1 mole of cd2+ will add with 4 mold of cn-. Therefore, cd2+ is x and cn- is 4x
12. The Cd(CN), ion has a formation constant, Ky, of 3 x 1018. Ca²+ (aq) +...
12. The Cd(CN) 2-ion has a formation constant, Ky, of 3 x 100 ca?+ (aq) + 4CN- (aq) Ca(CN).- (aq) What is the concentration of CN in a 0.01 M aqueous solution of K Cd(CN)4?
urgentt 5) The molecular complex Cd(CN)d-dissociates in water by the process Ca(CN)"(aq) = Cd2+(aq) +4 CN- Kc = 1.3 x 10-7 The initial concentration of Cd(CN).- in an aqueous solution is 0.0360 M. No Cd2+ or CN-ions are initially present. What is the concentration of Cd2+ ion present when equilibrium is achieved? [12 points]
5) The molecular complex Cd(CN)42- dissociates in water by the process Ca(CN): (aq) = Cd?" (aq) + 4 CN Kc -1.3 x 10-17 The initial concentration of Ca(CN).?- in an aqueous solution is 0.0360 M. No Cd2+ or CN ions are initially present What is the concentration of Cdion present when equilibrium is achieved? [12 points)
the molecular complex Cd(CN)2-4 dissociates in water 5) The molecular complex Cd(CN).- dissociates in water by the process Cd(CN) ? (aq) 5 C&'(aq) + 4 CN Kc = 1.3 x 10-17 The initial concentration of Ca(CN)6?- in an aqueous solution is 0.0360 M. No cd or CN ions are initially present. What is the concentration of Cd²+ ion present when equilibrium is achieved? (12 points)
The formation constant* of [M(CN)2]-is 5.30 x 1018, where M is a generic metal. A 0.170 mole quantity of M(NO3) is added to a liter of 0.650 M NaCN solution. What is the concentration of M+ ions at equilibrium? [M2+] =
3. Iron(II) nitrate and hydrocyanic acid react to form the hexacyanoferrate(II) ion, [Fe(CN).]*(aq), with a formation constant of 1.438x10's. 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'(aq) solution, what is the concentration of CN'(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).] (aq), with a formation constant of 1.028x10”. This complex ion...
The formation constant, Kf, of Fe(CN)63-(aq), Fe3+(aq) + 6 CN-(aq) ⇌ Fe(CN)63-(aq), is 1.0 x 1042. What are the equilibrium concentrations of Fe3+(aq), CN-(aq), and Fe(CN)63-(aq) if we add 0.113 mol of Fe(NO3)3 to 1.000 L of a 0.965 M aqueous solution of NaCN? Assume the volume remains fixed at 1.000 L.
The formation constant* of [M(CN)2]– is 5.30 × 1018, where M is a generic metal. A 0.170-mole quantity of M(NO3) is added to a liter of 0.540 M NaCN solution. What is the concentration of M ions at equilibrium?
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...