A solution contains 0.021 M Cl? and 0.017 M I?. A solution containing copper (I) ions is added to selectively precipita...
Excess solid Na₂CO₃ is added to a solution containing 0.400 M (each) Mg²⁺ and Zn²⁺ ions. Ksp for MgCO₃ is 3.50 × 10⁻⁸ and Ksp for ZnCO₃ is 1.00 × 10⁻¹⁰. ZnCO₃, with the smaller Ksp, will be the least soluble and will begin precipitating first. What will be the [Zn²⁺] concentration when MgCO₃ just begins to precipitate? (Assume no volume change upon addition of the solid Na₂CO₃).
A solution is 5.0 x 10-M in each of these ions: Ag+, so -, Cl, and co . Which precipitate will form? Ag2SO4 (Ksp = 1.12 x 10-5) AgCl (Ksp = 1.77 x 10-10 Ag2CO3 (Ksp = 8.46 x 10-12)
A solution contains 0.10 M concentrations of Ba2+, Ca2+, and Sr2+. Na2CO3 is slowly added to the solution. In what order will the ions begin to precipitate? What is the concentration of the first ion when the 2nd begins to precipitate? Ksp for BaCO3 = 2.58 x 10-9, for CaCO3 = 3.36 x 10-9, and for SrCO3 = 5.60 x 10-10.
Determine whether a precipitate form in the following reaction conditions: a. A solution containing lead (II) nitrate is mixed with one containing sodium bromide to form a solution that is 0.0150 M in Pb(NO3)2 and 0.00350 M in NaBr. Does a precipitate form in the newly mixed solution? Ksp PbBr2 = 4.67 x 10-6 . b. A solution containing iron (II) nitrate is mixed with one containing sodium phosphate to form a solution that is 0.0365 M in Fe(NO3)2 and...
A solution is 5.0 x 10-5 M in each of these ions: Agt, s02-, Cl-, and CO2- Which precipitate will form? AgCl (K sp = 1.77 x 10-19 Ag2CO3 (Ksp = 8.46 x 10-13) Ag2SO4 (Ksp = 1.12 x 10-5)
you have three flasks with 0.03 M Cl- , Br- I- if you have titrated each solution with Cu+ what order with the equivalence points appear in the titration curves? Ksp for CuI=1*10-12 Ksp for CuCl=1.9*10-7 Ksp for CuBr = 5 * 10-9 A. pCu+ (I-) < pCu+(Br-)<pCu+(Cl-) B.pCu+ (Cl-) < pCu+(Br-)<pCu+(I-) C.pCu+ (Br-) < pCu+(I-)<pCu+(Cl-)
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...
Determine the molar solubility of CuCl in a solution containing 0.030 M LiCl. Ksp (CuCl) = 1.7×10-7. Determine the molar solubility of CuCl in a solution containing 0.030 M LiCl. Ksp (CuCl) = 1.7×10-7. 4.1×10-4 M 2.9×10-14 M 5.7×10−6 M 5.1×10−9 M 4.7×10−5 M
2. (5 pts) A solution contains lead (II), copper(I) and silver ions. An HCl solution is used to precipitate out each ion, one at a time, to be separated. What are the chemical formulas of each precipitate and, in what order will the ions precipitate? For credit explain your reasoning in determining the order.
Lead(II) nitrate is added slowly to a solution that is 0.0100 M in Cl^- ions. Calculate the concentration of Pb^2+ ions (in mol/L) required to initiate the precipitation of PbCl2. (Ksp for PbCl2 is 2.40 X 10^-4.)