A student mixes of with of in a total volume of water at

CHEMISTRY · Multi-part · CBSE · Chemistry · Some Basic Concepts of Chemistry · Some Basic Concepts of Chemistry

Problem

A student mixes

1.00\,\text{mmol}

Pb(NO_3)_2\,(aq)

with

3.00\,\text{mmol}

KI\,(aq)

in a total volume of

100.0\,\text{mL}

water at

25\,^\circ\text{C}

. A bright yellow solid forms according to the reaction

Pb(NO_3)_2\,(aq) + 2\,KI\,(aq) \rightarrow PbI_2\,(s) + 2\,KNO_3\,(aq)

Assume all nitrate and potassium ions remain in the aqueous phase and that lead(II) iodide precipitates completely. (a) Write the balanced molecular equation for the reaction (already provided above) and verify that it is atom-balanced. (b) Write the corresponding complete ionic equation. (c) Derive the net ionic equation from the complete ionic equation, explicitly identifying the spectator ions removed. (d) Construct a particulate-level diagram of the reaction mixture AFTER precipitation is complete. Your diagram should: • Represent at least one full stoichiometric cycle based on the limiting reagent. • Include free ions that remain in solution and excess ions that did not react. • Use distinct sphere colors or cluster shapes for

Pb^{2+}

I^{-}

K^{+}

, and

NO_3^{-}

, and clearly show

PbI_2

as a separate solid phase. (e) Justify quantitatively how your diagram accounts for the limiting reagent, the excess reagent, and conservation of charge and mass.

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