Many buffers are polyprotic, such as carbonic acid. bicarbonate (hco3) has a pka of 10.33; while carbonic acid (hco3) has a pka of 6.35. use the henderson-hasselbalch equation to mathematically determine which form of this buffer predominates at ph 7.4 (homeostasis ph of blood). besides your mathematical answer, state the form that predominates too.

Carbonic acid/bicarbonate; bicarbonate  

Explanation:

H₂CO₃ + H₂O ⇌ H₃O⁺ + HCO₃⁻; pKₐ₁ =   6.35

HCO₃⁻ + H₂O ⇌ H₃O⁺ + CO₃²⁻;  pKₐ₂ = 10.33

The best buffer is one for which pKₐ ≈ pH.  

6.35 is closer to 7.4, so the carbonic acid/bicarbonate form of the buffer predominates

The pH of the blood is higher (more basic) than the pKₐ of carbonic acid, so its basic form (bicarbonate, HCO₃⁻) predominates.

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.