a. From the solubility product of zinc ferrocyanide, Zn,Fe(CN)6, calculate the concentration of Fe(CN), in 0.10 mM ZNSO4 saturated with Zn2Fe(CN),- Assume that Zn,Fe(CN), is a negligible source of Zn²+. b. What concentration of K4FE(CN), should be in a suspension of solid Zn,Fe(CN), in water to give [Zn²+] =5.0 × 10-7 M?
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![a. From the solubility product of zinc ferrocyanide, Zn,Fe(CN),, calculate the
concentration of Fe(CN) in 0,10 mM ZNSO4 saturated with Zn2Fe(CN),-.
69
Assume that Zn,Fe(CN), is a negligible source of Zn?+.
b. What concentration of K4Fe(CN), should be in a suspension of solid
Zn,Fe(CN), in water to give [Zn²+] = 5.0 × 10-7 M?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc83a7a2f-cf2a-411d-9c16-3e7840bfda5e%2Fa41f5908-156f-450e-8682-6373ff710559%2F4abcevn_processed.jpeg&w=3840&q=75)
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- Will Mn(OH)2 precipitate from a 0.01 M solution of MnCl2 at pH = 9? Ksp(Mn(OH)2) = 1,0 x 10-13. Discuss from solubility diagrams and prove by calculation.calculation. Co is a metal that is present in every lithium battery to stabilize its charge and toincrease stability. Every cell phone, tablet and electric car relies on the availability ofcobalt, 97% of which is extracted from mines in places like the Congo, where essentially slave labor is used.Cobalt ions form complexes with e.g. CN- . You see solubility diagrams and fraction diagrams for CoCO3 with and without the addition of 10 mM CN- .. Explain whythe solubility of cobalt carbonate increases at high pH when cyanide ions are present.Write reaction formulas for the formation of the dominant cobalt cyanide complexes.Two hypothetical salts, LM2 and LQ, have the same molar solubility in H2O. If Ksp for LM2 is 3.20 × 10–5, what is the Ksp value for LQ?The solubility of lead (II) iodide is found to be .00130 M What is the Ksp for PbI2?
- Both silver(I) bromide and silver(I) iodide are slightly soluble salts, with Ksp values at 25°C of 5.40×10-13 and 8.30×10-17, respectively. A solution of silver(I) nitrate is added to a solution that is 0.504 M in both Br– and I–. What are the minimum Ag+ concentrations required for precipitation of AgBr and of AgI to occur? - AgBr = AgI = What percentage of the halide ion that is precipitated first remains in solution before the second begins to precip itate?Calculate the solubility at 25°C of AgBr in pure water and in 0.47M NaI . You'll probably find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits.Both silver(I) bromide and silver(I) iodide are slightly soluble salts, with Ksp values at 25°C of 5.40×10-13 and 8.30×10-17, respectively. A solution of silver(I) nitrate is added to a solution that is 0.504 M in both Br– and I–. What are the minimum Ag+ concentrations required for precipitation of AgBr and of AgI to occur? AgBr = Agl = What percentage of the halide ion that is precipitated first remains in solution before the second begins to precipitate?
- 2. 6 M HCI is added to a solution of Ag*, Cu²+, Fe3•. A white precipitate forms. Predict which ions are present. Make sure you explain and justify your answer. 3. What reagent(s) can be used to identify and confirm Ag*, Hgz2", and Pb2+ ions? Please answer both questions will give rating surelyCrO42- can be used as an indicator when Br- is titrated with Ag+. What concentration of CrO42- should be used so that Ag2CrO4(s) just starts to form at the equivalence point? If a concentration of 0.0010 M CrO42- is used instead, at what concentration of Br- will Ag2CrO(s) just start to precipitate? Do you think this is likely to introduce significant error? The Ksp for Ag2CrO4(s) is 1.2x10-12.When silver chromate, Ag2CrO4, dissolves in otherwise pure water, what is the relation between [Ag+] and [CrO42-]? The solubility product of Ag2CrO4 is 1.9x10-12. Show that its solubility in pure water is 0.78x10-4 M.
- Both silver(I) bromide and silver(I) iodide are slightly soluble salts, with Ksp values at 25°C of 5.40×10-13 and 8.30×10-17, respectively. A solution of silver(I) nitrate is added to a solution that is 0.434 M in bothBr– andI–. What are the minimum Ag+ concentrations required for precipitation of AgBr and of AgI to occur?AgBr mol/L AgI mol/L Which will precipitate first?Choose one AgBr AgI What percentage of the halide ion that is precipitated first remains in solution before the second begins to precipitate? % If complete separation is defined as there being less than 0.10% of a particular ion left in solution, does this method completely separate Br– from I–?Choose one: Yes No Cannot be determinedA 500 mL sample of a solution saturated at 25°C with calcium oxalate is evaporated to dryness, giving a 0.00305 gram residue of calcium oxalate. Calculate the solubility product constant for this salt at 25°C.Suppose ZnS(s) is saturated with 0.04 M K2S (K2S completely dissolves and ZnS has limited solubility) (Ksp for ZnS is 2x10-25). What is pZn by taking activity coefficients into consideration? a)10.4 b)22.4 c)9 d)26.7 e)7