Writing equilibrium equation for reaction

Question

Assignment:

Maintaining blood pH: the role and control of CO₂ in blood buffering.

Maintenance of blood pH is critical to life. Slight fluctuations of pH result in conditions of acidosis or alkalosis. The carbonate buffer system is a key factor in controlling the pH. In this assignment you are to combine several key concepts in explaining this system.

Q1. Write an equilibrium equation for the reaction of CO₂ with water to produce carbonic acid and then bicarbonate and H⁺.

Q2. Discuss how CO₂ is produced and exchanged in the blood. In this discussion relate the exchange to Hess's law. Also discuss how increases or decreases in CO₂ affect the equation you wrote in the first part of this assignment (Le Chatelier's Principle).

Q3. With regard to the lungs discuss how CO₂ and O₂ exchange. Relate this discussion to Dalton's law of partial pressure.

Q4. Assuming a total air pressure of 760 mm Hg, and a concentration of CO₂ of 0.04% in air. What is the partial pressure of the CO₂?

Q5. Normal blood pH is 7.4, what is the H₃O⁺ concentration? What is the H₃O⁺ concentration whent the pH is 7.2? When the pH is 7.2 is the equilibrium in question 1 shifted to the left or the right.

Please provide the references for any information you utilize.

Provide complete and step by step solution for the question and show calculations and use formulas.