Introduction:
The degree of hydrolysis and pH of an aqueous solution of ammonia formate can be determined by considering the equilibrium reaction between ammonia formate and water. Ammonia formate is a salt formed by the reaction between ammonia (NH3) and formic acid (HCOOH). When ammonia formate dissolves in water, it undergoes hydrolysis, resulting in the formation of ammonium ions (NH4+) and formate ions (HCOO-). The degree of hydrolysis refers to the extent to which a compound undergoes hydrolysis, and it is expressed as the fraction of the compound that has undergone hydrolysis.

Degree of Hydrolysis:
The degree of hydrolysis of ammonia formate can be determined by considering the equilibrium reaction:

NH4HCOO + H2O ⇌ NH4+ + HCOO-

The equilibrium constant for this reaction is denoted by K. The degree of hydrolysis (α) can be calculated using the formula:

α = [NH4+] / [NH4HCOO]

Since the initial concentration of NH4HCOO is equal to its molarity (assuming the solution is dilute), we can write:

α = [NH4+] / C0

Where C0 is the initial concentration of NH4HCOO.

pH:
The pH of an aqueous solution is a measure of its acidity or basicity. It is determined by the concentration of hydrogen ions (H+) in the solution. In the case of ammonia formate, the pH can be calculated using the pKa value of formic acid, which is the negative logarithm of its acid dissociation constant (Ka).

The pKa of formic acid is approximately 3.75. Since formic acid is a weak acid, it only partially dissociates in water. The equilibrium reaction for the dissociation of formic acid can be written as:

HCOOH ⇌ H+ + HCOO-

Using the Henderson-Hasselbalch equation, the pH of the solution can be calculated as:

pH = pKa + log ([HCOO-] / [HCOOH])

Where [HCOO-] is the concentration of formate ions and [HCOOH] is the concentration of formic acid.

Conclusion:
The degree of hydrolysis of an aqueous solution of ammonia formate can be determined by calculating the fraction of ammonium ions formed relative to the initial concentration of ammonia formate. The pH of the solution can be calculated by considering the dissociation of formic acid and using the Henderson-Hasselbalch equation. These calculations require knowledge of the equilibrium constant and pKa value of formic acid.