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D2. (8 pts) Determine whether the following compound precipitates from a solution that has the concentrations...
Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for Ksp values.) (a) CaCO3: [Ca2+] = 0.003M, [CO32−] = 0.003M (b) Co(OH)2: [Co2+] = 0.01M, [OH–] = 1 × 10–7 M (c) CaHPO4: [Ca2+] = 0.01M, [HPO42−] = 2 × 10–6 M (d) Pb3(PO4)2: [Pb2+] = 0.01M, [PO43−]= 1 × 10–13 M
Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for Ksp values.) (a) CaCO3: [Ca2+] = 0.003 M, [CO3 2−] = 0.003 M (b) Co(OH)2: [Co2+] = 0.01 M, [OH–] = 1 × 10–7 M (c) CaHPO4: [Ca2+] = 0.01 M, [HPO4 2−] = 2 × 10–6 M (d) Pb3(PO4)2: [Pb2+] = 0.01 M, [PO4 3−] = 1 × 10–13 M
An aqueous solution contains 0.034 M Brand 0.079 MT. A chemist wishes to do a fractional precipitation experiment in which he slowly adds Pb+2, which can form ppts of PbBr2 (s) [Ksp = 4.6 x 106 and Pbl2(S) [Ksp= 8.4 x 10 °). Which of the following is entirely correct? a. I precipitates first when [Pb2+1 = 3.4 x 10-7M b. Br precipitates first when [Pb2+] = 1.4 x 10-4M c. I'precipitates first when [Pb2+] = 1.1 x 10-7M d....
Question 12 The following compounds precipitates from a solution with the concentrations indicated. Ag2S: [Ag+] = 1 10-10M, [S2-) = 1 x 10-13M True False
Consider the equilibrium shown. PbBr (s)Pb2 (aq) +2 Br (aq) Kp 2.10 x 10-6 Determine the concentrations of Pb + and Br in a saturated solution of PbBr, in pure water (assume u = 0 M). Pb2 +10.0375 М [Br]= 0.0749 м Determine the concentrations of Pb+ and Br in a saturated solution of PbBr, in a solution with an ionic strength of 0.010 M. Pb2+1 0.010 М Br]= 0.02 м Determine the concentrations of Pb+ and Br in a...
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)
Experiment 8 Solubility of lonic Precipitates Lead chloride is a slightly soluble salt. When lead chloride dissolves in pure water or an aqueous solution, the small quantity that dissolves completely ionizes and reaches equilibrium in a saturated solution, PbCl(s) ® Pb (aq) + 2Cl(aq) Kp = [Pb (C) (1) Lets be the molar solubility of lead chloride. In pure water, s = [Pb ) = (CH) / 2. In a solution containing Cl, a common ion to lead chloride, s...
Consider the equilibrium shown. PbBr_(s) = Pb2 + (aq) + 2 Br" (aq) Kop = 2.10 x 10-6 Determine the concentrations of Pb2+ and Br" in a saturated solution of PbBr, in pure water (assume = 0M). [Pb2+1 = 0.00806 M [Br") = 0.01612 Determine the concentrations of Pb2+ and Br" in a saturated solution of PbBr, in a solution with an ionic strength of 0.010 M [Pb2+] = 0.010 [Br") = 0.02 Determine the concentrations of Pb²+ and Br"...
Hint Check Answe estion 29 of 32 > Consider the equilibrium shown. PbBr(s) = Pb2+ (aq) + 2 Br" (aq) Kyp = 2.10 x 10-6 Determine the concentrations of Pb2+ and Brin a saturated solution of PbBr, in pure water (assume u = 0 M). (PB2+1 = M [B") = Determine the concentrations of Pb2+ and Br“ in a saturated solution of PbBr, in a solution with an ionic strength of 0.010 M [Pb2+) = B- Determine the concentrations of...
please help me find the cation and anion nominal
concentrations for columns 4 and 5. the original solutions used as
sources of ions are all 0.20 M.
I'd appreciate if you showed the process as well as the
answers.
thank you!
no
equilibrium constant was given. It says the dilution equation must
be used to determine the the nominal concentrations.
Solutions Mixed Cation Anion Solution Solution Concentrations [Cation] [Anion] AgNO3 NaCI 0.10 0.10 AgNO3 KI AgNO3 Na2SO4 BaCl2 NaCl 0.10...