Determine the concentration of Ag+ in a solution prepared by adding 0.10 mol AgNO3 to 1.0 L of 3.5 M NH3. Ag+(aq) + 2 NH3(aq) left right double arrow Ag(NH3)2+(aq) Kf= 1.7 x 107
Determine the concentration of Ag+ in a solution prepared by adding 0.10 mol AgNO3 to 1.0...
What is the “free” silver ion concentration in a solution that was (pre-equilibrium) 0.10M AgNO3(aq) and 0.50M NH3(aq)? Kf for [Ag(NH3)2]+ = 1.7x107.
Find the pH of a solution prepared by adding 1.0 L of 0.10 M butyric acid to 0.50 L of 0.10 M NaOH. (Ka = 1.5 x 10-5) A. 12.69 B. 7.00 C. 2.41 D. 4.82 E. 13.35
Calculate the equilibrium concentration of Ag (aq) in a solution that is initially 0.140 M AgNO3 and 0.600 MNH3, and in which the following reaction takes place: Ag (ag)+2NH3 CaAg(NH3(aq) (K-1.7010) M Agt
Calculate the equilibrium concentration of Ag+ (aq) in a solution that is initially 0.200 M AgNO3 and 0.200 M KCN. The formation constant for [Ag(CN)2] (aq) is Ka= 1.0 x 10^21. Show your work for each step. a. 5.6 x 10^-22 M b. 5.0 X 10^-22 M c. 3.3 x 10^-33 M d. 1.0 x 10^-30 M e. 1.3 x 10^-21 M
23. A solution is prepared by adding 0.10 mole of Ni(NH3). Cl2 to 0.50 L of 3.2 M NH3. Calculate (Ni (NH3)&2+) and (Ni2+in this solution. Koveralt for Ni (NH3)22+ is 5.5 x 108. That is, 5.5 x 108 = Ni (NH3) 2+1 [Ni2+] [NH3] for the overall reaction Ni2+ (aq) + 6NH3(aq) = Ni (NH3). 2+ (aq) (Ni (NH3), 2+] = 0 [Ni2+] = C M
To determine the solubility product, Ksp, for Ag2CO3, 1.00 mL of 1.00 mol/L Na2CO3(aq) and 1.00 mL of 0.100 mol/L AgNO3(aq) were combined. The mixture was stirred for 10 minutes to ensure that equilibrium had been reached. A voltaic cell was constructed to determine the concentration of soluble Ag (aq) ions left in solution at equilibrium, and [Ag leg was thus found to be 2.0 x 10-7 mol/L. Calculate the equilibrium concentration of CO32-(aq) ions left in solution at equilibrium,...
4- (a) Calculate the concentration of Cd2+ ion in a solution prepared by mixing 2.0 mL of 1 M CA(NO3)2 solution with 1.0 L of 4.0 M NH3 solution. [Assume that the volume does not change after the addition of 2.0 ml of 1 M Cd(NO3)2] (b) Will you be able to see Ca(OH)2(6) precipitate in the solution? (Kr for Ca(NH3)42+ = 1.0 x 107, Kb for NH3 = 1.8 x 10-5; Ksp for Ca(OH)2 = 5.9 x 10-15 Cd2+...
2+ What is the concentration of Co (aq) ions in the solution made by adding water to cobalt(II) nitrate (0.50 mol) and ethylenediamine (3.0 mol) so that the final volume of solution is 3.0 L? The Kstab of [Co(en)s]2 is 1.0 x 1014 4. а) 1.3 х 10-14м 15 b) 1.5 x 10 M 15 М c) 2.9 x 10 15 d) 3.3 x 10 -16 e) 8.7 x 101 M 2+ What is the concentration ofZn (aq) ions in...
5. In the hood, form solid AgCl by adding 1 mL of 6 M HCI (aq) to 1 mL of 0.1 M AgNO3 (aq) in a medium test tube, and then add 1 drop of 15 M NH3 (aq) to establish the equilibrium shown below. AgCI (s) +2 NH3 (aq)Ag(NH3)2 (aq)+CI (aq) Stress 1. Add reactant. Stress 2. Add product. action observation shift right or left Stress 1 Stress 2 What happens to the concentration of CI as reactant is...
Finding concentration... Help 6. What is the concentration of Zn²+ (aq) ions in the solution made by adding water to zinc nitrate (0.10 mol) and ammonia (3.0 mol) so that the final volume of solution is 1.5 L? The Kstab of [Zn(NH3)4]2 is 7.8 x 108 a) 4.9 x 10-'M b) 9.5 x 10-2 M c) 6.1 x 10-2 M d) 2.8 x 10-2 M e) 2.3 x 10-13 M