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please solve and show work! A solution of 0.10 M (each) Ni2+ and Cu2+ are separated...
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
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)
A precipitate forms when a solution that is 0.10 M in Cu2+, Pb2+, and Ni2+ is saturated with H2S and adjusted to pH = 1. What sulfides are present in the precipitate? [H2S] = 0.10 M; for H2S, Ka1 ´ Ka2 = 1.1 ´ 10–24 Ksp: CuS = 8.5 ´ 10–45, PbS = 7.0 ´ 10–29, NiS = 3.0 ´ 10–21 (The answer is D, Could anyone explain it by steps?) A) CuS, PbS, and NiS B) PbS and NiS...
It is of interest to decide if an analytical separation of the metal ions can be effected by selective precipitation of carbonates from a solution that is 0.102 M in Cu²+ and 0.110 Min Ni2+ NiCO3 CuCO3 Ksp = 6.60X10-9 K = 2.50X10-10 To analyze this problem, answer the following questions. (1) What carbonate concentration is needed to precipitate 99.9% of the metal that forms the least soluble carbonate? C M (2) When 99.9% of the least soluble carbonate has...
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...
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.
8) Calculate the following for 2.0 L solution containing [Ag+] = 0.100 M and [Pb2+] = 0.100 M. Assume no volume changes. (AgCl Ksp = 1.8 x 10-10, PbCl2 Ksp = 1.8 x 10-5). a) At what [Cl-] will each salt precipitate? b) What percent of the Ag+ has precipitated before the Pb2+ begins to precipitate? c) How much sodium chloride must be added (in grams) to precipitate a maximum AgCl before before any PbCl2 begins to precipitate?
It is of interest to decide if an analytical separation of the metal ions can be effected by selective precipitation of carbonates from a solution that is 9.11×10-2 M in Cu2+ and 0.100 M in Ca2+. CaCO3 Ksp = 3.80×10-9 CuCO3 Ksp = 2.50×10-10 To analyze this problem, answer the following questions. (1) What carbonate concentration is needed to precipitate 99.9% of the metal that forms the least soluble carbonate? __M (2) When 99.9% of the least soluble carbonate has...
A solution contains 0.020 M Mg2+ and 0.10 M Ca2+. Can 99.90% of Mg2+ be precipitated by addition of NaOH without precipitation of Ca2+? Note: use Ksp = 7.1 x 10-12 for Mg(OH)2 Ksp= 5.5 x 10^-6 CaOH2
A solution of Na2CO3 is added dropwise to a solution that contains 1.00×10-2 M Fe2+ and 1.49×10-2 M Cd2+. What concentration of CO32- is need to initiate precipitation? Neglect any volume changes during the addition. Ksp value: FeCO3: 2.10*10-11 Ksp value: CdCO3: 1.80*10-14 Which cation precipitates first? What is the concentration of CO32- when the second cation begins to precipitate?