Multiple Choice
Which of the following substances is most likely to dissolve in hexane?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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When aqueous solutions of strontium bromide (SrBr_2) and potassium sulfate (K_2SO_4) are mixed, which compound will precipitate as a solid?
A
SrSO_4
B
K_2SO_4
C
KBr
D
SrBr_2
Verified step by step guidance1
Write the balanced molecular equation for the reaction between strontium bromide (SrBr\_2) and potassium sulfate (K\_2SO\_4). When these two aqueous solutions are mixed, the ions present are Sr^{2+}, Br^{-}, K^{+}, and SO_4^{2-}. The possible products are SrSO_4 and KBr.
Identify the possible precipitate by considering the solubility rules: most sulfate salts are soluble except those of barium, strontium, and lead. Potassium salts are generally soluble. Therefore, SrSO_4 is likely to be insoluble and precipitate out.
Write the net ionic equation by removing the spectator ions (ions that do not form the precipitate). The net ionic equation will involve Sr^{2+} and SO_4^{2-} forming solid SrSO_4:
$$\mathrm{Sr^{2+} (aq) + SO_4^{2-} (aq) \rightarrow SrSO_4 (s)}$$
Confirm that KBr remains dissolved in solution because both potassium and bromide ions form soluble compounds.
Conclude that the compound that precipitates as a solid when SrBr_2 and K_2SO_4 solutions are mixed is strontium sulfate (SrSO_4).
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