Question

The blood is a buffered system as its pH must be maintained very close to 7.35 if its oxygen carrying capacity is to maintained.

(1) Name the components of the buffer system in the blood

Answer 1

I think the ans is FeO

Answer 2

I did a project on this! I forgot thho

Answer 3

thnx anyway

Answer 4

The presence of buffers in the blood and other fluids in our body, is fundamental. This happens mainly because several biological processes that occur in our bodies, enzymes are present, as is well known that their action is influenced significantly by pH. The normal pH value of plasma human blood is between 7.35 -7.45. Small changes in pH value of the order of tenth of the unit can cause serious illness or even death. Acidosis occurs when the pH drops below the normal value as be 7.2. This may result from cardiac or renal failure, prolonged diarrhea or even an exhaustive exercise, etc. This means that the patient falling into a coma. In other words, this little change in pH, which corresponds to an increase in [I3O +] of about 4 10-8 M, can bring a healthy person close to death. Alkalosis occurs when the blood pH value exceeds 7.6 and is accompanied by muscular rigidity. It is worth noting that the climbers who climb to high altitudes, eg on top of Mount Everest (8848 m), pH values ​​tend in their blood as 7.7 to 7.8 because of tachypnea that are due to the very low pressure of oxygen. The plasma is maintained at nearly constant pH value by means of buffers such as carbonates, phosphates and proteins. Of these perhaps most important is the system H2CO3 / HCO3-, which the regulatory action based on balance: H2CO3 + H2O [pic] HCO3-+ H3O + The CO2 enters the blood in the form H2CO3, during the breathing mode (the CO2 exchanged with O2 in the lungs). The content of the blood H2CO3 determined by the amount of CO2 we exhale, which correlates with the speed and depth of inhalation. The normal molar relationship HCO3-/ H2CO3 in blood is 20/1. If the concentration of HCO3-increase compared with that of H2CO3, then increases blood pH (alkalosis). If the concentration of H2CO3 increase compared with that of HCO3-, then the blood pH decreases (acidosis). To realize the high buffering capacity of blood, suppose we add 0,01 mol HCl to 1 L of blood. Then, the pH of blood varies from 7.4 to 7.2. If you do the same experiment, adding 0,01 mol HCl to 1 L saline (which is isotonic to the blood), the pH will change from 7.0 to 2.0. The hemoglobin found in red blood cells, pictured above, carries oxygen to tissues. Balance key for this action are: IIb + O2 [pic] H + + HbO2-. That this fundamental activity is controlled by the pH. Under acidic conditions the equilibrium is shifted to the left, which means that the hemoglobin can not hold constant the O2, while in basic environment shifts the balance right, which means that the hemoglobin does not leave easily O2 to the tissues.

Answer 5

A good question which might be more appropriate for the Biology section. I guess you got a really good answer though!