A student does an experiment to determine the molar solubility of lead(II) bromide. He constructs a voltaic cell at 298 K consisting of 0.821 M lead nitrate solution and a lead electrode in the cathode compartment, and a saturated lead bromide solution and a lead electrode in the anode compartment. If the cell potential is measured to be 5.60*10-2 V, what is the molar solubility of lead bromide at 298 K determined in this experiment? mol/L
A student does an experiment to determine the molar solubility
of lead(II) iodide. He constructs a voltaic cell
at 298 K consisting of 0.730 M lead nitrate
solution and a lead electrode in the cathode compartment, and a
saturated lead iodide solution and a lead
electrode in the anode compartment.
If the cell potential is measured to be
8.05×10-2 V, what is the value of
Ksp for lead iodide at 298 K based on
this experiment?
Ksp for PbI2 =...
A student does an experiment to determine the molar solubility
of lead(II) bromide. She constructs a voltaic cell
at 298 K consisting of 0.675 M lead nitrate
solution and a lead electrode in the cathode compartment, and a
saturated lead bromide solution and a lead
electrode in the anode compartment.
If the cell potential is measured to be
5.36×10-2 V, what is the molar
solubility of lead bromide at 298 K determined in
this experiment?
The reaction of aqueous potassium chloride and aqueous lead(II)
nitrate produces lead(II) chloride and potassium nitrate, according
to the balanced chemical equation shown. 2 KCl (aq) + Pb(NO3)2 (aq)
→ PbCl2 (s) + 2 KNO3 (aq) If equal volumes of 0.500 M KCl (aq) and
0.500 M Pb(NO3)2 (aq) are combined, what will the final
concentration of KNO3 (aq) be?
The solubility product of PbBr2 is 8.9 10-6. Determine the
molar solubility in the following.
(a) pure water
(b) 0.26 M KBr solution
(c) 0.21 M Pb(NO3)2 solution