pH & Buffer solution
Acids
definition:
these are substances that give hydrogen ions or
proton in solution.
Acid is a proton donor e.g. HCl------------> H + + Cl-
Types:
- Strong acids: e.g. HCL gives a large number of protons (H+) and dissociates completely in solution.
- Weak acids :e.g. Acetic acid gives a low number of protons (H+) and partially dissociate in solution.
Alkalies
definition:
these are substances that give (OH-)
hydroxyl ions in solution
types:
- Strong alkali: is that alkali which dissociates completely in water e.g. NaOH & KOH.
- Weak alkali : is that alkali which partially dissociate in water e.g Ammonium hydroxide (NH4OH) .
Amphoteric substances
These are substances , which act as an acid (proton
donor) or as a base (proton acceptor) e.g. H2O and amino acids.
H2O H3O (base)
OH- (acid) H+ + H2O
pH
- pH of a solution: it is the negative logarithm of hydrogen ions concentration to the base 10 . ( pH = - log [H+] to the base 10 ) .
The smaller the pH ,the increase the acidity.
pH of blood
- 7.37- 7.43)) 0.03 Blood pH is normally 7.4 ±
- A decreases in blood pH is called acidosis.
- An increases in blood pH is called alkalosis.
- Slight change in blood pH will affect the functions of the body e.g. any enzyme needs special pH for its maximum action.
- Severe change in blood pH may lead to death
- The blood pH is kept within very narrow rang due to the presence of buffers in both blood and tissues
Henderson – Hasselbalch equation
- This equation represents the relationship between pH and pK (acid dissociation constant) of a weak acid.
- a weak acid : HA ionizes as follows HA= H + + A-
- According the law of mass action :
- K = [A-] X [H +]
[HA]
- K [HA] = [A-] X [H +]
By dividing both sides by [A-]
v [H +] = K [HA]
[A-]
- By taking the Log of both sides.
v Log
[H +] = Log (K [HA]) = Log K + Log [HA]
[A-] [A-]
- By multiplying both sides by -1
v - Log [H +] = - Log K - Log [HA]
[A-]
- Log [H +] = pH
- Log K = PK
- pH = pK - Log [HA]
[A-]
Buffers
- Buffer is a solution , which resists change in pH when an acid or alkali is added to it.
- Buffers are usually a mixture of a weak acid with salt of strong base, or a mixture of a weak base and its salt of strong acid e.g. carbonic acid and sodium bicarbonate (H2CO3 / NaHCO3)
Body buffer
Buffers of the body are either present in plasma and
extracellular tissue or inside the RBCs. These buffer keep hydrogen ion
concentration within narrow range suitable
0.03 for life 7.4 ±
Physiologic buffers:
- Carbonic acid-bicarbonate buffer system H2CO3 -----> HCO3- + H+
Phosphate buffer: H2PO4 -------> PO-4
+ H+
- proteins .
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