Final answer:
To determine the pH of solutions 0.23 M KCHO₂ and 0.23 M CH₃NH₃I, additional data such as ionization constants are required. For the 0.19 M KI solution, because KI is a neutral salt and the ions do not contribute to the solution's acidity or basicity, the pH is approximately 7.
Step-by-step explanation:
The student's question asks to determine the pH of specific solutions. Given the concentrations of various substances, the pH calculation can involve different equations and concepts, such as the ionization constant of weak acids or bases and the complete ionization of strong acids or bases, depending on the nature of the substance in solution.
For parts a and b of the student's question that involve 0.23 M KCHO₂ and 0.23 M CH₃NH₃I respectively, the pH calculation would need further information about the ionization constants (Ka or Kb) of the related acids or bases, as these represent solutions of potentially weak acids or weak bases. The pH of these solutions cannot be determined without additional data regarding their ionization properties.
For part c, the solution of 0.19 M KI is comprised of a strong electrolyte that does not alter the pH of the solution. Since KI itself is neutral and does not contribute hydronium or hydroxide ions to any significant extent, the pH of 0.19 M KI would be neutral, assuming the solution is in pure water and at standard temperature conditions (25 °C), giving a pH of approximately 7.