Calculate the concentration (in M) of Tl + when TlSCN just begins to precipitate from a solution that is 0.0325 M in SCN −. (Ksp = 1.57 ✕ 10−4)
Calculate the concentration (in M) of Tl + when TlSCN just begins to precipitate from a...
Calculate the Qsp or Ksp, as indicated, and determine whether a precipitate will form when each of the following mixtures is prepared. (a) 25.12 mL 1.57 ✕ 10−4 M CaCl2 is mixed with 25.13 mL 3.26 ✕ 10−3 M NaF. (Ksp for CaF2 = 3.5 ✕ 10−11) (b) 14.77 mL 3.68 ✕ 10−3M Pb(NO3)2 is mixed with 35.01 mL 1.63 ✕ 10−4M Na2SO4. (Ksp for PbSO4 = 2.5 ✕ 10−8) (c) 50.33 mL 2.62 ✕ 10−2M Pb(NO3)2 is mixed with...
A solution of Na2C2O4 is added dropwise to a solution that is 7.15e-02 M in Cd2+ and 5.21e-04 M in Ag+. The Ksp of CdC2O4 is 1.42e-08. The Ksp of Ag2C2O4 is 5.4e-12. Calculate the concentration of C2O42- present in the Cd2+/Ag+ solution when the first (initial) cation begins to precipitate, and the concentration of C2O42- present in this solution when the second (final) cation begins to precipitate. Write down which cation precipitates first and which precipitates second (last). Choose...
What concentration of the lead ion, Pb2+, must be exceeded to precipitate PbCl2 from a solution that is 1.00×10−2 M in the chloride ion, Cl−? Ksp for lead(II) chloride is 1.17×10−5
Silver ion is being considered as a reagent for separating 103) from CO32- in a solution that is 0.060 M in K2CO3 and 0.070 M in NalO3. Which anion will precipitate first when silver ion is added to the solution and what will its concentration be when the second anion begins to precipitate? Can the two ions be separated with 99.99% efficiency? (6pts) Ksp = 3.1 x 10-8 for Agl03 Ksp = 8.1 x 10-12 for Ag2CO3
Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb2+ and 0.0050 M Ag+. What is the concentration of silver when the lead (II) iodide just begins to precipitate? [Ksp (Pbi2) = 1.4 × 10–8; Ksp (Agi) = 8.3 × 10–17] Please show all work
What is the maximum concentration of Ag+ in HM 1x10-6 M) to precipitate Ag3PO4 without precipitating AgCl in a solution that is 0.005 M CI- and 0.005 M PO43-? AgCl Ksp 1.6 x 10 10 Ag3PO4 Ksp= 1.8 x 10-18
A solution contains .04 M Ca+, .04 M Zn2+, and .04 M Ni2+ ions. A) If you separate them using (NH4)2C2O2, which ion will precipitate first as an oxalate? Consider Ksp Values for CaC2O4, ZnC2O4, and NiC2O4. CaC2O4 Ksp = 1.3 x 10^-9 ZnC2O4 Ksp = 1.5 x 10^-9 NiC2O4 Ksp = 4.0 x 10^-10 B) Calculate the concentration of the oxalate ion when the first cation (Ca2+, Zn2+, or Ni2+ begins to precipitate. C) Explain why ZnC2O4 and NiC2O4...
If a 0.01 M Mn(NO3)2 solution has an ammonia concentration of 6.0 M, should a precipitate of Mn(OH)2 form? Calculate the ion product (reaction quotient) and compare it to Ksp to support your answer.
A solution of Na2SO4 is added dropwise to a solution that is 1.1×10−2 M in Ba2+ and 1.1×10−2 M in Sr2+. 1. What concentration of SO2−4 is necessary to begin precipitation? (Neglect volume changes. BaSO4:Ksp=1.1×10−10; SrSO4:Ksp=3.2×10−7.) 2. What is the concentration of SO2−4 when the second cation begins to precipitate?
Consider a solution that is 2.4×10−2 M in Fe2+ and 1.8×10−2 M in Mg2+. [K2CO3] = 1.3×10−9 M is the minimum concentration of K2CO3 is required to cause the precipitation of the cation that precipitates first What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitate? What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitate? Express your answer using two significant...