Determine whether each cation is acidic or pH-neutral. For each cation that is acidic, write an equation that shows how the cation acts as an acid. a. Sr²⁺ b. Mn³⁺ c. C₅H₅NH⁺

Verified step by step guidance

1. Step 1: Understand the concept of acidic and pH-neutral cations. Acidic cations are typically those that can donate a proton (H+) or increase the concentration of H+ in solution, often by reacting with water. pH-neutral cations do not affect the pH of the solution significantly.
2. Step 2: Analyze Sr^{2+}. Strontium ion (Sr^{2+}) is a Group 2 metal cation. Group 2 metal cations are generally considered pH-neutral because they do not hydrolyze in water to produce H+ ions.
3. Step 3: Analyze Mn^{3+}. Manganese(III) ion (Mn^{3+}) is a transition metal cation. Transition metal cations with a high positive charge can act as acids by hydrolyzing in water. Write the hydrolysis equation: Mn^{3+} + H_2O \rightarrow Mn(OH)^{2+} + H^+.
4. Step 4: Analyze C_5H_5NH^+. Pyridinium ion (C_5H_5NH^+) is the conjugate acid of pyridine (C_5H_5N). It can donate a proton to water, making it acidic. Write the equation: C_5H_5NH^+ + H_2O \rightarrow C_5H_5N + H_3O^+.
5. Step 5: Summarize the findings. Sr^{2+} is pH-neutral, Mn^{3+} is acidic and hydrolyzes to produce H^+, and C_5H_5NH^+ is acidic and donates a proton to form hydronium ion (H_3O^+).