17.78 Copper(II) ferrocyanide, Cu2Fe(CN)6, dissolves to give and [Fe(CN)6Jions; Kgp for Cu2Fe(CN)6 equals 1.3 X 10-...
The solubility product constant of Ag4[Fe(CN)6] is Ksp = 1.55 x 10–41. Select the expression for the solubility product constant. Let x be the molar solubility. A. Ksp = [Ag+]4[Fe(CN)6-4] = 256x5 B. Ksp = [Ag+]4[Fe(CN)6-4] = x4 C. Ksp = [Ag+]4[Fe(CN)6-4] = x5 D. Ksp = [Ag+][Fe(CN)6-4] = x2
Calculate the solubility (in moles per liter) of Fe(OH)3 ( Ksp = 4 x 10-38) in each of the following. a. water Solubility = mol/L b. a solution buffered at pH = 6.0 Solubility = mol/L c. a solution buffered at pH = 11.0 Solubility = mol/L Approximately 0.15 g cadmium(II) hydroxide, Ca(OH),(s), dissolves per liter of water at 20°C. Calculate Ksp for Ca(OH)2(s) at this temperature. Kp =
The molar solubility of copper (II) iodide, Cul2 in water is 3.5 x 10-2 M. What is the KSP of copper (II) iodide? Cul2 (s) <-------...--> Cu2+ + 21 a. 4.9 x 10-3 b.1.7 x 10-4 M c. 4.3× 10-5 d. 8.1 x 10-3 e. 6.4×106 Estimate AGºrxn for the following reaction at 298 Kelvin tempeature.. HCN(g) + 2 H2(g) → CH3NH2(g) Given : AH°= -80.0 k); AS°= 180 JK a. 134 kJ b. - 134 k) C. - 26.4...
16. The Ksp value for copper (1) bromide, CuBr, is 63 x 10. What is the solubility (in water) of this compound in grams per liter? Pr= 79.90 741 -t0
3D 7.9 х 10-16. Calculate the molar solubility of Fe(OH)2 in a buffer solution where the pH has been fixed at the indicated values. Kgp (а) рH 7.1 М (b) рH 10.4 1.Зе-8 M (с) рH 12.7 M
Iron(II) nitrate and hydrocyanic acid react to form the hexacyanoferrate(II) ion, [Fe(CN)6] -4 (aq), with a formation constant of 1.438x1035 . This complex ion has an intense blue color in solution . a. If you add 182.734g of iron(II) nitrate solid to 750.0mL of 0.8324M CN-1 (aq) solution, what is the concentration of CN-1 (aq) still in solution when the reaction reaches equilibrium? b. Copper(II) also forms a complex ion with cyanide ions, tetracyanocuprate(II) ion, [Cu(CN)4] -2 (aq), with a...
Iron(II) nitrate and hydrocyanic acid react to form the hexacyanoferrate(II) ion, [Fe(CN)6] -4 (aq), with a formation constant of 1.438x1035 . This complex ion has an intense blue color in solution . a. If you add 182.734g of iron(II) nitrate solid to 750.0mL of 0.8324M CN-1 (aq) solution, what is the concentration of CN-1 (aq) still in solution when the reaction reaches equilibrium? b. Copper(II) also forms a complex ion with cyanide ions, tetracyanocuprate(II) ion, [Cu(CN)4] -2 (aq), with a...
Calculate the molar solubility of Fe(OH)3 if its Ksp equals 4.0 × 10 38. A) 2.0 × 10 10 M B) 2.6 × 10 10 M C) 4.5 × 10 10 M D) 1.2 × 10 19 M E) 2.0 × 10 19 M
Copper can be cemented onto iron particles by the reaction. Cu2+ + Fe = Cu + Fe2+. A dilute copper solution containing 0.50 g/L of copper is flowed continuously at a rate of 1 m3/h through a stirred tank reactor of volume 10 m3 containing 10 kg of suspended spherical iron particles with a diameter of Imm. The mass transfer coefficient of Cu2+ is 6 x 10-3 cm sl. (i) Calculate the concentration of copper ions in the discharge solution...
The solubility of iron (II) hydroxide, Fe(OH)2, is 1.43 x10–3 gram per litre at 25 0C. (a) Write a balanced equation for the solubility equilibrium. (b) Write the expression for the solubility product constant, Ksp, and calculate its value. (c) Calculate the pH of a saturated solution of Fe(OH)2 at 25 0C. (d) A 50.0 millilitre sample of 3.00x10–3 molar FeSO4 solution is added to 50.0 millilitres of 4.00x10–6 molar NaOH solution. Does a precipitate of Fe(OH)2 form? Explain and...