NEET MDS Lessons
Biochemistry
Acids and bases can be classified as proton donors and proton acceptors, respectively. This means that the conjugate base of a given acid will carry a net charge that is more negative than the corresponding acid. In biologically relavent compounds various weak acids and bases are encountered, e.g. the acidic and basic amino acids, nucleotides, phospholipids etc.
Weak acids and bases in solution do not fully dissociate and, therefore, there is an equilibrium between the acid and its conjugate base. This equilibrium can be calculated and is termed the equilibrium constant = Ka. This is also referred to as the dissociation constant as it pertains to the dissociation of protons from acids and bases.
In the reaction of a weak acid:
HA <-----> A- + H+
the equlibrium constant can be calculated from the following equation:
Ka = [H+][A-]/[HA]
As in the case of the ion product:
pKa = -logKa
Therefore, in obtaining the -log of both sides of the equation describing the dissociation of a weak acid we arrive at the following equation:
-logKa = -log[H+][A-]/[HA]
Since as indicated above -logKa = pKa and taking into account the laws of logrithms:
pKa = -log[H+] -log[A-]/[HA]
pKa = pH -log[A-]/[HA]
From this equation it can be seen that the smaller the pKa value the stronger is the acid. This is due to the fact that the stronger an acid the more readily it will give up H+ and, therefore, the value of [HA] in the above equation will be relatively small.
Vitamin B6: Pyridoxine, Pyridoxal, Pyridoxamine
Aids in protein metabolism and red blood cell formation. It is also involved in the body’s production of chemicals such as insulin and hemoglobin.
Vitamin B6 Deficiency Deficiency symptoms include skin disorders, dermatitis, cracks at corners of mouth, anemia, kidney stones, and nausea. A vitamin B6 deficiency in infants can cause mental confusion.
COENZYMES
Enzymes may be simple proteins, or complex enzymes.
A complex enzyme contains a non-protein part, called as prosthetic group (co-enzymes).
Coenzymes are heat stable low molecular weight organic compound. The combined form of protein and the co-enzyme are called as holo-enzyme. The heat labile or unstable part of the holo-enzyme is called as apo-enzyme. The apo-enzyme gives necessary three dimensional structures required for the enzymatic chemical reaction.
Co-enzymes are very essential for the biological activities of the enzyme.
Co-enzymes combine loosely with apo-enzyme and are released easily by dialysis. Most of the co-enzymes are derivatives of vitamin B complex
STEROIDS
Steroids are the compounds containing a cyclic steroid nucleus (or ring) namely cyclopentanoperhydrophenanthrene (CPPP).It consists of a phenanthrene nucleus (rings A, B and C) to which a cyclopentane ring (D) is attached.
Steroids are the compounds containing a cyclic steroid nucleus (or ring) namely cyclopentanoperhydrophenanthrene (CPPP).It consists of a phenanthrene nucleus (rings A, B and C) to which a cyclopentane ring (D) is attached.
There are several steroids in the biological system. These include cholesterol, bile acids, vitamin D, sex hormones, adrenocortical hormones,sitosterols, cardiac glycosides and alkaloids
The Hemoglobin Buffer Systems
These buffer systems are involved in buffering CO2 inside erythrocytes. The buffering capacity of hemoglobin depends on its oxygenation and deoxygenation. Inside the erythrocytes, CO2 combines with H2O to form carbonic acid (H2CO3) under the action of carbonic anhydrase.
At the blood pH 7.4, H2CO3 dissociates into H+ and HCO3 − and needs immediate buffering.
Buffers
• Biological systems use buffers to maintain pH.
• Definition: A buffer is a solution that resists a significant change in pH upon addition of an acid or a base.
• Chemically: A buffer is a mixture of a weak acid and its conjugate base
• Example: Bicarbonate buffer is a mixture of carbonic acid (the weak acid) and the bicarbonate ion (the conjugate base): H2CO3 + HCO3 –
• All OH- or H+ ions added to a buffer are consumed and the overall [H+ ] or pH is not altered
H2CO3 + HCO3 - + H+ <- -> 2H2CO3
H2CO3 + HCO3 - + OH- <- -> 2HCO3 - + H2O
• For any weak acid / conjugate base pair, the buffering range is its pKa +1.
It should be noted that around the pKa the pH of a solution does not change appreciably even when large amounts of acid or base are added. This phenomenon is known as buffering. In most biochemical studies it is important to perform experiments, that will consume H+ or OH- equivalents, in a solution of a buffering agent that has a pKa near the pH optimum for the experiment.
Most biologic fluids are buffered near neutrality. A buffer resist a pH change and consists of a conjugate acid/base pair.
Important Physiological Buffers include carbonate (H2CO3/HCO3-),
Phosphate (H2PO-4 /HPO2-4) and various protiens
The pH scale
An acidic solution is one in which [H+ ] > [OH- ]
•In an acidic solution, [H+ ] > 10-7 , pH < 7.
•A basic solution is when [OH- ] > [H+ ].
•In a basic solution, [OH- ] > 10-7 , pOH < 7, and pH >7.
• When the pH = 7, the solution is neutral.
•Physiological pH range is 6.5 to 8.0