Answer
Concentration of NaX in 50 ml=[NaX]= {(50×8.9)/1000}Mole = 0.445 Mole
Concentration of CuNO3 in the solution = [ CuNO3 ] =
[{(6.2×10-3)×50}/1000}]moles = 3.1 ×10-4 moles
A solution is formed by mixing 50.0 mL of 8.9 MNaX with 50.0 mL of 6.2...
A solution is formed by mixing 50.0 mL of 9.6 MNaX with 50,0 mL of 1.0 x 108 M CuNO3. Assume that Cut forms complex ions with X as follows: Cu+ (aq) + X(aq) + CuX(aq) K1 = 1.0 x 102 CuX(aq) + X- (aq) + Cux,- (aq) Kg = 1.0 x 104 CuX2 - (aq) + X-(aq) = CuXg2- (aq) K3 = 1.0 x 108 with an overall reaction Cu" (aq) + 3X- (aq) + CuX, 2- (aq) K...
OWO References apter 15: EOC stion 16 A solution is formed by mixing 50.0 mL of 9.5 M/ NX with 50.0 ml. of 2.8 x 10-M CUNO, Assume that a forma complex ions with X as follows: stion 17 stion 18 stion 13 1 pt 1 pt pe tpt Cu (aq) +X-(e) CX(a) K -1.0 x 10' CX(g) + (aq) + Cux," () K -1.0 x 10" OuX;"(aq) + (aq) Cux, (a) Ks = 10 X 10' with an overall...
Chapter 15 COC Reference NO,Aume that Out forms complex ions with X as follows Destion 18 Destion 19 Question 20 A solution is formed by mixing 50.0 mL of 10.9 MNX with 500 ml of 8.6 x 10-M Out (g) + X() OXog K; -10 x 10 CuX(aq) + X() - Cux, (a) K; -1.0 x 109 CuX;" ) + X (a) Cux,- (aq) K; -1.0 x 100 with an overall reaction Cu* (eq) +3X" () - CuX; (aq) -10x10'...
A solution of 350 mL of 0.0470M Cu(NO3)2
are mixed with 1.2 L of 0.8 M Na2X, where X–
represents an unknown ion, acts as a ligand to form a complex ion
with the Cu2+ ion with a coordination number of two.
a) Calculate the equilibrium constant for the
following formation.
Cu2+ +
2X2–
[Cu(X)2]2–
Cu2+ +
X2– CuX
K1 = 1.96
× 104
[Cu(X)2] 2– CuX +
X2–
K2 = 3.88 ×
10–2...
A 50 mL sample of 2.2 x 10^-4 M CuNO3 is added to 50 mL of a 4.0 M NaCN. Cu^+ reacts with CN^- to form the complex ion Cu(CN)3^2- according to Cu^+(aq) + 3CN^-(aq) <--> Cu(CN)3^2- , Kf= 1.0 x 10^9 determine the concentrations of CN^-, Cu^+, Cu(CN)3^2- at equilibrium
A 50.0 mL sample of a 1.00 M solution of CuSO4 is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The temperature of both solutions was 20.3°C before mixing and 31.7 °C after mixing. The heat capacity of the calorimeter is 12.1 J/K. From these data, calculate AH for the process: CuSO4(1M) + 2KOH(2M) +Cu(OH)2 (s) + K2SO4(0.5M) Assume that the specific heat and density of the solution after mixing are the same as those of pure...
For questions 17 and 18. A solution is prepared by mixing 150.0 mL of 1.0 x 10 M AgNO3 with 200mL of 5.0M Na S O The stepwise formation equilibria are Ag +S203 Ag (S2O3) Ag(S2O3) +S20, Ag(S20s)2 17. What is the concentration of Ag(S203) in solution (5 points): A. 3.8x 10 B. 1.8 x 10 18 C. 4.3x 10 D. 5.6 x 10 K1 7.4 x 10 K2 3.9 x 104
5. A solution is made by mixing 200.0 ml of 1.5 x 10-4 M Cu(NO3)(aq) with 250.0 ml of 0.20 M NH3(aq). Calculate the concentration of copper ion (Cu? (aq)) in the solution when it reaches equilibrium. (Kr for [Cu(NH3)4]2+ = 1.7 x 1013)
23. What is the pH of the solution which results from mixing 50,0 ml. of 0.30 M HF(a) and 50.0 ml. of 0.30 M NaOH(aq) at 25 °C?(K, of HF 7.2 x 10") a. 1.98 b. 5.84 c. 8.16 d. 10.85 e. 12.02
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+...