Multiple Choice
Which pair of compounds is soluble in water?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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Which of the following chemical reactions will produce a precipitate?
A
KNO3(aq) + NaCl(aq) → KCl(aq) + NaNO3(aq)
B
Li2SO4(aq) + NaCl(aq) → 2 LiCl(aq) + Na2SO4(aq)
C
NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq)
D
Ba(NO3)2(aq) + Na2SO4(aq) → BaSO4(aq) + 2 NaNO3(aq)
Verified step by step guidance1
Identify the ions present in each reaction by writing the full ionic equation. For example, in the reaction NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq), the ions are Na⁺, Cl⁻, Ag⁺, and NO3⁻.
Determine the possible products by exchanging the ions between the reactants (this is called a double displacement reaction). For example, Ag⁺ pairs with Cl⁻ to form AgCl, and Na⁺ pairs with NO3⁻ to form NaNO3.
Check the solubility rules for each product to see if any of them are insoluble in water. Insoluble products will form a precipitate (solid). For example, AgCl is known to be insoluble and will precipitate out of solution.
Repeat this process for each reaction: write the ions, predict products, and apply solubility rules to identify if a precipitate forms.
Conclude which reactions produce a precipitate by identifying the formation of an insoluble solid (indicated by (s)) in the products.
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