1.Given a solution in which [Cu2+] = 0.20 mol/L and [NH3] = 1.40 mol/L, what is the equilibrium concentration of free Cu2+? The complex Cu(NH3)42+ has Kf = 5.0 X 1013. The answer to the question is 3.1 X 10 -14 I just need how to do it with the work shown.
2. You titrate a 20.00 mL sample of ammonia (Kb = 1.8 X 10-5) to the equivalence point using 10.00 mL of .20 M HCl solution. What is the pH of the solution at the equivalence point of the titration. The answer to the question is 5.21 but I do not know how to get there.
1.Given a solution in which [Cu2+] = 0.20 mol/L and [NH3] = 1.40 mol/L, what is...
Calculate [Cu2+] at equilibrium when 0.20 mol of CuSO4 is added to 1.000 L of 1.20 M NH3 solution. Kf for [Cu(NH3)4]2+ is 5.0 × 1013.
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
a) What is the pH of a solution that consist of 0.20 M ammonia, NH3, and 0.20 M ammonium choride, NH4Cl? (Kb for ammonia is 1.8 x 10-5) b) 1.25 g of benzoic acid (C6H5CO2H) and 1.25 g of sodium benzoate (NaC6H5CO2) are dissolved in enough water to make 250 mL solution. Calculate the pH of the solution using the Handerson-Hasselbach equation (Ka for benzoic acid is 6.3 x 10-5). c) What is the pH after adding 82 mg of...
Consider titration of 20.0 mL of 0.100 M NH3 with 0.200 M HCl solution. Calculate the pH after the addition of the following volumes of HCl solution. The Kb of NH3 = 1.8 x 10^5 a. 0.00 mL b. 6.00 mL c. 10.00 mL d. 20.00 mL
1)A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid.Kb of NH3 is 1.8 × 10−5.Henderson–Hasselbalch equation:Part a):1) After adding 10 mL of the HCl solution, the mixture is [ Select ] ["at", "before", "after"] the equivalence point on the titration curve.2) The pH of the solution after...
Question 6 1 pts A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid. Ko of NH3 is 1.8 x 10-5 Henderson-Hasselbalch equation: pH = pka + log og HCI NH, NH3- Parta): 1) After adding 10 mL of the HCl solution, the mixture is (Select] the equivalence...
A 25.0 mL solution of 0.817 mol L-1 NH3 is titrated using 0.669 mol L-1 HCl. What volume of NaOH (in mL) is needed to reach the equivalence point in this experiment?
e equivalen 26 Calculate the pH at the equivalence point for the titration of 0.20 M HCl with 0.20 M NH3 (Kb = 1.8 x 10-5). B. C. 2.87 4.98 5.12 7.00 D. E. 11.12 inn of 100 mL of 0.10 M HCl
What is the pH of a solution containing 0.342 mol L-1 NH3 and 0.140 mol L-1NH4? Round your answer to 2 decimal places. Remember you can find KA and/or Kg values in your textbook in chapter 15. Answer: Check A 45.3 mL solution of 0.283 mol L-1 HCl is titrated using 0.820 mol L-'NaOH. What volume of NaOH (in mL) is needed to reach the equivalence point in this experiment? Remember you can find KA and/or Ke values in your...
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...