1) The molar solubility of PbI2 is 1.5X10-3 mol/L. PbI2(s) ? Pb2+(aq) + 2I-(aq) What is the molar concentration of iodide ion in a saturated PbI2 solution in mol/L? Hint: Consider mol ratios. Don't use scientific notation. Use 2 significant figures. ________
2) The molar solubility of PbI2 is 1.5X10-3 mol/L. PbI2(s) ?Pb2+(aq) + 2I-(aq) Determine the solubility constant, ksp, for lead(II) iodide: ksp = [Pb2+][I-]2 Don't use scientific notation. Use 2 significant figures. ________
3) How is the molar solubility affected by addition of lead(II) nitrate to the solution? Molar solubility = moles of salt that dissolve per L of solution. Hint: Consider Le Chatelier’s Principle, you are adding Pb2+ ions. PbI2(s)?Pb2+(aq) + 2I-(aq)
A) Increases molar solubility, equilibrium is shifted to the right. B) Decreases molar solubility, equilibrium is shifted to the left. C) No change, equilibrium can never be altered!
4) The molar solubility of PbI2 is 1.5X10-3 mol/L. PbI2(s) ?Pb2+(aq) + 2I-(aq) Determine the solubility constant, ksp, for lead(II) iodide: ksp = [Pb2+][I-]2 Don't use scientific notation. Use 2 significant figures. ________
1)
PbI2(s) ⇌ Pb2+(aq) + 2I-(aq)
s s
Ksp = [Pb2+] [2I-]
1.5*10^-3 = s*s
s^2 = 1.5*10^-3
s = 0.039 M
Answer: 0.039 M
2)
PbI2(s) ⇌ Pb2+(aq) + 2I-(aq)
s s
Ksp = [Pb2+] [2I-]
Ksp = s*s
Ksp = s^2
Ksp = (1.5*10^-3)^2
Ksp = 2.3*10^-6
Ksp = 0.0000023
Answer: 0.0000023
3)
when we add Pb(NO3)2 in PbI2 equilibrium, we are adding a common ion Pb2+
PbI2(s) ⇌ Pb2+(aq) + 2I-(aq)
Adding Pb2+, is like adding a product.
So, according to LeChatellier’s principle the equilibrium will shift to reactant side
So, solubility will decrease for PbI2
Answer: B) Decreases molar solubility, equilibrium is shifted to the left.
4)
This question is same as question number 2
PbI2(s) ⇌ Pb2+(aq) + 2I-(aq)
s s
Ksp = [Pb2+] [2I-]
Ksp = s*s
Ksp = s^2
Ksp = (1.5*10^-3)^2
Ksp = 2.3*10^-6
Ksp = 0.0000023
Answer: 0.0000023
1) The molar solubility of PbI2 is 1.5X10-3 mol/L. PbI2(s) ? Pb2+(aq) + 2I-(aq) What is the molar concentration of iodi...
6) The molar solubility of PbI2 is 1.5X10-3 mol/L. PbI2(s) ??Pb2+(aq) + 2I-(aq) A) What is the molar concentration of iodide ion in a saturated PbI2 solution? Hint: consider mol ratios. B) Determine the solubility constant, ksp, for lead(II) iodide: ksp = [Pb2+] x [I-]
A saturated solution of lead (II) iodide, PbI2 has an iodide concentration of 3.0 × 10-3 mol/ L. Calculate the solubility constant, Ksp, for lead (II) iodide. PbI2 (s) ß---à Pb2+(aq) + 2I-(aq) A saturated solution of lead (II) iodide, Pbl2 has an iodide concentration of 3.0 x 10-3 mol/ L. Calculate the solubility constant, Ksp, for lead (II) iodide Pbl2 (s) 8 3.5 x 10-8 5.0 x 10-8 2.8 x 10-8 1.4 x 10-8 -à Pb2 (aq)+2I(aq)
1- A saturated solution of lead(II) iodide, PbI2 has an iodide concentration of 3.0*10^-3 mol/L. a- What is the molar solubility of PbI2? b- Determine the solubility constant, Ksp for lead (II) iodide. c- Does the molar solubility of lead(II) iodide increase, decrease or remain unchanged with the addition of potassium iodide to the solution? Explain? 2- The Ksp of Ca(OH)2 was 5.2*10^-6 and 4.8*10^-6 respectively. a- What is the average Ksp of Ca(OH)2?
A saturated solution of lead(II) iodide, PbI2 has an iodide concentration of 3.0 x 10^-3 mol/L. a) What is the molar solubility of PbI2? b) Determine the solubility constant, Ksp, for lead(II) iodide. c) Does the molar solubility of lead (II) iodide increase, decrease, or remain unchanged with the addition of potassium iodide to the solution? EXPLAIN.
1/ The molar solubility of PbI2 is 1.5 x 10-3 M. a/ What is the molar concentration of iodide ion in a saturated PbI2 solution? b/ Determine the solubility constant, Ksp, for lead(II) iodide 2/ Calculate the molar solubility of PBI2 in the presence of 0.10 M NaI 3/ Compare the molar solubility given in problem 1 and the molar solubility calculated in problem 2. Explain the cause of the difference.
1. The molar solubility of Pbly in water is 1.5x10-mol/L. What is the solubility product of Pblz? answer = What is the molar solubility of Pb(OH)2 in a solution that is 0.010 M NaOH? The Ksp for Pb(OH)2 is 2.8x10-16 answer = 3. CaF2 dissolves in pure water. If the molar solubility of CaF2 is 2.2x10-4 mol/L, what is the concentration of fluoride in solution at equilibrium? answer
Determine the molar solubility of lead (II) iodide, PbI2, in 0.0500 mol/L NaI.
For the following equilibrium, if Ksp=1.4×10−11, what is the molar solubility of zinc carbonate? ZnCO3(s)↽−−⇀Zn2+(aq)+CO2−3(aq) Report your answer in scientific notation with two significant figures.
A saturated solution of lead (II) iodide has an iodide ion concentration of 3.0 x 10-3. What is the molar solubility of PbI2? Determine the Ksp for PbI2.
Solid PbI2 was added to a 0.030 M NaI solution. Calculate the molar concentration of lead ion in this solution. Ksp = 7.9 x 10-9 (at 25ºC) (Please show work) PbI2(s) <=> Pb2+ + 2I-