The solutions at the two Pb electrodes of a concentration cellwere prepared as follows:
Cell A: A mixture of 1.00 mL of 0.0500 MPb(NO3)2 with 4.00 mL of 0.0500 M KX (the soluble potassium salt ofan unspecified monovalent ion X-). Some PbX2(s) precipitates.
Cell B: 5.00 mL of 0.0500 M Pb(NO3)2.
The cell potential was measured to be 0.05100 V at 25 °C.
1.)By use of the Nernst equation, determine the concentration(M) of Pb2+ in the solution of Cell A.
2.)In Cell A, how many moles of X- have reacted with Pb2+?
3.)What is the concentration (M) of X- in the solution of cellA.
4.) Calculate Ksp of PbX2.
