What is the iron II concentration when KCN is added to a 0.100 M solution of Fe(CN)64- if the cyanide ion concwntration at equilibrium is 0.50 M?
I know the answer is 6.41x10-35, but unsure how to get the answer.
What is the iron II concentration when KCN is added to a 0.100 M solution of...
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...
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...
please help What is the approximate concentration of free Cu* ion at equilibrium when 1.57x102 mol copperII) nitrate is added to 1.00 L of solution that is 1.380 M in NH3. For [Cu(NH3)4j2, Kf 2.1 1013 [Cu2 м What is the approximate concentration of free Fe2* ion at equilibrium when 1.42x102mol iron(II) nitrate is added to 1.00 L of solution that is 1.38so M in CN. For [Fe(CN)6]4, Kf=1.0x1035 [Fe"]= In the presence of excess OH, the Al*(aq) ion forms...
The equilibrium concentration of iron(II) ion in a saturated iron(II) sulfide solution is M .
Solid iron(II) nitrate is slowly added to 150 mL of a 0.0529 M ammonium sulfide solution. The concentration of iron(II) ion required to just initiate precipitation is ? M please double check and make sure it is right please because i cant afford to get this wrong
3. When C12(g) is added to aqueous K4[Fe(CN).), [Fe(CN)]*- is oxidized to [Fe(CN).]>- and K:[Fe(CN)] precipitates, as shown below. 2K.[Fe(CN),](aq) +Cl2(g) = 2Ks[Fe(CN)2](3) + 2Cl(aq) a. Write the net ionic equation for the reaction and calculate its equilibrium constant. (10 pts) At 25°C [Fe(CN).J” (aq) + € → [Fe(CN).]" (aq) E = 0.356 V Cl2(g) + 2e → 2Cl(aq) E* = 1.360 V Kup of Kj[Fe(CN).] = 106.5 Answer: b. When 80.0 mL of 1.00 M KCN is added to...
3. When Cl2(g) is added to aqueous K [Fe(CN)6], [Fe(CN).]*- is oxidized to [Fe(CN).]}-and K [Fe(CN)6] precipitates, as shown below. 2K [Fe(CN).] (aq) + Cl2(g) = 2K3[Fe(CN).J(8) + 2Cl(aq) a. Write the net ionic equation for the reaction and calculate its equilibrium constant (10 pts) At 25°C: [Fe(CN).]" (aq) + e[Fe(CN).]" (aq) E° = 0.356 V Cl2(9) + 2e → 2Cl(aq) E° = 1.360 V Ksp of K3 [Fe(CN)6] = 106.5 b. When 80.0 mL of 1.00 M KCN is...
What is the equilibrium Fe2+ concentration when 2.15 L of a 0.144 M iron(II) iodide solution are mixed with 1.94 L of a 0.291 M potassium carbonate solution? [Fe2+] = M
A solution contains 1.34*10-2 M nickel(II) nitrate and 8.49x10-3 M zinc acetate. Solid potassium cyanide is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula B. What is the concentration of cyanide ion when this precipitation first begins? [CN) - M