Calculate the solubility of lead iodide, PbI2 in units of grams per liter. Ksp(PbI2) = 8.7×10-9. solubility = g/L
Calculate the solubility of lead iodide, PbI2 in units of grams per liter. Ksp(PbI2) = 8.7×10-9....
Calculate the solubility of lead chloride, PbCl2 in units of grams per liter. Ksp(PbCl2) = 1.7×10-5. solubility = g/L
Calculate the solubility of nickel carbonate, NiCO3 in units of grams per liter. Ksp(NiCO3) = 6.6E-9. solubility = g/L
The Ksp of PbI2 is 7.9 x 10-9. What is the molar solubility of lead (II) iodide?
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)
Calculate the solubility (g/L) of calcium sulfate, CaSO4 in units of grams per liter. Ksp(CaSO4) = 2.4E-5
Calculate the solubility of barium sulfate. BaSO4 in units of grams per liter. Ksp (BaSO4) = 1.1x10-10 solubility = AL The equilibrium concentration of chloride ion in a saturated lead chloride solution is M. In the presence of excess OH, the Ar+ (aq) ion forms a hydroxide complex ion. Al(OH)4 Calculate the concentration of free Ap+ ion when 1.56x10-mol Al(CH2C00)3(s) is added to 1.00 L of solution in which [OH-] is held constant (buffered at pH 12.10). For Al(OH)4, Ke=...
The Ksp for lead iodide (PI) is 1.4 x 10-8. Calculate the solubility of lead iodide in each of the following. a. water Solubility = mol/L b. 0.18 M Pb(NO3)2 Solubility = mol/L c. 0.018 M Nal Numeric input field Solubility = mol/L
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.