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04-26-2008, 04:42 AM
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In Remembrance
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you need to restore your pH
here is a link -on ph that is good http://www.answers.com/topic/ph?cat=technology also known as acid base homeostasis http://www.answers.com/topic/acid-ba...s-1?cat=health only part of the info -yet important part Non-volatile acids. When a healthy person exercises maximally, the exercising muscles cannot obtain all the energy that they need by aerobic metabolism (using oxygen) and must in addition metabolize anaerobically (i.e. without oxygen). This results in the breakdown of glucose to lactic acid, via a series of chemical reactions that release energy but do not require oxygen. This is a normal physiological situation in which excess non-volatile acid is released into the body fluids. The excess acid is subsequently taken up from the blood by the liver where most of the lactic acid is reconverted to glucose. Hydrogen ions are produced as an end product of the oxidation of sulphur-containing amino acids derived from proteins in the diet; this yields sulphuric acid. The metabolism of phospholipids, nucleic acids, and other phosphorus-containing chemicals yields phosphoric acid. Certain organic acids are formed during the metabolism of carbohydrates and fats; normally these acids are further oxidized to carbon dioxide and water, but in certain circumstances they may accumulate. A pathological example is diabetes mellitus, which has been called ‘starvation in the presence of plenty’. Here, although the concentration of glucose in the blood is high, the tissues are unable to metabolize it properly. Instead of using glucose, the body derives energy from excessive breakdown of lipids to yield so-called ketone bodies, including aceto-acetic and β-hydroxy-butyric acids. An excess of these fixed acids accumulates in the body. Surplus alkali accumulates when a person persistently vomits gastric contents. Acid is secreted into the gastric contents by cells in the wall of the stomach as part of the digestive process. This secretion of acid is accompanied by an equal movement of alkali from the acid-secreting cells in the opposite direction into the body fluids, so loss of acid in vomitus results in a surplus of alkali in the body. Defence of hydrogen ion concentration. The body has several lines of defence to accommodate surplus acid or base. The extracellular fluid, the contents of the cells, and bone all provide chemical buffering. A buffer is a system of chemicals that combines with an excess of hydrogen ions or hydroxide ions. Buffering therefore tends to stabilize the hydrogen ion concentration. It minimizes changes but does not alter the total acid or base load in the body. The final disposal of surplus fixed acid or base may be via metabolic pathways in the body, as described for lactic acid in the healthy exercising person. If such mechanisms are not available, then the excess acid or base must be expelled from the body, via the lungs and kidneys — the homeostatic processes of respiratory compensation and renal compensation. Respiratory compensation. The aeration of the lungs influences the hydrogen ion concentration of the blood by regulating the amount of carbon dioxide expelled from the body into the atmosphere. Other things being equal, an increase in the volume of air breathed in and out leads to a washing-out of carbon dioxide from the body, and hence a lowering of the hydrogen ion concentration of the body. In reaction 2, the concentration of carbon dioxide falls so the reaction is driven to the left, with a reduction in the number of hydrogen ions in the body. Conversely, a reduction of breathing results in a rise in hydrogen ion concentration in the body. In a healthy person, the concentration of carbon dioxide in the arterial blood is usually held constant by appropriate aeration of the lungs. The depth and rate of breathing are controlled by special centres in the brain, which influence the nerves that cause contraction and relaxation of the muscles of respiration. In a person with a surplus of fixed acid in the body, such as in maximal muscular exercise or in uncontrolled diabetes mellitus, the shift towards acidity (detected by chemoreceptors — specialized sensory structures) stimulates breathing. As a result, the concentration of carbon dioxide falls below normal. This in effect removes some of the excess hydrogen ions. In this way breathing can help to bring the hydrogen ion concentration back towards normal, despite the excess of fixed acid in the body. This is respiratory compensation. Renal compensation. Whereas the lungs regulate the amount of volatile acid (carbon dioxide) in the body, the kidneys regulate other acids and bases by excreting acidic or alkaline urine. In healthy people on a mixed diet, although the food itself is neutral, its metabolism releases an excess of non-volatile acid, and the kidneys must match this by excreting acidic urine as a normal necessity. The food of vegetarians yields an excess of base and the urine of healthy vegetarians is alkaline. In patients with renal damage the contribution of the kidneys is compromised; a feature of renal failure, in a person on a mixed diet, is an accumulation of acid in the body. The hydrogen ion concentration in aqueous solutions One way of expressing the concentration of a substance is in moles of the substance per litre of solution. A mole of a substance is its molecular weight in grams. For hydrogen ions, the concentration is conventionally described as a pH value: the pH is the negative logarithm of the hydrogen ion concentration expressed in moles per litre. As the hydrogen ion concentration of a solution becomes higher, its pH becomes lower — more acidic. In a neutral solution at a temperature of 25°C, the hydrogen ion concentration is 10-7 moles per litre, or 100 nanomoles/litre (1 nanomole = 10-9 mole). This corresponds to a pH value of 7.0. In a neutral solution at 37°C, the hydrogen ion concentration is 157 nanomoles/litre. In the arterial blood plasma of a normal person at rest, the hydrogen ion concentration usually lies in the range 35 to 45 nanomoles/litre, with an average of 40. The hydrogen ion concentration of plasma is therefore normally about a quarter of that for a neutral solution at body temperature. A rise in plasma hydrogen ion concentration towards that of a neutral solution will result in death in most people. By contrast, the hydrogen ion concentration of the intracellular fluid is normally close to that of a neutral solution. The range of hydrogen ion concentration in disease In persons with acid-base disorders, hydrogen ion concentration may be as low as 20 or as high as 80 nanomoles/litre, this being the usually tolerable range for survival. Thus a 4-fold range is compatible with life. This is a much larger variation than the range tolerated for certain other chemicals, for instance sodium ions, chloride ions, and water itself. For short periods of time, it is possible for the hydrogen ion concentration to go beyond these limits, particularly on the acid side. Enzymes and hydrogen ion concentration. Ultimately the regulation of hydrogen ion concentration is important in keeping conditions ideal for the biological catalysts, enzymes. These enzymes are essential for the chemical processes of life, both inside cells and in the extracellular fluids. Enzymes consist of complex protein molecules: there are sites on these molecules that attract and release hydrogen ions. Enzymic activity depends on the molecule being in the correct state of ionization; if an enzyme is associated with an excess of hydrogen ions or has lost many hydrogen ions, its enzymic activity is reduced or abolished. This is why enzymes operate optimally at a given hydrogen ion concentration. Enzymes on the surfaces of cells, which are bathed in extracellular fluid, operate optimally at the hydrogen ion concentration of extracellular fluid. Intracellular enzymes operate optimally at the hydrogen ion concentration of intracellular fluid. Effects of disturbances of hydrogen ion concentration. In disease states, deviation from normal hydrogen ion concentration usually occurs in association with other serious pathological processes, and it may be difficult to specify the effects of altered hydrogen ion concentration alone. With a high hydrogen ion concentration, there is a widespread relaxation of smooth muscle, including the muscle in the walls of blood vessels: this results in a severe drop in arterial blood pressure, with circulatory collapse. When elevation of hydrogen ion concentration is prolonged, minerals are leached from bones, causing them to become weak mechanically; the condition of osteoporosis. A low hydrogen ion concentration occurs as a result of overbreathing, in which carbon dioxide is blown off excessively in the lungs. The condition occurs in certain otherwise normal people who overbreathe as a reaction to stress. A reduction in hydrogen ion concentration unveils sites on protein molecules that attract positive ions. Other positive ions then tend to attach to these binding sites instead of hydrogen ions. An ion of importance in this respect is calcium; a lowering of hydrogen ions leads to a lowering of the concentration in the body fluids of calcium ions, the condition of hypocalcaemia. This leads to an increase in the excitability of nerve fibres, resulting in the occurrence of spontaneous action potentials. These cause hypocalcaemic tetany — involuntary uncoordinated contractions of skeletal muscles — bizarre subjective sensations, and numbness. The balance of hydrogen and hydroxide ions influences our bodily functions out of all proportion to the minute concentrations of these ions in biological fluids. The adverse effects arising from disturbances of hydrogen ion concentration are due to interference with the normal harmonious interaction of the many thousands of enzymes on which life depends. — Oliver Holmes Bibliography Holmes, O. (1993). Human acid-base physiology. Chapman and Hall Medical, London See also body fluids; carbon dioxide; enzymes; homeostasis; hyperventilation; kidneys; respiration. __________________ you need to alkalize -after vomiting your blood acid maybe to high - soon you should stabolize -but = you need to drink water /good water your electrolytes are low as well -when you buy ph litmus paper to chck your acidity- when you are abit more green blue or blue on litmus test - of which you may put on your tongue ,or urinate on . briefly wetting the paper -when you read it within the minute it is wet yet doesnt change color anymore and before the litmus paper dries when balance is found ~ it will also boost your immune system... http://www.answers.com/alkalize http://www.answers.com/topic/electrolyte?cat=technology partial info Food & Culture Encyclopedia: Electrolytes Electrolytes are molecules that, in solution, dissociate into positively charged ions (cations) and negatively charged ions (anions). Principal ions in body fluids are sodium, potassium, and chloride. A 70 kg adult has a body content of approximately 100 g sodium, 140 g potassium, and 95 g chloride. To maintain a stable body content, the amount of principal ions lost must equal the amount consumed. During growth and during pregnancy, the amount accreted for tissue formation also must be considered. Physiological Functions Sodium is the predominant cation in fluids outside the cells (extracellular fluid), whereas potassium is the predominant cation in the intracellular fluid. Chloride is the major anion of the extracellular fluid. Sodium plays a central role in regulating body fluid balance and distribution of fluid between the extracellular and intracellular compartments. As sodium is the major osmotically active particle in the extracellular fluid, sodium and its accompanying anion determines the osmolar concentration, or osmolarity, of this compartment. An increase in sodium concentration will increase the osmolarity of the extracellular fluid, thus causing water to move out of the cells into the extracellular compartment. It will also cause water retention by stimulating the thirst mechanism and by decreasing urine flow. The opposite occurs when sodium concentration is decreased. Thus, sodium plays a central role in regulating body fluid balance and the distribution of fluid between the extracellular and intracellular compartments. Potassium is necessary for normal growth and plays an important function in cell metabolism, enzyme reactions, and synthesis of muscle protein. Both sodium and potassium are involved in maintaining proper acidity (pH) of the blood and in maintaining nerve and muscle functions. Normal resting membrane potentials of nerve and muscle cells range between –50 and 100 mV, with the inside of the cells negative with respect to the outside. These resting membrane potentials are maintained by the chemical gradient of potassium across cell membranes. Activation of excitable cells alters their membrane permeabilities to sodium and potassium, leading to changes in their membrane potentials. A weak stimulus causes a small depolarization (the inside of the cell is made less negative) as a result of sodium influx along its electrochemical gradient via the voltage-gated sodium channels in cell membranes. This is followed by repolarization, which is a manifestation of potassium efflux. If the stimulus is sufficiently strong, large changes in the membrane potential occur, during which the membrane potential may change from –70 mV to +30 mV, and then repolarize back to its resting membrane potential. This action potential, cause by alternation of potassium steady-state potentials with pulsed sodium potentials, gives rise to a traveling wave of depolarization that is conducted along the nerve fiber to exert an effect on the effector cells it innervates (supplies with nerves). In muscles, action potential leads to muscle contraction. Dietary sodium chloride in foods and beverages is absorbed mostly in the small intestine. Active transport of sodium out of the small intestinal epithelial cells across their basolateral membrane provides an electrochemical gradient for the absorption of sodium across the luminal membrane. Entry of sodium through carrier proteins can either transport other solutes against their concentration gradient in the same direction (co-transport) or in an opposite direction (counter-transport). A number of transporters have receptor sites for binding sodium and glucose, galactose, or amino acids. Therefore, entry of sodium across the luminal membrane also brings in a solute. Counter-transport mechanisms operating in the kidneys allow excess hydrogen and potassium to be excreted in the urine. Consumption of Sodium, Chloride, and Potassium Consumption usually exceeds the needs of an individual, although the amount consumed varies widely with dietary habits. Most natural foods contain high potassium content but are lower in sodium content (Table 1). American adults consume an average of 2.5 to 3.5 g of potassium daily. Individuals consuming large amounts of fruits and vegetables may have a daily intake of as high as 11 g. Sodium is consumed mainly as sodium chloride (table salt). A small amount is consumed as sodium carbonate, sodium citrate, and sodium glutamate. Intakes of sodium vary, averaging 2 to 5 g/day of sodium or 5 to 13 g/day of sodium chloride. Only about 10 percent of sodium intake is from natural foods, the rest from sodium salts added during cooking and at the table, and from salts added during processing of foods. In regions where consumption of salt-preserved foods is customary, intake of sodium can be as high as 14 to 20 g/day. Under normal circumstances, about 99 percent of dietary sodium, chloride, and potassium is absorbed. Absorption occurs along the entire length of the intestine, the largest fraction being absorbed in the small intestine and the remaining 5 to 10 percent in the colon. Potassium is also secreted in the colon. Various homeostatic regulatory mechanisms, the most important of which is aldosterone, modulate the absorption of sodium and secretion of potassium. Loss of Sodium, Chloride, and Potassium Obligatory loss of fluids through skin, urine, and feces invariably causes loss of these ions. Minimal obligatory loss for an adult consuming average intakes has been estimated to be 115 mg/day for sodium and 800 mg/day for potassium. Over 95 percent of loss is in the urine. Under most circumstances, loss of chloride parallels that of sodium. Loss of these ions can increase greatly in diuresis, vomiting, and diarrhea. Loss of sodium chloride can also increase greatly from profuse sweating. Recommended Intake. Daily minimum needs can be estimated from the amount required to replace obligatory (Table 2). The need is increased in infants and children, and during pregnancy and lactation. Estimated safe minimum intake levels are higher than the minimum requirements to account for the various degrees of physical activity of individuals and environmental conditions. Average intakes in the United States are higher than the estimated safe minimum levels of sodium chloride (1.3 g/day) and potassium (2 g/day). return to link - http://www.answers.com/litmus?cat=technology and the last link is important http://books.google.com/books?id=vue...Pi0195Fw&hl=en ps -dear howard - remove red meat etc. as much as you can out of your diet -our meat idustry is vile -*yuckie instead supplement with MB-12 luv 
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with much love, lou_lou . . by . , on Flickr pd documentary - part 2 and 3 . . Resolve to be tender with the young, compassionate with the aged, sympathetic with the striving, and tolerant with the weak and the wrong. Sometime in your life you will have been all of these. Last edited by lou_lou; 04-26-2008 at 05:41 AM. |
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| "Thanks for this!" says: | Howardh (04-26-2008) |
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