Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral, write balanced chemical equations for the reactions causing the solution to be acidic or basic.

a.C5H5NHCLO4
b.NH4NO2
c.KOCL
d.NH4OCL

How do I know by looking?

You can look at the parent base & acid.

To determine whether the solutions of the given salts are acidic, basic, or neutral, we need to analyze the nature of the ions produced when these salts dissolve in water.

a. C5H5NHCLO4:
To analyze this salt, we consider its ions: C5H5NH+ and CLO4-. The ion C5H5NH+ is the conjugate acid of a weak base, pyridine. Therefore, it can react with water to produce H3O+ ions, making the solution acidic. The balanced chemical equation for this reaction is:

C5H5NH+ + H2O -> C5H5N + H3O+

b. NH4NO2:
The ions in this salt are NH4+ and NO2-. The ion NH4+ is the conjugate acid of a weak base, ammonia. Thus, it can react with water to produce H3O+ ions, making the solution acidic. The balanced chemical equation for this reaction is:

NH4+ + H2O -> NH3 + H3O+

c. KOCL:
The ions in this salt are K+ and OCL-. None of these ions react with water to produce H3O+ or OH- ions, meaning that they do not contribute to the acidity or basicity of the solution. Therefore, the solution is neutral.

d. NH4OCL:
The ions in this salt are NH4+ and OCL-. The NH4+ ion will react with water to produce H3O+ ions, as we have discussed before. However, OCL- is the anion of hypochlorous acid, which can dissociate into H+ and OCL- ions in water. This results in an increase in H+ ions, making the solution even more acidic. The balanced chemical equation for this reaction is:

H2O + OCL- -> H+ + OCl- + OH-

Therefore, the solution of NH4OCL becomes even more acidic due to the additional H+ ions produced by the OCL- ion.

You should be able to know this just by looking. What exactly do you not understand about the process?