Calculate the concentration of the free copper (II) that is in equilibrium with the complexed copper (II) ion, Cu(NH3)42+ in the solution. Does the calculated value make sense and what does it imply?
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Calculate the concentration of the free copper (II) that is in equilibrium with the complexed copper...
What is the approximate concentration of free Cu2+ ion at equilibrium when 1.22x102 mol copper(II) nitrate is added to 1.00 L of solution that is 1.210 M in NH3. For [Cu(NH3)4]. Ke-2.1x1013 (Cu?") - Submit Answer Determine ion concentration when separating ions in a mixture. A solution contains 1.58x102 M lead acetate and 1.58x10 ? Mmanganese(II) nitrate. Solid sodium sulfide is added slowly to this mixture. What is the concentration of lead ion when manganese(II)ion begins to precipitate? Solubility product...
1- What is the approximate concentration of free Cu2+ ion at equilibrium when 1.71×10-2 mol copper(II) nitrate is added to 1.00 L of solution that is 1.310 M in NH3. For [Cu(NH3)4]2+, Kf = 2.1×1013. [Cu2+] = ------ M
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...
Consider the insoluble compound copper(II) hydroxide , Cu(OH)2 . The copper(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Cu(OH)2 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Cu(NH3)42+ , Kf = 6.8×1012 . Use the pull-down boxes to specify states such as (aq) or (s). + + K = Submit Answer Voit needed for this question. Consider the insoluble...
Solid copper(II) carbonate and solid copper(II) sulfide are in equilibrium with a solution containing 1.12×10-2 M sodium carbonate. Calculate the concentration of sulfide ion present in this solution. [sulfide] = M
Calculate the equilibrium molar concentration of free Zn2+(aq) in a solution that contains 0.021 mol of Zn2+ per liter to which 0.498 mole of NH3 is added. Kf for Zn(NH3)42+ is 2.9x109. Show the equilibrium equation.
Indicate whether the following would increase or decrease the solubility of copper(II) hydroxide. It may help to know that copper(II) ion forms a complex ion with ammonia: Cu2+ (aq) + 4 NH3 (aq) ⇌ Cu(NH3)42+ (aq). adding 50.0 mL of a solution of 0.25 M sulfuric acid adding 50.0 mL of a solution of 6.0 M ammonia
18. A 200.0-mL sample of a 0.0015 M copper(II) nitrate solution is mixed with a 250.0-mL sample of 0.20 M NH3. After the solution reaches equilibrium, what concentration of copper(II) ion remains? You will have to look up the appropriate complex formation constant.
Worksheet 17c (Gen Chem) Other Equilibria - Calculate the free cobalt(II)ion concentration in a solution that is initially 0.010 M cobalt(II) nitrate and 1.00 M ammonia. (Hint: assume 1 L of solution). How does decreasing the pH affect the free cobalt(II) id concentration? Explain.
Copper(II) carbonate is very poorly soluble in water, but better soluble in NH3(aq) due to the formation of the Cu(NH3)4 2+ complex: CuCO3(s) + 4NH3(aq) ⇄ Cu(NH3)4 2+ (aq) + CO3 2- (aq) CuCO3 (Ksp = 2.3·10-10 ) and the formation constant for Cu(NH3)4 2+ (Kf = 5.0·1012) What was the initial concentration of NH3(aq), if 0.010 mol of CuCO3(s) dissolved at equilibrium in 1.00 L of this solution? [Consider the change in the volume of solution negligible.]