Multiple Choice
Which of the following compounds is considered partially soluble in water according to common solubility rules?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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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.
Verified step by step guidance1
Recall the general solubility rules for ionic compounds in water, which help predict whether a precipitate will form when ions are combined in solution.
Identify that potassium ions (K^+) belong to the group of alkali metal ions, which are known to form soluble salts with almost all anions.
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.
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.
Conclude that no precipitate will form in a solution containing potassium ions and bromide ions because potassium bromide dissolves completely in water.
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