28) The solubility of CdCO3(s) in 1.00 M KI(aq) is 1.2 x 10-3 mol/L. Given that Ksp of CdCO3 is 5.2x 10-12, what is Kf for [CdI4]2-?
28) The solubility of CdCO3(s) in 1.00 M KI(aq) is 1.2 x 10-3 mol/L. Given that...
To determine the solubility product, Ksp, for Ag2CO3, 1.00 mL of 1.00 mol/L Na2CO3(aq) and 1.00 mL of 0.100 mol/L AgNO3(aq) were combined. The mixture was stirred for 10 minutes to ensure that equilibrium had been reached. A voltaic cell was constructed to determine the concentration of soluble Ag (aq) ions left in solution at equilibrium, and [Ag leg was thus found to be 2.0 x 10-7 mol/L. Calculate the equilibrium concentration of CO32-(aq) ions left in solution at equilibrium,...
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...
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-]
The solubility of Ce(IO3)3 in a 0.14-M KIO3 solution is 1.3 x 10-7 mol/L. Calculate Ksp for Ce(IO3)3 - Ksp = Submit Answer Try Another Version 10 item attempts remaining Which of the following two compounds is expected to be more soluble in acidic solution than in pure water? a. Agi AgNO2 b. Mn(NO3) Mn(CN)2 Submit Answer Try Another Version 10 item attempts remaining Calculate the solubility of solid Ca3(PO4)2 (Ksp = 1.3x10-32) in a 0.16 M Na3PO4 solution. S...
A saturated solution of calcium iodate contains 2.37 g/L of Ca(IO3)2. (a) What is the solubility of calcium iodate in mol/L? (b) What are the concentrations of Ca2+ and IO3 – ion, respectively, in the saturated solution? (c) Calculate the Ksp value for Ca(IO3)2. Part b ) Silver ion, Ag+ , readily forms complex ion, Ag(S2O3)2 3– , with thiosulfate, S2O3 2– , according to the following equation: Ag+ (aq) + 2S2O3 2– (aq) ⇌ Ag(S2O3)2 3– (aq); Kf =...
The solubility of AgCN (s) in 0.200M NH3 (aq) is 8.8×10−6mol/L. Calculate Ksp for AgCN. ANSWER Ksp = 1.2×10−16
What is the solubility of PbBr2(s) in mol/L in pure water? ..010 ..0015 1.2 x 10-6 ..017 0.0021
Question 7 Determine the solubility of Cul(s) (Ksp = 1.1 x 10-12) in 0.15 M Cu(NO3)2(aq) solution 1- 1- Ksp = (S+ 0.15). (25)?. S = (Ksp/0.6) 1/2, S = 1.35 x 10-6 M 2- 2- Ksp = S . (S + 0.30). S = (Ksp/0.30), S = 3.67 x 10-12 M 3- 3- Ksp = (S + 0.15).S. S = (Ksp/0.15). S = 7.33 x 10-12 M
Q1 The solubility product, Kps, of Al (OH) 3 (s) is 1.0 x 10-33. What is its solubility (in g / L) in an aqueous solution of NaOH with a pH of 12.21? Q2 The formation constant, Kf, of PbCl42- (aq), Pb2 + (aq) + 4 Cl- (aq) ⇌ PbCl42- (aq), is 2.5 x 1015. What are the equilibrium concentrations of Pb2 + (aq) , Cl- (aq), and PbCl42- (aq) if we add 0.103 mol of Pb (NO3) 2 to...
BaCO;(s)Ba2t(aq) +CO3 (aq) The solubility product is given by: Ksp = [Ba2+] [C0321-5.5 × 10-10 mol2 dm-6 If [Ba2+1 CO is greater than 5.5 x 10-10 mol2 dm-6 a precipitate will form. [CO,2-] is less than 5.5 x 10-10 mol2 dm-6 no If [Ba2+1[ precipitate will form. WORKED EXAMPLE Will a precipitate form if we mix equal volumes of solutionsof 1.00 × 10-4 mol dm-3 Na,co, and 5.00 × 10-5 mol dm-3 BaCl2? 9