A solution containing both Mn2+ and Cd²+ at 0.10M each is saturated with H2Sgas at 25ºC and 1 atm pressure. The [H+] is adjusted with HCl to 0.30M.a) Will the sulfides of these metals precipitate under these conditions?b) Calculate the maximum concentration of Cd2+ and Mn²+ that can remainin solution.Ksp for MnS = 1.0 x 10-13 ; Ksp for CdS = 1.0 x 10-26%3DIn a saturated solution of H2S at 1 atm and 25°C, [H2S] = 0.10M%3DKa1(H2S) = 5.7 x 10-8 ; Ka2 = 1.3 x 10-13

Given: Concentration of Mn2+ is [Mn2+] = 0.10 M Concentration of Cd2+ is [Cd2+] = 0.10 M The…

Answered: A solution containing both Mn2+ and…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 101QRT

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What mass of ZnS (Ksp = 2.5 1022) will dissolve in 300.0 mL of 0.050 M Zn(NO3)2? Ignore the basic properties of S2.
Calculate the solubility of copper(II) iodate, Cu(IO3)2 (Ksp = 7.4 108), in (a) water. (b) a 0.10 M copper(II) nitrate solution.
Calculate the molar solubility of AgBr in 0.035 M NaBr (KSP=51013).
The solubility of cadmium oxalate. CdC2O4, in 0.150 M ammonia is 6.1 103 mol/L. What is the oxalate-ion concentration in the saturated solution? If the solubility product constant for cadmium oxalate is 1.5 108, what must be the cadmium-ion concentration in the solution? Now calculate the formation constant for the complex ion Cd(NH3)42+.
Calculate the molar solubility of AgI in a 2.5 M NH3 solution if the Ksp for AgI is 8.5 x 10-17 and the Kf for [Ag(NH3)2]+ is 1.6 x 107.
A weighed sample of sodium nitrite was treated with 0.05 mol of ceric sulfate in solution, in air-free conditions. The resulting solution was titrated with standard Fe(II) solution and 0.01 mol of Fe(II) were required. Determine the moles of sodium nitrite present in the weighed sample. NO2– + 2 Ce4+ + H2O → NO3– + 2 Ce3+ + 2 H+ Fe2+ + Ce4+→ Fe3+ + Ce3+
Calculate the molar solubility of Mg(OH)2 in a solution of 0.050 M MgCl2 [Ksp for Mg(OH)2 = 5.6 × 10–12].
Can cadmium (II), and mercury (II) be separated quantitatively by precipitation as sulfides from a solution that is 0.15 M cadmium nitrate and 0.10 M in mercuric ions? If possible, what range of sulfide concentration is permissible? Do you expect any interference from the formation of hydroxides of both heavy metals? CdS (144.46); Ksp = 1.0 x 10 ^ -27HgS (232.66); Ksp = 2.0 x 10 ^ -53 HINT: Determine the concentration at which each of the cations start to precipitate out of solution. >Quantitative precipitation means 1/1000 remains in solution.
The solubility products of Fe(OH)3 and Ni(OH)2 are about 10-36 and 6 × 10-18, respectively. Find the approximate pH range suitable for the separation of Fe3+ and Ni2+by precipitation of Fe(OH)3 from a solution initially 0.01 M in each ion, as follows: (a) Calculate the lowest pH at which all but 0.1% of the Fe3+ will be precipitated as Fe(OH)3; (b) calculate the highest pH possible without precipitation of Ni(OH)2.
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The phosphate in a 3.00 g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO₃ (169.87 g/mol). The solution was filtered and the filtrate, upon addition of 1.00 mL of 0.01 M FeCl₃, required 18.23 mL of 0.1377 M KSCN for titration to the endpoint. Identify (a) what type of precipitation titrimetry was used (b) which served as the indicator (c) the color at the end point Calculate (d) the weight percent of phosphate (94.97 g/mol) in the detergent.
a. Calculate the molar solubility of AgBr in pure water.Ksp for AgBr is 5.0×10-13. b. Calculate the molar solubility of AgBr in 3.0 M NH3. The overall formation constant for Ag(NH3)2+is 1.7×107, that is, Ag+(aq) + 2NH3(aq) → Ag(NH3)2+(aq) K = 1.7×107 . c. Compare the calculated solubilities from parts a and b. Explain any differences. d. What mass of AgBr will dissolve in 250.0 mL of 3.0 M NH3? e. What effect does adding HNO3 have on the solubilities calculated in parts a and b?

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