Notifications
Clear all
Chemistry
1
Posts
2
Users
0
Likes
295
Views
0
18/10/2021 9:52 am
Topic starter
Assuming that the buffer in the blood is CO2 - HCO3- Calculate the ratio of conjugate base to acid necessary to maintain blood at its proper pH of 7.4.
K1(H2CO3) = 4.5 × 10-7
(a) 11
(b) 8
(c) 6
(d) 14
1 Answer
0
18/10/2021 11:20 am
Correct answer: (a) 11
Explanation:
CO2 with H2O forms H2CO3
CO2 + H2O ⇌ H+ + HCO3-
K1 = \(\frac{[H^+][HCO_3^-]}{[CO_2]}\)
= 4.5 x 10-7
Again pH = -log[H+] = 7.4
∴ [H+] = 4.0 x 10-8
∴ \(\frac{[HCO_3^-]}{[CO_2]}\)
= \(\frac{4.5 \times 10^{-7}}{4 \times 10^{-8}}\) = 11