Question

In which of the following dissociation of \[N{H_4}OH\] will be minimum?
A. \[NaOH\]
B. \[{H_2}O\]
C. \[N{H_4}Cl\]
D. \[NaCl\]

Answer 1

Hint: Weak electrolytes can dissociate in a solvent upto a specific quantity. One weak electrolyte dissociates into ions partially, the number of ions per unit volume of the weak electrolyte helps in determining the solubility of that electrolyte.

Complete step-by-step answer:In order to know that the difference between strong and weak electrolytes is determined by the dissociation constant. The electrolytes dissociate more as the dissociation constant increases. That means, the strong electrolytes must dissociate more in water.
On the other hand, a weak electrolyte is less likely to unionize.
The ammonia solution in water has the formula \[N{H_4}OH\]. Dissociation of \[N{H_4}OH\] will be minimum in \[N{H_4}Cl\] because of the common ion effect. In \[N{H_4}Cl\] it will form buffer and the common ion \[N{H_4}^+\] present in the solution suppresses the ionization of \[N{H_4}OH\] by adding more of an ion which is a product of the equilibrium. NaCl is a strong electrolyte but does not have a common ion.

Option ‘C’ is correct

Note: It should be noted that a complex separates into its constituent particles during the dissociation process, just as salt separates into its constituent ions. As the salt separates into its ion components, they reassociate to create the complex once more. The dissociation process is a sort of reversible reaction of the association process. Both of these processes are in equilibrium for a weak electrolyte.