Question

In some solutions, the concentration of ${H_3}{O^ + }$ remains constant even when small amounts of strong acid or strong base is added to them. These solutions are known as:
A) Colloidal solution.
B) Buffer solution.
C) True solution.
D) Ideal solution.

Answer 1

We know that the Buffer Solutions are water solvent-based solutions which contain a mixture of a weak acid and the conjugate base of the weak acid, or a weak base and the conjugate acid of the weak base. Buffer solution resists a change in upon dilution or upon the addition of small amounts of acid/alkali to them.

Complete step by step answer: Colloidal solutions:
Colloidal solution is also called colloidal suspension. Colloidal solutions are a mixture in which the substances are uniformly suspended in a fluid. A colloid is a very tiny and small material that extends out regularly all through another substance.
Therefore, the option A is incorrect.
In some solutions, the concentration of ${H_3}{O^ + }$ remains constant even when small amounts of strong acid or strong base is added to them. These solutions are known as buffer solutions.
Therefore, the option B is correct.
The homogenous mixture of two solutions is called a true solution.
Therefore, the option C is incorrect.
An ideal solution may be a mixture during which the molecules of various species are distinguishable, however, unlike the perfect gas; the molecules in the ideal solution exert forces on each other. When those forces are equivalent for all molecules independent of species then an answer is claimed to be ideal.
Therefore, the option D is incorrect.

Therefore, Option (B) is correct.

Note: We know the Bohr Effect is associated with the hemoglobin and it's inversely associated with acidity. Bohr Effect refers to the shift within the dissociation curve caused by the concentration of$C{O_2}$ which helps in increasing the efficiency of oxygen transportation through the blood.
The bicarbonate buffer system is an acid-base homeostatic mechanism involving the balance of acid, bicarbonate ion, and Carbon dioxide to take care of $pH$ within the blood, and among other issues, to support proper metabolic function.
Human blood contains a buffer of acid $\left( {{{\text{H}}_2}C{O_3}} \right)$, and bicarbonate anion $\left( {HC{O_3}^ - {\text{ }}} \right)$so as to take care of blood pH between $7.35$, and $7.45$ as a value above $7.8$ or less than $6.8$ can cause death. During this buffer, ${H_3}{O^ + }$ and $HC{O_3}^ -$ anion are in equilibrium with acid.
The reaction is,
$C{O_2} + {H_2}O \rightleftharpoons {H_2}C{O_3} \rightleftharpoons {H^ + } + HC{O_3}^ -$