Final answer:
The pH of human blood is regulated by buffer pairs and is normally around 7.35 due to the carbonate buffer system. Addition of H+ to blood plasma with a total carbonate pool would cause a decrease in pH.
Step-by-step explanation:
The concentration of carbonic acid (H2CO3) in blood is low compared to the concentration of the hydrogen carbonate ion (HCO3-).
This is because most of the by-products of metabolism that enter the bloodstream are acidic, so there needs to be a larger proportion of base than acid in order to prevent the buffer capacity from being exceeded.
The pH of human blood is regulated by the buffer pairs, and in this case, the buffer pairs determine a pH of 7.35. Normal variations in blood pH are usually less than 0.1, and pH changes of 0.4 or greater can be fatal.
Therefore, if 0.01 M H+ is added to blood plasma with a total carbonate pool, the pH would be slightly lower than the normal value of 7.35.