AP Chemistry
4.7 Types of Chemical Reactions
4.5 Stoichiometry
4.2 Net Ionic Equations
A student mixes \(100.0\text{ mL}\) of \(0.10\text{ M Pb(NO}_3)_2\text{(aq)}\) with \(100.0\text{ mL}\) of \(0.10\text{ M KI(aq)}\) at \(25^\circ\text{C}\). A precipitate of \(\text{PbI}_2\text{(s)}\) forms according to the balanced equation below.
\[ \text{Pb(NO}_3)_2\text{(aq)} + 2\,\text{KI(aq)} \rightarrow \text{PbI}_2\text{(s)} + 2\,\text{KNO}_3\text{(aq)} \]
The molar mass of \(\text{PbI}_2\) is \(461\text{ g/mol}\). Assuming the reaction goes to completion, what is the maximum mass of \(\text{PbI}_2\text{(s)}\) that can be produced?
\[ \text{Pb(NO}_3)_2\text{(aq)} + 2\,\text{KI(aq)} \rightarrow \text{PbI}_2\text{(s)} + 2\,\text{KNO}_3\text{(aq)} \]
The molar mass of \(\text{PbI}_2\) is \(461\text{ g/mol}\). Assuming the reaction goes to completion, what is the maximum mass of \(\text{PbI}_2\text{(s)}\) that can be produced?
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