number of moles of Ni(NO3)2=0.020
number of moles of NH4OH=0.22
NH4OH is in excess so the product obtained will be 0.020mole
[Ni(NH3)4]2+ ------> Ni2+ + 4NH3
0.02 -
x
x
4x
kd=x*4x/0.02 - x =1.1x10^-8(neglecting x in the denominator)
x=7.416x10^-6=concentration of Ni2+
Calculate the Ni+2 concentration of a solution made by mixing 0.020 mole of solid Ni(NO3)2 into...
22. What will be the concentration of Ni in a solution that is made at 25°C and a high pH by adding 1.0 mL of 0.250 M Ni(NO3)2 to 100 mL of 0.058 M ammonia? You can assume that all of the Ni(NO3)2 originally dissolves to pro- duce Ni2+ and NO3 and that the value of [NH3] at equilib- rium is approximately equal to the analytical concentration of ammonia.
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+...
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)
20. A solution is made 0.020 M in Cu(NO3)2 and 0.40 M in NH3. After the solution reaches equilibrium, what concentration of Cu'* ions remains? The Kr for Cu(NH342* is 1.7x1013 16
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
i just want to know if i need to divide the concentration for Ni(NO3)2 in half because the molar ratio isnt 1:1. i dont need this problem to be solved. 2. Consider a 100.0 mL sample of 0.0200 M NI(NO3)2. Then 10.0 mL of 0.300 M NH3 is added. What are the molar concentrations of Ni2+, NH3, and (Ni(NH3).]” at equilibrium? (8 pts) K for [Ni(NH3).)?* = 2.0 x 108
5. A solution is made 1.1 x 103 M in Zn(NO3)2 and 0.150 M in NH3. After the solution reaches equilibrium, what concentration of Zn2 (aq) remains?
One millimole of Ni(NO3)2 dissolves in 230.0 mL of a solution that is 0.300 M in ammonia. The formation constant of Ni(NH3)62+ is 5.5×108. What is the initial concentration of Ni(NO3)2 in the solution? I already have this answer which is 4.35E-3, but I cannot figure out the second part which is: What is the equilibrium concentration of Ni2+(aq ) in the solution? and the answer IS NOT 1.08E-8
One millimole of Ni(NO3)2 dissolves in 230.0 mL of a solution that is 0.500 M in ammonia.The formation constant of Ni(NH3)62+ is 5.5×108. What is the initial concentration of Ni(NO3)2 in the solution? What is the equilibrium concentration of Ni2+(aq ) in the solution?
2. You mix a 105.0 mL sample of a solution that is 0.0114 M in Ni(NO3)2 with a 190.0 mL sample of a solution that is 0.300 M in NH3. After the solution reaches equilibrium, what concentration of Ni2+ remains? The value of Kr for [Ni(NH3)6]2+ is 2.0x108.