The solubility product, Ksp, of PbCl2 is 1.6 × 10-5. What mass
of KCl(s) must be dissolved in 150.00 mL of 1.15M Pb(NO3)2 to
produce a solution that is just saturated in PbCl2?
Solubility products for AgCl and AgI are:
Ksp(AgCl) = 1.82*10-10
Ksp(AgI) = 8.31*10-17
0.010 moles of AgCl is added to 100 mL of water, then 0.020
moles of NaI is added. What are the concentrations of Cl and Ions
at equilibrium?
a) The solubility product for PbCl2 is 1.6 ∙ 10-5. The
solubility product for AgCl is 1.6 ∙ 10-10. How does the solubility
of lead chloride in a 0.10 M AgNO3 solution compare to the
solubility in pure water? Will it be higher, lower og not
changed?
Please explain your answer briefly as I dont get it.
b) The solubility of a salt MX is 1.1 ∙ 10-3 mol / L. What is
the solubility product Ksp for the salt?
Determine the molar solubility of AgI (Ksp = 8.50e-17) in 2.577
M S2O32- if the complex ion [Ag(S2O3)2]3- forms with a Kf =
2.90e13. Answers 0.09193/ 0.11637/ 0.04516/ or 0.14730
For PbCl2 (Ksp 2.4 x 10-4),
will a precipitate of PbCl2 form when 0.10 L of 3.0 x
10-2 M Pb(NO3)2 is added to 400 ml
of 9.0 x 10-2 M NaCl?
Please show, thanks!