Nature of Buffer Solution
NH3 (aq) + H + (aq) → NH4 + (aq)
On base addition
If what is added is a base, the equilibrium shifts to the left, so that the OH ion concentration can be maintained. The added base reacts with the acidic component (NH4 +), forming a basic component (NH3) and water.
NH4 + (aq) + OH– (aq) → NH3 (aq) + H2O (l)
How the Buffer Solution Works
The buffer solution contains the acidic and basic components with their conjugate acids and bases, so that they can bind both H + ions and OH- ions. So that the addition of a little strong acid or strong base does not change the pH significantly.
Nature of Buffer Solution
The Characteristics of the Buffer Solution are:
The pH does not change when the solution is diluted.
The pH of the solution does not change if the solution is added with acid or base.
The relationship between pH and buffer solution is as follows:
A buffer solution of a mixture of weak acids and their salts.
[H +] = Ka or [H +] = Ka
pH = - log H +
Where:
Ka = Equilibrium Provision
= Number of moles of weak acid
= Number of moles of conjugate bases
A buffer solution of a weak base mixture with salt.
[OH–] = Kb or [H +] = Kb
pH = 14 - POH
POH = - OH log -
Where:
Kb = Equilibrium Provision
= Number of weak base moles
= Number of moles of conjugate acid
Buffer Solution Function
The existence of this buffer solution can be seen in everyday life such as in medicine, photography, leather industry and dyes. In addition to these applications, there is the function of applying the concept of this buffer solution in the human body as in body fluids.
This body fluid can be in intracellular fluid or extracellular fluid. Where the main buffer system in intracellular fluid such as H2PO4-and HPO42- which can react with an acid and base. As for the buffer system, it can maintain a nearly constant blood pH of around 7.4.
Maintaining the pH of the blood plasma to be in the pH range of 7.35 - 7.45, namely from the HCO3 ion - with Na + ion. If the blood pH is more than 7.45, alkalosis will occur, resulting in hyperventilation / excessive breathing, severe mutation. If the blood pH is less than 7.35, acidosis will result as a result of heart, kidney, liver and digestion will be disrupted.
Maintain the pH of processed foods in cans so they are not easily damaged / oxidized (asambenzoate with sodium benzoate).
In addition, the application of this buffer solution can be found in everyday life such as eye drops.
The existence of this buffer solution can be seen in everyday life such as in medicine, photography, leather industry and dyes. In addition to these applications, there is a function of applying the concept of this buffer solution in the human body as in bodily fluids.
This body fluid can be in intracellular fluid or extracellular fluid. Where the main buffer system in intracellular fluid such as H2PO4- and HPO42- which can react with an acid and base. As for the buffer system, it is able to maintain a nearly constant blood pH of around 7.4.
Maintaining the pH of the blood plasma so that the pH is around 7.35 - 7.45, which is from the HCO3 ion with Na + ion. If the pH of the blood is more than 7.45, it will experience alkalosis, resulting in hyperventilation / excessive breathing, great mutation. If the pH of the blood is less than 7.35, acidosis will result as a result of which the heart, kidneys, liver and digestion will be disrupted.