Final answer:
PbCl2 will precipitate out when equal volumes of 0.010 M Pb(NO3)2 and 0.010 M NaCl are mixed.
Step-by-step explanation:
To determine if PbCl2 will precipitate out when equal volumes of 0.010 M Pb(NO3)2 and 0.010 M NaCl are mixed, we need to compare the ionic product of PbCl2 (Qsp) to its solubility product constant (Ksp). If Qsp exceeds Ksp, then PbCl2 will precipitate. The balanced equation for the reaction is:
Pb(NO3)2 + 2NaCl → PbCl2 + 2NaNO3
The stoichiometry of the reaction shows that one mole of Pb(NO3)2 reacts with two moles of NaCl to give one mole of PbCl2 precipitate. Since both solutions have equal volumes and concentrations, the number of moles of Pb(NO3)2 will be half of the number of moles of NaCl. Therefore, there will be an excess of NaCl and PbCl2 will precipitate out.