Consider the following reaction
CaCl2(aq) + 2Ag2SO4(aq) !
CaSO4(?) + 2AgCl(?) .Which of the following statements is true?
1. Both CaSO4 and AgCl will precipitate
from solution.
2. Neither CaSO4 nor AgCl will precipitate
from solution.
3. CaSO4 will precipitate from solution, but
AgCl will not.
4. AgCl will precipitate from solution, but
CaSO4 will not
AgCl will precipitate from solution, but Ca(NO3)2 will not.
To determine which statement is true, we need to consider the solubility rules for the compounds involved. Solubility rules provide a set of guidelines that help us predict whether a compound will dissolve or form a precipitate in a solution.
For the reaction:
CaCl2(aq) + 2Ag2SO4(aq) -> CaSO4(?) + 2AgCl(?)
1. To determine if CaSO4 will precipitate, we look at the solubility rules for sulfates. Most sulfates are soluble, but there are some exceptions. One of the exceptions is calcium sulfate (CaSO4), which is considered moderately soluble. Therefore, CaSO4 is likely to precipitate from solution.
2. To determine if AgCl will precipitate, we look at the solubility rules for chlorides. Most chlorides are soluble, but there are again some exceptions. One of the exceptions is silver chloride (AgCl), which is considered insoluble. Therefore, AgCl is likely to precipitate from solution.
Based on this analysis, statement 1 is correct: Both CaSO4 and AgCl will precipitate from solution.