Question

How to predict whether the aqueous solution for the following salts are acidic, basic or neutral (a) $N{H_4}Br$ (b) $KCl{O_4}$ (c) $NaH{C_2}{O_4}$ (d) CsBr (e)$KHS{O_4}$ (f) $[C{H_3}N{H_3}]Cl$?

Answer 1

Hint: When a strong acid reacts with a strong base, then a neutral salt is formed. When a strong acid reacts with a weak base, then an acidic salt is formed. When a weak acid reacts with a strong base, then a basic salt is formed.

Complete step by step answer:
The salts are the chemical compound formed by the reaction between the acid and base with the elimination of water. The reaction is known as neutralization reaction.
Ammonium bromide $N{H_4}Br$ is a salt formed of a weak base ammonia $N{H_3}$ and strong acid hydrogen bromide HBr, so the salt ammonium bromide $N{H_4}Br$ is acidic salt.
Potassium perchlorate $KCl{O_4}$ is salt formed of strong acid perchloric acid $HCl{O_4}$ and strong base KOH, the salt is neutral salt.
Sodium hydrogen oxalate $NaH{C_2}{O_4}$ is a salt formed from weak acid oxalic acid ${H_2}{C_2}{O_4}$ and strong base NaOH, so the salt is basic salt.
Cesium bromide CsBr is a salt formed from strong base cesium hydroxide CsOH and strong acid hydrogen bromide HBr, so it is neutral salt.
Potassium bisulfate $KHS{O_4}$ is a potassium acid salt of sulfuric acid formed from potassium chloride and sulphuric acid. So it is an acidic salt.
Methyl ammonium chloride $[C{H_3}N{H_3}]Cl$ is an acidic salt. The $C{H_3}NH_3^ +$ is a conjugate acid of weak base methylamine $C{H_3}N{H_2}$.

Note:
The acidic salt dissolved in water forms an acidic solution. The basic salt on dissolving in water forms a basic solution. The neutral salt on dissolving in water forms a neutral solution.