In each of the following cases, decide whether a precipitate...

In each of the following cases, decide whether a precipitate will form when mixing the indicated reagents, and write a balanced equation for the reaction. (a) $\mathrm{NaBr}(\mathrm{aq})+\mathrm{AgNO}_{3}(\mathrm{aq})$ (b) $\mathrm{KCl}(\mathrm{aq})+\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})$

In each of the following cases, decide whether a precipitate will form when mixing the indicated reagents, and write a balanced equation for the reaction.
(a) $\mathrm{NaBr}(\mathrm{aq})+\mathrm{AgNO}_{3}(\mathrm{aq})$
(b) $\mathrm{KCl}(\mathrm{aq})+\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})$

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Key Concepts

Precipitation Reactions

Precipitation reactions occur when two aqueous solutions mix and form an insoluble solid, the precipitate. This reaction is driven by the combination of ions in solution that form a compound with low solubility, causing it to separate out from the solution.

Double Displacement Reactions

Double displacement reactions involve the exchange of ions between reacting compounds, generally leading to the formation of two new products. This type of reaction is common in precipitation reactions, as the swapped ions may combine to form an insoluble compound.

Solubility Rules

Solubility rules are guidelines that help predict whether a particular ionic compound will dissolve in water. These rules are essential in determining whether a precipitate will form when two aqueous solutions are mixed, by identifying compounds that are insoluble under standard conditions.

Balanced Chemical Equations

Balanced chemical equations represent the quantitative relationships between reactants and products in a chemical reaction. Writing a balanced equation involves ensuring that both mass and charge are conserved, which is crucial for accurately depicting reactions like precipitation and double displacement.

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