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. d. Li⁺

검증된 단계별 안내

Identify the nature of the cation: Li^+ is a Group 1 metal cation.

Recall that cations from Group 1 metals, such as Li^+, are typically pH-neutral because they do not react with water to form H^+ ions.

Understand that acidic cations are usually those that can donate a proton (H^+) or increase the concentration of H^+ in solution.

Since Li^+ does not have the ability to donate a proton or increase H^+ concentration, it is considered pH-neutral.

Conclude that Li^+ is a pH-neutral cation and does not act as an acid in aqueous solution.

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Acidic Cations

Acidic cations are positively charged ions that can donate protons (H+) in solution, thereby lowering the pH. These cations typically come from weak bases or are transition metals that can hydrolyze in water, forming acidic solutions. Understanding whether a cation is acidic involves analyzing its ability to interact with water and affect the concentration of hydrogen ions.

pH Neutral Cations

pH neutral cations do not significantly affect the pH of a solution. They are usually derived from strong bases and do not hydrolyze in water, meaning they do not release protons. An example of a pH-neutral cation is Li+, which does not react with water to produce H+ ions, thus maintaining a neutral pH.

Hydrolysis Reactions

Hydrolysis reactions involve the reaction of a cation with water, leading to the formation of an acid or base. In the case of acidic cations, hydrolysis results in the release of H+ ions, which can be represented by an equation. For example, if a cation is acidic, the hydrolysis reaction can be written as: M^n+ + H2O ⇌ MH(n-1)+ + H+, where M^n+ is the cation.

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. d. Li+