In aqueous solution, is potassium perbromate, $K{\mathrm{Br}}_4$, expected to produce an acidic, basic, or neutral solution?

• A. Neutral, because it is a salt of a strong base ($KOH$) and a strong acid ($H{\mathrm{Br}}_4$)
• B. Basic, because $K+$ hydrolyzes water to form $KOH$
• C. Basic, because ${\mathrm{Br}}_4-$ is the conjugate base of a weak acid
• D. Acidic, because ${\mathrm{Br}}_4-$ is the conjugate base of a weak acid

Answer: (A)

Verified step by step guidance

1. Identify the ions produced when potassium perbromate (KBr\_4) dissolves in water. It dissociates into K\^+ and BrO\_4\^- ions.
2. Determine the nature of the cation K\^+. Since K\^+ comes from KOH, a strong base, it does not hydrolyze water and does not affect the pH significantly.
3. Determine the nature of the anion BrO\_4\^-. It is the conjugate base of perbromic acid (HBrO\_4), which is a strong acid, so BrO\_4\^- does not hydrolyze water or affect the pH.
4. Since neither ion hydrolyzes water to produce H\^+ or OH\^-, the solution remains neutral.
5. Conclude that potassium perbromate produces a neutral solution because it is a salt formed from a strong acid and a strong base.