Theoretical Test

5. Acid-Base Chemistry (5 pts)5-1. Calculate [H + ], [OH - ], [HSO - 4 ], and [SO 2- 4 ] in a 1.0 x 10 -7 M solution ofsulfuric acid (K w = 1.0 x 10 -14 , K 2 = 1.2 x 10 -2 at 25 o C). In your work youmay use mass- and charge-balance equations. Answer with two significantfigures.5-2. Calculate the volume of 0.80 M NaOH solution that should be added toa 250 mL aqueous solution containing 3.48 mL of concentrated phosphoricacid in order to prepare a pH 7.4 buffer. Answer with three significantfigures. (H 3 PO 4 (aq), purity = 85 % wt/wt, density = 1.69 g/mL, FW = 98.00)(pK 1 = 2.15, pK 2 = 7.20, pK 3 = 12.44).5-3. The efficacy of a drug is greatly dependent on its ability to be absorbedinto the blood stream. Acid-base chemistry plays an important role in drugabsorption.MembraneStomachpH = 2.0BloodpH = 7.4H + + A - HA HA H + + A -Assume that the ionic form (A - ) of a weakly acidic drug does not penetratethe membrane, whereas the neutral form (HA) freely crosses the membrane.Also assume that equilibrium is established so that the concentration of HAis the same on both sides. Calculate the ratio of the total concentration([HA] + [A - ]) of aspirin (acetylsalicylic acid, pK = 3.52) in the blood to that inthe stomach.8