The kidneys and lungs work together to help maintain the blood pH by affecting the components of buffers in the blood.
Equation: H+(aq) +HCO•3 (aq) H2CO3(aq) H2O(l) + CO2(g)
2) Buffers are used in enzymes; most enzymes have an optimum pH range of approximately 7. If the pH falls to either side of 7 it can impair or destroy the function and structure of the enzyme. According to the company ‘Patient Storm’ a new invention has discovered a method to stabilise an enzyme during freezing providing the enzyme in a zwitteronic buffer solution.
A zwitterionic composition is useful as a surface active agent in aqueous solutions. The buffer solution has the capacity to stabilise an enzyme, such as glocuse oxidase, in a liquid state whilst providing protection if the the end solution is frozen. The zwitterionic buffer can stabalise the activity of enzymes by preventing large pH shifts during freezing.
Water will freeze and ice crystals will grow in a typical buffer composition and as the temperature approaches the eutectic points of the salts that are present, the less soluble salts crystallise out of the solution first. This can cause massive changes in pH before the frozen solid is formed. The zwitterionic buffer may prevent the shift in pH, maintain the acitvity and stabilise the enzyme.
3) Saliva in the mouth has a buffering capacity, as the pH of the mouth must be kept near neutral for things such as tooth maintenance. The oral pH is buffered to a small extent by saliva proteins and phosphate.
Buffers neutralises acids in the mouth based on systems such as the phosphate system and the carbonic acid/ bicarbonate system. A very important buffer is bicarbonate in solution neutralising the acids in the mouth.
Equation: CO2 + H2O ← H2CO3 ← HCO•3 + H+
Bicarbonate concentration increases in saliva as the flow rate rises because of the increased metabolic rate. This then raises the pH of saliva, so that it is more alkaline. Bicarbonate ions diffuse and neutralise the acid produced by plaque bacteria.
If saliva is not stimulated, the concentration of inorganic phosphate is high whilst the concentration of carbonic acid/bicarbonate system is low. But if saliva is stimulated the acid/bicarbonate system is the most important buffer as it has a higher concentration. Bicarbonate ions maintain the pH of saliva above 6.3.
4) Soil is a significant element in finding out how much acid deposition affects lakes, forests watercourses. Soil can be tested by the use of a pH meter to see id acidic or alkali. The pH of the soil is important to the health of vegetation and soil microorganisms as it determines the availability of nutrients to plants. Soil is considered to be acidic if it has a high concentration of hydrogen ions and considered to be basic if it has a low concentration of hydrogen ions. Acid soils are distinguished by the lack of soluble salts and an acidic reaction. If the content of salt is low the ionic strengths in the solutions will be low. Soil rich and deep in limestone and calcium carbonate have a neutralising capacity to neutralise acids directly in water, acting as a buffer. Buffers are useful to farmers to alter the pH of the soil in order to grow selected crops.
Soil Buffering Reactions in Relation to Soil pH (lawr.ucdavis.edu)
The pH range of important soil buffers:
10 - 14 OH- from water and oxides of Ca, Mg, Na, and K
10 - 6.5 Carbonates ƒ (solubility of the carbonate)
All Mineral weathering
10 - 3 Soil organic matter
4 - up Exchange reactions
4.2- 2.8 Aluminum oxides and hydroxides
3.8 - 2.4 Iron hydroxides and oxides
< 3 H+ from water
5) Acid rain is a form of precipitation formed from air pollutants such as sulphur dioxide and nitrogen oxides, which are released as gasses into the atmosphere. The gasses are from the burning of fossil fuels such as coal etc. the gasses combine with moisture in the air to form sulphuric and nitric acid solutions that fall to the earth.
The effect of acid precipitation can have devastating effects on aquatic animals and vegetation. A healthy lake has a pH value of 8, which is slightly basic which is maintained by the presence of buffering solutions in the water. The buffering chemicals in a lake provide an indication to the types of rocks, soils and minerals in the surrounding area. Providing buffering materials can be obtained from the rocks, soils and minerals the alkalinity levels may be restored to normal.
BIBLIOGRAPHY
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