Question

Among the following given salts:
$N{a_2}C{O_3},NaCl,N{H_4}Cl,C{H_3}COONa,{K_2}S{O_4},{(N{H_4})_2}S{O_4}$
Which of these salts will give?
(A) Acidic solution
(B) Basic solution (alkaline solution)
(C) Neutral solution

Answer 1

To determine whether the given solution is acidic, basic or neutral, we have to look for the concentration of hydrogen ions in the solution ${H^ + }$ . Acidic solutions are any aqueous solution that has hydrogen ion concentration, ${H^ + }$ greater than water.

Complete answer:
So, the basic solution will be any aqueous solution which has hydrogen ion concentration less than water or pH of the solution is greater than $7$ .
Similarly, acidic solution should have a pH less than $7$ .
A neutral solution can be defined as the solutions which are neither acidic nor basic. Neutral solutions have a pH $7$ .
So, based on our knowledge, we can :
So, among the given salts, let’s categorise all the salts.
-So , the acidic solutions will be given by the salts - $N{H_4}Cl$ , ${(N{H_4})_2}S{O_4}$
-And the basic or alkaline salts will be given by the salts - $N{a_2}C{O_3}$ , $C{H_3}COONa$
-Neutral solutions will be given by the - $NaCl$ , ${K_2}S{O_4}$
Neutral solutions have balanced charges and they dissociate completely in the water.

Note:
$N{H_4}Cl$ will give an acidic solution because it is composed of strong acid $HCl$ and the weak base $N{H_4}OH$ . So, on dissociation in water, it will give an acidic solution. Similarly, $C{H_3}COONa$ will give basic solution because it is a combination of weak acid – acetic acid and strong base – sodium hydroxide i.e. $NaOH$ . So, it will give an alkaline solution. Whereas, $NaCl$ is a neutral salt and will give a neutral solution as it is composed of strong acid - $HCl$ and strong base $NaOH$ . So they neutralize the charges of each other and yield neutral solutions. The combination of weak acid and weak base with same intensity also results in neutral solutions.