A is an aqueous solution of KCl(aq) with unknown concentration. The
following experiment was carried out at 25°C to determine the concentration
of Cl- (aq) in A, and the Ksp of AgCl(s)
Step 1: A half-cell was made by dipping a silver strip into 100.0 cm3
Step 2: A galvanic cell was constructed by connecting the half-cell made in
Step 1 to a standard Zn2+(aq) Zn(s) half-cell with a suitable salt bridge.
Step 3: 0.100 M of AgNO3(aq) was added in portions from a burette to A. After
each addition of AgNO3(aq), the emf of the galvanic cell was measured.
When 8.0 cm3
of AgNO3(aq) had been added to A, what is the cell emf
(E) and the concentration of Ag+(aq) and Cl-
(aq) in the resultant solution?
The Attempt at a Solution
i just simply cal the [Ag+] added to the solution and by (mole added)/[total volume (108cm3)]
and [Cl-] by (mole remained after reaction)/[total volume(108cm3)]
is it correct? or need other specific equation to cal this problem?