Multiple Choice
According to general solubility rules, is CaCO3 soluble or insoluble in water?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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Which combination of aqueous solutions should produce a precipitate?
A
NaCl(aq) and AgNO3(aq)
B
LiBr(aq) and Na2CO3(aq)
C
NH4Cl(aq) and KOH(aq)
D
KNO3(aq) and Na2SO4(aq)
Verified step by step guidance1
Identify the ions present in each aqueous solution. For example, NaCl(aq) dissociates into Na\textsuperscript{+} and Cl\textsuperscript{-}, and AgNO3(aq) dissociates into Ag\textsuperscript{+} and NO3\textsuperscript{-}.
Consider the possible combinations of cations and anions when the two solutions are mixed. For NaCl and AgNO3, the possible new pairs are Ag\textsuperscript{+} with Cl\textsuperscript{-} and Na\textsuperscript{+} with NO3\textsuperscript{-}.
Use the solubility rules to determine if any of these new combinations form an insoluble compound (precipitate). For example, silver chloride (AgCl) is known to be insoluble in water and will precipitate.
Repeat this process for each pair of solutions given: identify ions, predict new combinations, and check solubility rules to see if a precipitate forms.
Conclude which pair produces a precipitate based on the formation of an insoluble compound according to the solubility rules.
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