Determine if each salt will form a solution that is acidic, basic, or pH-neutral. b. C₂H₅NH₃NO₃ c. K₂CO₃ d. RbI e. NH₄ClO

Verified step by step guidance

1. <b>Step 1:</b> Identify the ions formed by each salt when dissolved in water. For example, C₂H₅NH₃NO₃ dissociates into C₂H₅NH₃⁺ and NO₃^-.
2. <b>Step 2:</b> Determine the nature of each ion. Check if the cation or anion is derived from a weak acid or weak base. For instance, C₂H₅NH₃⁺ is the conjugate acid of a weak base (ethylamine), and NO₃^- is the conjugate base of a strong acid (HNO₃).
3. <b>Step 3:</b> Predict the pH effect of each ion. A cation that is the conjugate acid of a weak base will make the solution acidic, while an anion that is the conjugate base of a weak acid will make the solution basic. If both ions are from strong acids and bases, the solution is neutral.
4. <b>Step 4:</b> Apply this analysis to each salt: (b) C₂H₅NH₃NO₃ is acidic, (c) K₂CO₃ is basic, (d) RbI is neutral, (e) NH₄ClO is acidic.
5. <b>Step 5:</b> Summarize the results: Analyze the ions' origins and their effects on the solution's pH to determine if the solution is acidic, basic, or neutral.