Based on general solubility rules, would a solution containing potassium ions (K^+) and bromide ions (Br^-) form a precipitate?

• A. Yes, because potassium bromide is only slightly soluble.
• B. Yes, because bromide salts are generally insoluble.
• C. No, because all potassium salts are soluble in water.
• D. No, because only sodium salts are always soluble.

Answer: (C)

Verified step by step guidance

1. Recall the general solubility rules for ionic compounds in water, which help predict whether a precipitate will form when ions are combined in solution.
2. Identify that potassium ions (K^+) belong to the group of alkali metal ions, which are known to form soluble salts with almost all anions.
3. Recognize that bromide ions (Br^-) generally form soluble salts, except when paired with certain ions like Ag^+, Pb^{2+}, or Hg_2^{2+}, which are exceptions.
4. Combine the two points: since potassium salts are always soluble and bromide salts are generally soluble except for specific exceptions, potassium bromide (KBr) is soluble in water.
5. Conclude that no precipitate will form in a solution containing potassium ions and bromide ions because potassium bromide dissolves completely in water.