The importance of pH maintenance in blood.
Maintenance of the pH in blood and in intracellular fluids is absolutely crucial to the processes that occur in living organisms. This primarily because the functioning of enzymes-catalysts for these processes - is sharply pH dependent. The normal pH value of blood plasma is 7.4. Severe illness or death can result from sustained variations of a few tenths of pH unit.
Among the factors that lead to a condition of acidosis, in which there is a decrease in the pH of blood are heart failure, kidney failure diabetes mellitus, persistent diarrhoea or a long term high protein diet.A temporary condition of acidosis may result from prolonged, intensive exercise. Alkalosis, which causes increase in pH of blood may occur as a result of severe vomiting over breathing or exposure to high altitudes.
Several factors are involved in the control of the pH of blood. A particularly important one is the ratio of dissolved $H C O_{3}^{-}$ to $H_{2} C O_{3}$ . $C O_{2} (g)$ is moderately soluble in water and in aqueous solution reacts only to a limited extent to produce $H_{2} C O_{3}$ .

$C O_{2} + H_{2} O ⇌ H_{2} C O_{3} (a q)$
$H_{2} C O_{3} + H_{2} O ⇌ H C O_{3}^{-} + H_{3} O^{+}$ , $p K_{a_{1}} = 6.11$

$H C O_{3}^{-} + H_{2} O ⇌ C O_{3}^{2 -} + H_{3} O^{+}$ , $p K_{a_{2}} = 10.25$
In the $H_{2} C O_{3}$ , $H C O_{3}^{-}$ buffer system, we deal only with the first ionization step $(K_{a_{1}})$ : $H_{2} C O_{3}$ is a weak acid and $H C O_{3}^{-}$ is the conjugate base (salt). $C O_{2}$ enters the blood from tissues as the by -product of a metabolic reaction. In the lungs, $C O_{2}$ (g) is exchanged for $O_{2}$ (g), which is transported throughout the body by the blood.Important diagnostic analysis in the blood is :

[H_{2} P O_{4}^{-}] / [H P O_{4}^{-}]

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[H C O_{3}^{-}] / [C O_{2}]

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[C O_{3}^{2 -}] / [H C O_{3}^{2 -}]

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[P O_{4}^{3 -}] / [H P O_{4}^{2 -}]

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Solution

The correct option is A $[H C O_{3}^{-}] / [C O_{2}]$
Important diagnostic analysis in the blood is the ratio $[H C O_{3}^{-}] / [C O_{2}]$ .
This indicates that the extent of the dissolution of carbon dioxide in the blood and the extent to which the pH of blood can be affected.

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Similar questions

The pH of blood is 7.4. If the buffer in bloods is $C O_{2} a n d H C O_{3}^{-}$ , calculate the ratio of conjugate base to acid $(H_{2} C O_{3})$ to maintain the pH of the blood. Given $K_{1}$ of $H_{2} C O_{3} = 4.5 \times 10^{- 7}$

Q. Blood

p H

is controlled by the concentrations of

H_{2} C O_{3}

and

H C O_{3}^{-}

. In the presence of

N a H C O_{3}

p H

of blood:

Q. The

\frac{[H C O_{3}^{-}]}{[H_{2} C O_{3}]}

ratio in blood (pH = 7.4) is approximately (pKa = 6.1 for

H_{2} C O_{3})

:
(Take log 2 = 0.3, log 3 = 0.5, log 7 = 0.85)

Q. The

[H C O_{3}^{-}] / [H_{2} C O_{3}]

ratio in the blood (pH = 7.4) is approximately

(p K_{a} = 6.1 f o r H_{2} C O_{3})

log 20= 1.301

Q. The species present in solution when

C O_{2}

is dissolved in water are

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The correct option is A [HCO−3]/[CO2]Important diagnostic analysis in the blood is the ratio [HCO−3]/[CO2].This indicates that the extent of the dissolution of carbon dioxide in the blood and the extent to which the pH of blood can be affected.

The correct option is A $[H C O_{3}^{-}] / [C O_{2}]$
Important diagnostic analysis in the blood is the ratio $[H C O_{3}^{-}] / [C O_{2}]$ .
This indicates that the extent of the dissolution of carbon dioxide in the blood and the extent to which the pH of blood can be affected.