Question

Consider 0.25 M solutions of the following salts: $\mathbf{NaCl},\mathbf{RbOCl},\mathbf{KI},\mathbf{Ba}{\left({\mathbf{ClO}}_4\right)}_2,\mathbf{and}{\mathbf{NH}}_4{\mathbf{NO}}_3$. For each salt, indicate whether the solution is acidic, basic, or neutral.

Short answer

NaCl solution: Neutral

RbOCl solution: Basic

KI solution: Basic

$\mathrm{Ba}{\left({\mathrm{ClO}}_4\right)}_2$solution: Neutral

${\mathrm{NH}}_4{\mathrm{NO}}_3$solution: Acidic

Step-by-step solution

Nature of NaCl Solution 

As NaCl is a salt of a strong acid (HCl) and strong base (NaOH), the pH of the solution will be 7. Thus solution would be neutral.

Nature of RbOCl Solution

As RbOCl is a salt of a weak acid (HOCl) and strong base Rb(OH)₂, the solution would be basic.

Nature of Kl Solution

As KI is a salt of a strong acid (Hl) and strong base KOH, the solution would be neutral.

Nature of Ba(ClO4)2 Solution

As $\mathrm{Ba}{\left({\mathrm{ClO}}_4\right)}_2$is a salt of a strong acid ( ${\mathrm{HClO}}_4$) and strong base $\mathrm{Ba}{\left(\mathrm{OH}\right)}_2$, the solution would be neutral.

Nature of NH4NO3 Solution

As ${\mathrm{NH}}_4{\mathrm{NO}}_3$is a salt of a strong acid ( ${\mathrm{HNO}}_3$) and weak base ${\mathrm{NH}}_4\mathrm{OH}$, the solution would be acidic.