Buffer Solutions

The concentration of calcium lactate is given as 0.005 M. Since calcium lactate dissociates completely, the concentration of lactate ions is:

Calcium lactate is a salt of a weak acid (lactic acid) and a strong base (calcium hydroxide). Therefore, hydrolysis of the salt will take place, and the pH can be calculated as:

Substituting the values:

Simplify:

Thus, the pH is:

Let's analyze the given statements and their validity concerning buffer solutions and physiological examples such as blood.

1. Statement I: "A Buffer solution is the mixture of a salt and an acid or a base mixed in any particular quantities."
   • This statement is false because a buffer solution is not just any mixture of a salt and an acid or base. It specifically consists of a weak acid and its conjugate base (or a weak base and its conjugate acid) in a suitable ratio. This combination helps maintain a stable pH upon the addition of small amounts of acid or base.
2. Statement II: "Blood is naturally occurring buffer solution whose pH is maintained by concentrations."
   • This statement is true. Blood is indeed a natural buffer system primarily maintained by a carbonic acid ( ) and bicarbonate ( ) buffer system. This mechanism is efficient in regulating the pH of blood around 7.4, crucial for physiological processes.

In conclusion, the correct option is that Statement I is false but Statement II is true. This correctly identifies the nature of buffers and recognizes the specific biological example of blood as a buffering system.

Step 1: Calculate the initial pH of the buffer solution.
Using the Henderson-Hasselbalch equation for a basic buffer: $ M, M \) $
The magnitude of the change is .
Expressing this in the required format: .
Rounding to the nearest integer gives 48.