Final answer:
The question requires knowledge of Chemistry, addressing the calculation of pH for various solutions. Methods involve using the dissociation constants, concentrations, and relevant formulas to find the pH or ion concentration, applicable to college-level studies.
Step-by-step explanation:
The subject of this question falls under Chemistry, specifically involving pH calculations and acid-base chemistry at a College level. While the provided examples do not directly address sulfacetamide sodium monohydrate, they revolve around the calculation of pH or ion concentration for various acids, bases, and their respective titrations.
For instance, when calculating the pH of a 0.60M solution of formic acid, one would use the provided acid dissociation constant (Ka) and apply the formula pH = -log[H3O+], after determining the concentration of H3O+ ions in the solution. Similar methodologies apply to other examples, where equations involving either the Ka or Kb values, concentrations and pH or pOH are used to deduce the sought information.
However, since no specific Ka value for sulfacetamide sodium monohydrate is given in the original question, a precise pH calculation for that compound's solution cannot be performed without additional data.