Predict whether aqueous solutions of the following compounds are acidic, basic, or neutral: $(\mathbf{a}) \mathrm{NH}_{4} \mathrm{Br},(\mathbf{b}) \mathrm{FeCl}_{3},$ (c) \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) (e) \(\mathrm{NaHC}_{2} \mathrm{O}_{4}\). (d) \(\mathrm{KClO}_{4}\),

For each given compound, identify the cation and anion present. This will help us understand their behaviors when dissolved in water. (a) NH4Br: NH4+ (cation), Br- (anion) (b) FeCl3: Fe3+ (cation), Cl- (anion) (c) Na2CO3: Na+ (cation), CO3^2- (anion) (d) KClO4: K+ (cation), ClO4- (anion) (e) NaHC2O4: Na+ (cation), HC2O4- (anion)

Now we will analyze the behavior of the cations and anions when dissolved in water. (a) NH4Br: NH4+ behaves as an acid, donating a proton (H+) to water molecules, while Br- is a neutral spectator ion. The solution is acidic. (b) FeCl3: Fe3+ can hydrolyze water, producing H+ ions, while Cl- is a neutral spectator ion. The solution is acidic. (c) Na2CO3: Na+ is a neutral spectator ion, while CO3^2- behaves as a base, accepting protons (H+) from water molecules. The solution is basic. (d) KClO4: K+ is a neutral spectator ion, while ClO4- is a weak base. However, the basic character of ClO4- is negligible, so the solution is considered neutral. (e) NaHC2O4: Na+ is a neutral spectator ion, while HC2O4- can both accept a proton (acting as a base) and donate a proton (acting as an acid) from/to water molecules. However, the equilibrium lies more towards the acidic side. The solution is slightly acidic.

Based on the behavior of the cations and anions, we can predict whether the aqueous solutions of the compounds are acidic, basic, or neutral. (a) NH4Br: Acidic (b) FeCl3: Acidic (c) Na2CO3: Basic (d) KClO4: Neutral (e) NaHC2O4: Slightly Acidic