Topics & Terms
The value of Ksp of AgCl is 1.8 x 10-10. What would be the molar concentration of Ag+ and Cl- in AgCl in pure water placed in contact with solid AgCl(s)?
(a) 1.8 x 10 -10 M
(b) 1.3 x 10 -5 M
(c) 3.24 x 10 -20 M
What are the molar concentrations of ions in solution when solid PbI2 is in contact with pure water? (Ksp for PbI2 = 7.9 x 10-9)
(a) [Pb+2 ] = 1.3 x 10-3 M & [I-] = 2.6 x 10 -3 M
(b) [Pb+2] = 1.6 x 10-3 M & [I-] = 3.2 x 10-3 M
(c) [Pb+2] = [I-] = 2.0 x 10-3 M
What is the molar concentration of [Ag+] in AgCl solution in 0.10 M NaCl ?
(Ksp = 1.8 x 10-10) Remember that in this case the molar solubility of AgCl is equal to the [Ag+] as only the Ag+ reflects the amount of AgCl that dissolved.
(a) Ag+ = 1.3 x 10-5 M
(b) Ag+ = 0.10 M
(c) Ag+ = [AgCl] = 1.8 x 10-9 M
The molar solubility of PbCl2 in 0.10 M NaCl is 1.7 x 10-3 moles in a liter (that is 1.7 x 10-3 moles of PbCl2 will dissolve in 1 liter of the solution). What is the Ksp of PbCl2?
(a) Ksp = 1.8 x 10-5
(b) Ksp = 1.9 x 10-8
(c) Ksp = 1.7 x 10-4
Will CaSO4 precipitate if 50 mL of 0.0010 M CaCl2 is added to 50 mL of 0.010 M Na2SO4?
(Ksp for CaSO4 = 2.4 x 10-5)
(a) no precipitation will occur
(b) it is at equilibrium
(c) precipitation will occur
How many grams (g) of CaSO4 is formed when 20 mL of 0.010 M Na2SO4 is added to 100 mL of 0.001 M CaCl2?