What is the "Carbonic acid-bicarbonate" buffer system?

Answer 1

It's a buffer system that consists of a weak acid and its conjugate base.

The carbonic acid - bicarbonate buffer system consists of carbonic acid, a weak acid, and the bicarbonate anion, its conjugate base.

The important thing to realize here is that carbonic acid, #H_2CO_3#, is actually formed when carbon dioxide, #CO_2#, is dissolved in water.

After carbon dioxide is dissolved, it combines with the water molecules to form carbonic acid according to the following equilibrium reaction

#CO_(2(aq)) + H_2O_((l)) rightleftharpoons H_2CO_(3(aq))#

Being a weak acid, carbonic acid can then go on and donate its protons in two steps to form the bicarbonate, #HCO_3""^(-)#, and the carbonate anions, #CO_3^(2-)#.

The equilibrium of interest will be

#underbrace(H_2CO_(3(aq)))_(color(green)("weak acid")) + H_2O_((l)) rightleftharpoons H_3O_((aq))^(+) + underbrace(HCO_(3(aq))^(-))_(color(blue)("conjugate base"))#

In essence, if a disturbance occurs in the concentration of the species involved in this equilibrium reaction, the equilibrium will shift in a direction that will compensate that disturbance - think Le Chatelier's Principle.

If a strong acid is introduced in the system, which is equivalent to having an increased concentration of hydronium ions, it will react with the bicarbonate anion and form carbonic acid, a weak acid.

The equilibrium will thus shift to the left.

The fact that a strong acid is converted to a weak one will prevent to acidity of the solution to increase significantly.

Likewise, if a strong base is introduced, it will react with the carbonic acid to form the bicarbonate anion, thus reducing the potential increase in pH.

The equilibrium will shift right.

This buffer is actually used by the body to regulate blood acidity.

Check out this really cool demonstration by Professor Diane O'Dowd of how this buffer works

https://tutor.hix.ai

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Answer 2

The carbonic acid-bicarbonate buffer system is a chemical system that helps maintain the pH of blood and other bodily fluids within a narrow range. It consists of carbonic acid (H2CO3) and bicarbonate ions (HCO3-), which can react with each other to maintain a stable pH. When there is an increase in acidity, carbonic acid dissociates to release bicarbonate ions, which can bind to hydrogen ions and neutralize them, helping to raise the pH. Conversely, when there is an increase in alkalinity, carbonic acid can be formed from bicarbonate ions, helping to lower the pH. This buffer system plays a crucial role in regulating the body's acid-base balance.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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