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A 99.8 mL sample of a solution that is 12.0% KI by mass (density: 1.093 g/mL) is added to 96.7 mL of another solution that is 14.0% Pb(NO3)2 by mass (density: 1.134 g/mL). How many grams of PbI2 should form?

\[ \text{Pb(NO}_3\text{)}_2(aq) + 2 \text{KI}(aq) \rightarrow \text{PbI}_2(s) + 2 \text{KNO}_3(aq) \]

Answer :

Answer:

[tex]m_{PbI_2}=18.2gKI[/tex]

Explanation:

Hello,

In this case, the undergoing chemical reaction is:

[tex]2KI+Pb(NO_3)_2\rightarrow 2KNO_3+PbI_2[/tex]

Thus, we proceed to compute the reacting moles of Pb(NO3)2 and KI, by using the given concentrations and densities and molar masses which are 331.2 g/mol and 166 g/mol respectively:

[tex]n_{Pb(NO_3)_2}=96.7mL*\frac{1.134g}{mL}*\frac{0.14gPb(NO_3)_2}{1g}*\frac{1molPb(NO_3)_2}{331.2gPb(NO_3)_2} =0.0464molPb(NO_3)_2\\\\n_{KI}=99.8mL*\frac{1.093g}{mL}*\frac{0.12gKI}{1g}*\frac{1molKI}{166gKI} =0.0789molKI[/tex]

Next, the 0.0464 moles of Pb(NO3)2 will consume the following moles of KI (consider their 1:2 molar ratio):

[tex]n_{KI}^{consumed\ by\ Pb(NO_3)_2}=0.0464molPb(NO_3)_2*\frac{2molKI}{1molPb(NO_3)_2} =0.0928molKI[/tex]

Hence, as only 0.0789 moles of KI are available, KI is the limiting reactant, therefore the formed grams of PbI2, considering its molar mass of 461.01 g/mol and 2:1 molar ratio, are:

[tex]m_{PbI_2}=0.0789molKI*\frac{1molPbI_2}{2molKI} *\frac{461.01gPbI_2}{1molPbI_2} \\\\m_{PbI_2}=18.2gKI[/tex]

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