A solution contains .04 M Ca+, .04 M Zn2+, and .04 M Ni2+ ions. A) If...
A solution contains 0.100 mM of Ni2+ and Zn2+. Hydroxyl ions are slowly added to this solution to precipitate either Ni(OH)2 or Zn(OH)2. Determine which ion precipitates first at the pH range from 0-14 and the range of OH- concentrations that will allow a clean separation of the two ions. Ksp for Ni(OH)2=6x10^-16 and for Zn(OH)2 Ksp=3x10^-16
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.
Consider a solution that is 1.3×10−2 M in Ba2+ and 1.8×10−2 M in Ca2+. Ksp(BaSO4)=1.07×10−10 Ksp(CaSO4)=7.10×10−5 *Part A: If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? A) Ba2+ (ANSWER) B) Ca2+ *Part B: What minimum concentration of Na2SO4 is required...
please solve and show work! A solution of 0.10 M (each) Ni2+ and Cu2+ are separated using selective precipitation by the addition of solid Na2CO3. Assuming no volume change upon this addition, how much of the first precipitated ion remains at the point where the second ion begins to precipitate? Ksp of NiCO3 = 1.4'10-7 Ksp of CuCO3 = 2.510-10 A. 1.4 x 10-6 M CUCO3 B. 1.2 x 102 M CUCO3 C. 1.8x 10-4M NICO D. 1.4 x 106...
Question 4 1 pts A solution has 0.10 M of Ni2+ and 0.10 Mof Ca2+. When Na2CO3 is added to the solution, which compound will precipitate first? Ksp (NICO3) = 1.4 x 10-7 Ksp (CaCO3) = 8.7x10-9 NaCO3 NICO o Сасоз Nica CaNa
You are using gravimetric analysis to determine the concentration of calcium (Ca2+) in tap water. The calcium is precipitated as calcium oxalate monohydrate upon addition of ammonium oxalate to the tap water according to the following reaction: Ca +2 (aq) + C2O4 -2 (aq) → CaC2O4 ∙H_2 O (s) Ksp = 1.3 x 10 -8 The protocol calls for addition of 25 mL of 1.0 M ammonium oxalate to 25 mL sample. In order to ascertain the accuracy of your...
A solution of Na3PO4 is added dropwise to a solution that is 0.0353 M in Ca2+ and 1.43e-08 M in A13+ The Ksp of Ca3(PO4)2 is 2.07e-33. The Ksp of AlPO4 is 9.84e-21. (a) What concentration of PO4 is necessary to begin precipitation? (Neglect volume changes.) [PO3) = (b) Which cation precipitates first? Ca A13+ (c) What is the concentration of PO43- when the second cation begins to precipitate? (PO43-] = M.
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...
b, When blood is donated, sodium oxalate solution is used to precipitate Ca2+, which triggers clotting. A 114.0−mL sample of blood contains 9.70 × 10−5 g Ca2+/mL. A technologist treats the sample with 100.0 mL of 0.1550 M Na2C2O4. Calculate [Ca2+] after the treatment. (CaC2O4 · H2O Ksp = 2.30 ×10−9) Enter your answer in scientific notation.
A solution contains 0.0500 M Co2+and 0.0500 M Ni2+. Is it possible to lower the concentration of Co2+by 99.9% without precipitating Ni2+by adding Na2CO3to the solution? Ksp,CoCO3= 1.0 x 10-10and Ksp,NiCO3= 1.3 x 10-7 Please show work so I can understand why this is the answer! Answer: Yes, it is possible. (QNiCO3 < Ksp,NiCO3, no precipitation)