You make 1.00 L of a 5.00 ppm solution of Pb2+ from its anhydrous nitrate salt.

Question

You make 1.00 L of a 5.00 ppm solution of Pb2+ from its anhydrous nitrate salt. You typically have to add a little acid to metal ion stock solutions to prevent the metal from precipitating as an insoluble hydroxide. Write a balanced chemical equation for this precipitation reaction for Pb2+ (including physical states), and calculate its equilibrium constant. [Note that the resulting solid will actually be PbO (assume the “yellow” form), so you will need to include a water molecule in your equation to get it to balance.]

Explanation / Answer

The dissolution of lead(II) nitrate involves dissociation into its constituent ions.

2 Pb(NO3)2( s) + H2O(l) 2 PbO(s) + 4 NO2(g) + O2(g) + + H2O(l)

Equilibirium conatant for the above reaction is

K= ([PbO (s)]2 [NO2(g)]4 [O2(g)]) / [Pb(NO3)2(s)]2

Related Questions

Navigate

• Browse (All)
• Browse Y
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.