When K2S is added to a saturates solution of FeS, what happens to the solubility of FeS? (a) More FeS will dissolve in the solution due to the presence of additional S2- (b) there will be no change in the solubility of FeS (c) some FeS will precipitate out of the solution due to the presence of additional S2- (d) more FeS will dissolve in sultion due to the presene of K+ (e) some FeS will precipitate out of the solution due to the oresence of K+

When K2S is added to a saturates solution of FeS, what happens to the solubility of FeS? (a) More FeS will dissolve in the solution due to the presence of additional S2- (b) there will be no change in the solubility of FeS (c) some FeS will precipitate out of the solution due to the presence of additional S2- (d) more FeS will dissolve in sultion due to the presene of K+ (e) some FeS will precipitate out of the solution due to the oresence of K+

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter27: Relative Stabilities Of Complex Ions And Precipitates Prepared From Solutions Of Copper(ii)

Section: Chapter Questions

Problem 1ASA

See similar textbooks

Similar questions

(a) If the molar solubility of Cu3(PO4)2 at 25 oC is 1.67e-08 mol/L, what is the Ksp at this temperature?Ksp = _______(b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3?solubility = ______ mol/L
In photography, unexposed silver bromide was removed from film by soaking the film in a solution of sodium thiosulfate, Na2S2O3. Silver ion, Ag+, forms a soluble complex with the thiosulfate ion, S2O3-2, that has a formula of Ag(S2O3)2-3, and the formation of the complex causes the AgBr in the film to dissolve. The formation of the complex has a Kf of 2.0 x 10^13 while the Ksp of AgBr is 5.0 x 10^-13. How many grams of AgBr will dissolve in 125 mL of 1.20 M Na2S2O3 solution?
In the presence of aqueous cyanide, cadmium(II) ions will form the complex Cd(CN)42- .Determine the molar concentration of free (uncomplexed) cadmium(II) ion in solution when 47.3g of Cd(NO3)2 is dissolved in 1 liter of 2.0M sodium cyanide Given: Kf of Cd(CN)42- @25 degrees C is 7.1x1016
A 0.0300 M solution in Ni (N03) 2 and 0.15 M in the cyanide anion (CN-) is prepared. Ni2 + and CN- form the complex ion [Ni (CN) 4] 2-. If the dissolution is also 0.20 M in S2-, Will NiS (s) precipitate? NiS, Ksp = 3.2 · 10-19; [Ni (CN) 4] 2-, Kf = 2 · 1031
You want to separate Cd2* and Fe2+ (initial concentration 103 mol/L) by means ofprecipitation of the corresponding sulphides. Is therea pH range in which one of the two metals is precipitated quantitatively(concentration in the solution less than or equal to 10" mol/L) is precipitatedwhile the other is still completely_in solution?Calculate and name this pH range where pH values below 0are set equal to O. Illustrate the situation graphically by drawing
Explain why the addition of NH3 or HNO3 to a saturated solution of Ag2CO3 in contact with solid Ag2CO3 increases the solubility of the solid.
Compare the solubility of nickel(II) carbonate in each of the following aqueous solutions: 0.10 M Ni(CH3COO)2 0.10 M (NH4)2CO3 0.10 M KNO3 0.10 M NH4CH3COO More soluble than in pure water. Similar solubility as in pure water. Less soluble than in pure water.
Fill in the blank: excess hydroxide ions must be neutralized with oxalic acid. The oxalic acid will alsoneutralize the hydroxide ions of the iron (III) hydroxide precipitate, releasing the iron(III)ion back into solution. Oxalic acid is chosen so that no additional anions will be present tointerfere with the formation of the complex. The excess oxalate ions convert all iron presentinto a soluble complex ion with three oxalate ions attached to the iron(III) ion.____ Fe(OH)3 (s) + ___________ (aq) → ____( ) + ___ H2O ( ) + ______ ( )
The Kf for the complex ion Ag(S2O3)23− is 2.9 x 1013. The Ksp for AgI is 8.5 x 10−17. What is the molar solubility of AgI in a solution that is made by adding Na2S2O3 to make the solution 2.0 M in Na2S2O3?
Consider the insoluble compound silver iodide , AgI . The silver ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of AgI (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction.For Ag(NH3)2+ , Kf = 1.6×107 . Be sure to specify states such as (aq) or (s). + + K =
The overall K, for the complex ion Ag(NH3)2 is 1.7 x 107. The Rp for Agl is 1.5 x 10-16 What is the molar solubility M in NH3? 8.4 x 10-5 O 1.5×10 9 O1.0 × 10 -4 O 5.8 x 10-12 O 1.3 x 10