When aqueous solutions of sodium chloride and silver (I) nitrate are mixed, does a precipitate...
Question:
When aqueous solutions of sodium chloride and silver (I) nitrate are mixed, does a precipitate form? If so, what is the balanced equation for the reaction?
a. No precipitate forms. This combination produces no apparent reaction.
b. {eq}NaCl(aq) + AgNO_{3}(aq) \rightarrow NaNO_{3}(aq) + AgCl(aq) {/eq}
c. {eq}NaCl(aq) + AgNO_{3}(aq) \rightarrow NaNO_{3}(aq) + ClAg(s) {/eq}
d. {eq}NaCl(aq) + AgNO_{3}(aq) \rightarrow Na(s) + AgNO3Cl(aq) {/eq}
e. {eq}NaCl(aq) + AgNO_{3}(aq) \rightarrow NaNO_{3}(aq) + 3AgCl(s) {/eq}
f. {eq}NaCl(aq) + AgNO_{3}(aq) \rightarrow NaNO_{3}(aq) + AgCl(s) {/eq}
Precipitation Reactions:
When two solutions of ionic compounds are mixed, the component ions can recombine in the solution. When the combination results in the formation of a solid product, a chemical reaction called precipitation occurred.
Answer and Explanation: 1
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The answer is f. {eq}NaCl(aq) + AgNO_{3}(aq) \rightarrow NaNO_{3}(aq) + AgCl(s) {/eq}.
When aqueous solutions of sodium chloride and silver (I)...
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Precipitation Reactions: Predicting Precipitates and Net Ionic Equations
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Chapter 10 / Lesson 9
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Study precipitate reactions. Determine precipitate solubility according to solubility rules. Learn to write ionic equations by following a molecular reaction.
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