Question

1. Use the Henderson-Hasselbalch equation to determine the ratio of acid to base in a formic acid-formate buffer with a pH of 3.00

2. Assume that the human blood buffer includes 0.00080 M carbonic acid and 0.0080 M hydrogen carbonate. What is the pH of 7.00 liter of blood under these conditions?

3. How many moles of strong acid must be added to the blood in question 2 to bring the hydrogen carbonate/ carbonic acid ratio to the hazardous level of 5:1 AND what would the pH be?

4. How many moles of hydrogen carbonate need to be added to the blood in question 3 to raise the pH to 7.45?

Answer 1

1)- Ratio of Acid to base is 5.62.A

2)- pH of blood at the given conditions is 7.35.

3)- Moles of strong acid added = 3.115*10-7

4)- Amount of hydrogen carbonate added = 0.014 mol
According to Henderson - Hasselbalch equation. pH a pka + los CA71 [HA] , Where , Ka - Acid dissociation constant [HA] - concentration of [n] = concentration of Aeid conjugate Вале: NOW, PH = 3:00 Pka = 3.75 lotor Jarmic acid) 3.75 + 3) 2 = 3,15 + logio a content 5) -0.75 2 Logio lamina) 0,178 so the ratio of Acid to base in ait i 5.6 5.62

0.83 Here the human blood is a carbonic acid and its conjugate 50, Handerson - Hasselbalch qqn buffer of base is valid CAL 5) pH = P ka t log10 Here, pka = 6.35 56 0.0056 3) PH = 6.35 + log10 (0.01666) PH = 6.35 +1 = 7,357 1. So, the pH of blood is 7.35

In ay Here, [A]. 5. [HAT . 2) PH 6.35 + log10 (5) 5) PH = 6.35 +0.7 = 7,05 a) JPH 3.7:05 ) concentration of H= 10 17:05 Gritical concentration of it+ = 10-7-35 So, concentration of added = 5-7.05 -7.35 10 - 10 So, the added - 4.45 X10-8 male Moles of strong acid (4.45 x 108 x7) mo! 1 3 3.335 x 10-7 moles.

Day 7 Here, PHE PKO + Cogno con pH = pka = 7.45 6.35 6) =) [A] - 12.56 X 0.0008 = 0.01 = concentration of Base Jiras = orod gnitial conc. of Base = 0.008 so, Amount of Base added > 0.01 -0.002 = 0.002 Hence of carbonate Amount of hydrogen added 2 (0.002% 7) mos 0.014 mol