Questions: In which of the following aqueous solutions would you expect AgBr to have the lowest solubility? A) 0.15 M KBr B) pure water C) 0.10 M AgNO3 D) 0.10 M LiBr E) 0.20 M NaBr

In which of the following aqueous solutions would you expect AgBr to have the lowest solubility? A) 0.15 M KBr B) pure water C) 0.10 M AgNO3 D) 0.10 M LiBr E) 0.20 M NaBr
Transcript text: In which of the following aqueous solutions would you expect AgBr to have the lowest solubility? A) 0.15 M KBr B) pure water C) 0.10 M AgNO3 D) 0.10 M LiBr E) 0.20 M NaBr
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Solution

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Solution Steps

Step 1: Understanding Solubility and Common Ion Effect

The solubility of a salt like AgBr in a solution is affected by the presence of common ions. The common ion effect states that the solubility of a salt decreases in a solution that contains a common ion. In this case, the common ion is Br⁻.

Step 2: Analyzing Each Option
  • Option A (0.15 M KBr): Contains Br⁻ ions, which will decrease the solubility of AgBr due to the common ion effect.
  • Option B (pure water): No common ions present, so AgBr will have its normal solubility.
  • Option C (0.10 M AgNO₃): Contains Ag⁺ ions, which will also decrease the solubility of AgBr due to the common ion effect.
  • Option D (0.10 M LiBr): Contains Br⁻ ions, which will decrease the solubility of AgBr due to the common ion effect.
  • Option E (0.20 M NaBr): Contains Br⁻ ions, which will decrease the solubility of AgBr due to the common ion effect. This solution has the highest concentration of Br⁻ ions among the options.
Step 3: Determining the Lowest Solubility

The solubility of AgBr will be lowest in the solution with the highest concentration of the common ion, Br⁻. Among the options, 0.20 M NaBr (Option E) has the highest concentration of Br⁻ ions.

Final Answer

\(\boxed{\text{E) 0.20 M NaBr}}\)

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