C) Ch3COOH is weak acid ostwald dilution law is only applicable on weak acid and weak bases

According to Ostwald's dilution law, the degree of ionization of weak electrolytes increases with dilution. This law applies to weak acids and bases, which partially dissociate in solution. Let's analyze each electrolyte mentioned in the question to see if Ostwald's dilution law gives satisfactory results for them:

A) HCl:
HCl is a strong acid that completely ionizes in water to form H+ and Cl- ions. Since it is a strong electrolyte, Ostwald's dilution law does not apply to it. The degree of ionization of a strong acid remains constant regardless of dilution.

B) HNO3:
HNO3 is also a strong acid that fully dissociates in water to produce H+ and NO3- ions. Similar to HCl, Ostwald's dilution law does not apply to strong acids like HNO3.

C) CH3COOH:
CH3COOH is a weak acid, also known as acetic acid. It partially dissociates in water to release H+ and CH3COO- ions. As per Ostwald's dilution law, the degree of ionization of weak acids increases with dilution. Hence, the dilution of CH3COOH will result in a higher degree of ionization.

D) NaOH:
NaOH is a strong base that fully ionizes in water to produce Na+ and OH- ions. Similar to strong acids, Ostwald's dilution law does not apply to strong bases like NaOH.

In summary, Ostwald's dilution law gives satisfactory results with the solution of weak electrolytes. It predicts that the degree of ionization of weak acids, such as acetic acid (CH3COOH), will increase upon dilution, while strong acids and bases, such as HCl, HNO3, and NaOH, do not follow this law as they are fully ionized even at low concentrations.