i need to find the;
[Cl-] in PbCl2 solution,[Pb2+] in PbCl2 solution, and the ksp
given:
PbCl2(s)--> Pb2+(aq)+2Cl-(aq)
Temp of solution =20.2
volume of Pbcl2 solution=25.00ml
mass of dry AgCl2(g)=0.2543g
#moles :
AgCl(s)=1.77e-3
Cl(aq)=1.77e-3
Pb2+(aq)= 8.85e-4
To find the concentration of Cl- in PbCl2 solution, we need to calculate the number of moles of Cl- in the solution.
Given:
Volume of PbCl2 solution = 25.00 mL = 0.02500 L
Moles of Cl- = 1.77e-3
To calculate the concentration of Cl-:
Concentration (Na) = Moles (n) / Volume (V)
Concentration of Cl- = Moles of Cl- / Volume of PbCl2 solution
Concentration of Cl- = 1.77e-3 / 0.02500
To find the concentration of Cl- in PbCl2 solution, divide the moles of Cl- (1.77e-3) by the volume of the PbCl2 solution (0.02500 L).
Now, let's move on to finding the concentration of Pb2+ in the PbCl2 solution.
Given:
Moles of Pb2+ = 8.85e-4
To calculate the concentration of Pb2+:
Concentration (Nb) = Moles (m) / Volume (V)
Concentration of Pb2+ = Moles of Pb2+ / Volume of PbCl2 solution
Concentration of Pb2+ = 8.85e-4 / 0.02500
To find the concentration of Pb2+ in the PbCl2 solution, divide the moles of Pb2+ (8.85e-4) by the volume of the PbCl2 solution (0.02500 L).
Finally, let's find the Ksp (solubility product constant).
Given:
Mass of dry AgCl2 (g) = 0.2543 g
To calculate the Ksp:
mass of AgCl = mass of AgCl2
moles of AgCl = mass of AgCl / molar mass of AgCl
moles of PbCl2 = moles of AgCl
Ksp = [Pb2+] * [Cl-]^2
To find the Ksp, we need to find the moles of AgCl by dividing the mass of AgCl2 (0.2543 g) by the molar mass of AgCl. Since 1 mole of PbCl2 produces 2 moles of AgCl, the moles of PbCl2 will be the same as the moles of AgCl.
Once we have the moles of PbCl2 and the concentrations of Pb2+ and Cl- in the solution, we can calculate the Ksp using the formula: Ksp = [Pb2+] * [Cl-]^2