time if steps are not taken to maintain a balance. \n\npH is important for the organic gardener for several reasons, including the fact that many plants and soil life forms prefer either acid or alkaline conditions, that some diseases tend to thrive when the soil is alkaline or acidic, and that the pH can affect the availability of nutrients in the soil. \n\nTable of contents [showhide]  \n1 Nutrient availability in relation to soil pH \n2 Soils and acidity \n3 Soil life and pH \n4 pH and plant diseases \n5 Determining pH \n6 Altering soil pH \n7 See also \n \n \n\n\n\nNutrient availability in relation to soil pH \nThe majority of food crops prefer a neutral or slightly acidic soil, because the solubility of most nutrients necessary for healthy plant growth is highest at at pH 6.3-6.8. Some plants however prefer more acidic (e.g., potatos, strawberries) or alkaline (brassicas) conditions. \n\nWhen the pH falls below 5.5, most major plant-nutrient minerals (those needed in substantial quantities to promote healthy plant growth include nitrogen (N), phosphorus (P), potassium (K), sulphur (S), magnesium (Mg), and calcium (Ca)) and some micronutrients[?] (elements important to plant growth in very small amounts) become insoluble and hence unavailable for uptake by plant roots. \n\nMany cationic (positively charged) nutrients such as zinc (Zn2+), aluminium (Al3+), iron (Fe2+), copper (Cu2+), cobalt (Co2+), and manganese (Mn2+) are soluble and available for uptake by plants below pH 5.0, although their availability can be excessive and thus toxic in more acidic conditions. In more alkaline conditions they are less available, and symptoms of nutrient defficiency may result, including thin plant stems, yellowing (chlorosis[?]) or mottling of leaves, and slow or stunted growth. \n\npH levels also affect the complex interactions among soil chemicals. Phosphorus (P) for example requires a pH between 6.0 and 7.0 and becomes chemically immobile outside this range, forming insoluble compounds with iron (Fe) and aluminium (Al) in acid soils and with calcium (Ca) in calcareous soils. \n\nThis table indicates the availability of several nutrients at various pH values: \n\n  Acid  Neutral Alkali  \n  4   4.5 5   5.5 6   6.5 7   7.5 8   8.5 9   9.5 10 \nnitrogen, N       \nphosphorus, P         \npotassium, K         \ncalcium, Ca       \nmagnesium, Mg       \nsulfur, S     \niron, Fe     \nmanganese, Mn       \nboron, B       \ncopper, Cu       \nzinc, Zn       \nmolybdenum, Mo     \n\n\n\nSoils and acidity \nUnder conditions in which rainfall exceeds evapotranspiration (leaching) during most of the year, the basic soil cations (Ca, Mg, K) are gradually depleted and replaced with cations helds in colloidal[?] soil reserves, leading to soil acidity. Clay soils often contain Fe and hydroxy Al, which affect the retention and availability of fertilizer cations and anions in acidic soils. \n\nSoil acidification may also occur by addition of hydrogen, due to decomposition of organic matter, acid-forming fertilisers, and exchange of basic cations for H+ by the roots. \n\nSoil acidity is reduced by volatilization and denitrification of nitrogen. Under flooded conditions, the soil pH value increases. In addition, nitrate fertilizers containing cations such as Ca, K, or Na also increase the soil pH value. \n\n\nSoil life and pH \nA pH level of around 6.3-6.8 is also the optimum range preferred by
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# Anoxic autotrophs: Obtain hydrogen from chemicals such as sulfur.\n[[[[[[[[[[[[[[[[[[[[[[[[[[[[[[[[[[Dead Zones are areas where the bottom water (the water at the sea floor) is anoxic, meaning that it has very low (or completely zero) concentrations of dissolved oxygen.]]]]]]]]]]]]]]]]]]]]]]]]]\nDead Zones are areas where the bottom water (the water at the sea floor) is anoxic, meaning that it has very low (or completely zero) concentrations of dissolved oxygen. These dead zones are occurring in many areas along the coasts of major continents, and they are spreading over larger areas of the sea floor. Because very few organisms can tolerate the lack of oxygen in these areas, they can destroy the habitat in which numerous organisms make their home.\n\nThe cause of anoxic bottom waters is fairly simple: the organic matter produced by phytoplankton at the surface of the ocean (in the euphotic zone) sinks to the bottom (the benthic zone) where it is subject to breakdown by the action of bacteria, a process known as bacterial respiration. The problem is, while phytoplankton use carbon dioxide and produce oxygen during photosynthesis, bacteria use oxygen and give off carbon dioxide during respiration. The oxygen used by bacteria is the oxygen dissolved in the water, and that’s the same oxygen that all of the other oxygen-respiring animals on the bottom (crabs, clams, shrimp, and a host of mud-loving creatures) and swimming in the water (zooplankton, fish) require for life to continue.\n\nThe "creeping dead zones" are areas in the ocean where it appears that phytoplankton productivity has been enhanced, or natural water flow has been restricted, leading to increasing bottom water anoxia. If phytoplankton productivity is enhanced, more organic matter is produced, more organic matter sinks to the bottom and is respired by bacteria, and thus more oxygen is consumed. If water flow is restricted, the natural refreshing flow of "oxic" waters (water with normal dissolved oxygen concentrations) is reduced, so that the remaining oxygen is depleted faster.\n\nMany of the areas where increasing bottom water anoxia has recently been observed are near the mouths of major river systems. While Satellite images can’t see the bottom of the ocean, they can see the surface, where sediments from rivers mix with ocean waters. The images shown here are Satellite images (SeaWiFS) observations of the Mississippi River delta, the Yangtze River mouth in China (The Yangtze River mouth is not currently identified as an area with an associated dead zone, but such conditions could develop there in the future), and the Pearl River mouth in China, near Hong Kong.\n\nSeaWiFS can also observe areas where water flow is restricted, such as the Baltic Sea in Europe. The image on the left features Denmark after strong storms caused flooding and increased sediment suspension in the Baltic. On the right is an overview of the Baltic Sea, including a plankton bloom in the Skagerrak just north of Denmark.\n\nThe apparent cause of the creeping dead zones is agriculture, specifically fertilizer. While fertilizer is necessary to foster bumper agricultural crops, it also runs off the fields into the streams and rivers of a watershed. When the fertilizer reaches the ocean, it just becomes more nutrients for the phytoplankton, so they do what they do best: they grow and multiply. Which leads to more organic matter reaching the bottom, more bacterial respiration, and more anoxic bottom water.\n\nThese effects can be magnified by catastrophe. When the heavy rains of Hurricane Floyd caused extensive flooding in North Carolina in September 1999, the heavy load of nutrients (from dead animals, flooded animal waste ponds, and numerous other sources) reached the sounds that lie between the coast and the Outer Banks, oxygen levels in the water plummeted. The picture at the top of the page shows the heavy load of sediments flowing into Pamlico Sound. SeaWiFS captur
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Because settling only works if there is no chemical reation involved. All of the prticals of some substances will not settle out of water. like sugar. Even if they do the time frame needed to accomplish this is to long.
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They change the pH of the environment of the mildew, which stresses the fungus and kills it, as it preferes an acidic environment.\n\nSodium bicarbonate is a base, not an acid, by the way, you must not pay attention to the answer above.\n\nCheck this study out:\nhttp://phytoparasitica.org/phyto/pdfs/1997/issue1/NOTE.pdf
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In 1909 a Danish biochemist, by the name of Sorenson, suggested reporting the concentration of H+ ion on a logarithmic scale, which he named the pH scale. Because of the magnitude of these concentrations it has become more convenient to give the acidity in terms of the pH, rather than as [H+]. pH is defined as; \npH = -log [H+] \nThe scale can be adjusted to include pH values at various [H+]. Now an acid can be defined as a substance which when added to water has a pH < 7.00 and base has a pH>7.00.