Question

Blood is a buffer solution. When carbon dioxide is absorbed into the bloodstream, it produces carbonic acid and lowers the pH. The body compensates by producing bicarbonate, a weak base to partially neutralize the acid. The equation which models blood pH in this situation is pH(x)=6.1+log(800/x) where xx is the partial pressure of carbon dioxide in arterial blood, measured in torr. Find the partial pressure of carbon dioxide in arterial blood if the pH is 7.7.

Answer 1

Answer:

x ≅ 20.10 torr

Step-by-step explanation:

Given that the equation which models blood pH in the question is;

pH(x)=6.1+log(800/x)

where;

pH = 7.7

x = partial pressure of carbon dioxide in arterial blood, measured in torr.

we are asked to find (x)

In order to do that, we use the given equation:

pH(x)=6.1+log(800/x)

since pH = 7.7

7.7 = 6.1 + log (800/x)

7.7 - 6.1 =  log (800/x)

1.6 =  log (800/x)

$10^{1.6}= \frac{800}{x}$

$x= \frac{800}{10^{1.6}}$

x = 20.09509145

x ≅ 20.10 torr

Answer 2

Answer:

20.10

Step-by-step explanation: