What is the equilibrium concentration of Ni^2+ (aq) in the solution. If one millimole of Ni(NO3)2...

What is the equilibrium concentration of Ni^2+ (aq) in the solution. If one millimole of Ni(NO3)2 dissolves in 220.0 mL of a solution that is 0.300 M in ammonia?

Expert Solution

queen_honey_blossom answered 2 years ago

One millimole of Ni(NO3)2 dissolves in 210mL of a solution that is .500M in NH3. (a)...

One millimole of Ni(NO3)2 dissolves in 210mL of a solution that is .500M in NH3. (a) What is the initial concentration of Ni(NO3)2 in the solution? ------> The answer to (a) is .00476 M. I just can't figure out part (b) (b) What is the equilibrium concentration of Ni^2+(aq) in the solution? HINT: The Ni^2+ forms a hexammonia complex: Ni(NH3)6^2+. Kf = 5.5 x 10^8.

One millimole of Ni(NO3)2 dissolves in 260.0 mL of a solution that is 0.400 M in...

One millimole of Ni(NO3)2 dissolves in 260.0 mL of a solution that is 0.400 M in ammonia. The formation constant of Ni(NH3)62+ is 5.5×10^8. What is the equilibrium concentration of Ni2+(aq ) in the solution?

One millimole of Ni(NO3)2 dissolves in 210.0 mL of a solution that is 0.500 M in...

One millimole of Ni(NO3)2 dissolves in 210.0 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 equilibrium concentration of Ni2+(aq ) in the solution?

Please answer both questions. One millimole of Ni(NO3)2 dissolves in 270.0 mL of a solution that...

Please answer both questions. One millimole of Ni(NO3)2 dissolves in 270.0 mL of a solution that is 0.400 M in ammonia. The formation constant of Ni(NH3)62+ is 5.5×108. 1. What is the initial concentration of Ni(NO3)2 in the solution? 2. What is the equilibrium concentration of Ni2+(aq ) in the solution?

Using (Kf=1.2×109) calculate the concentration of Ni2+(aq), assuming that it is present as Ni(NH3)2+6, at equilibrium...

Using (Kf=1.2×109) calculate the concentration of Ni2+(aq), assuming that it is present as Ni(NH3)2+6, at equilibrium after dissolving 1.28 gNiCl2 in 100.0 mL of 0.20 MNH3(aq).

Using the appropriate Ksp values, find the concentration of NO3− ions in the solution at equilibrium...

Using the appropriate Ksp values, find the concentration of NO3− ions in the solution at equilibrium after 700 mL of 0.35 M aqueous Cu(NO3)2 solution has been mixed with 350 mL of 0.40 M aqueous KOH solution. (Enter in M.) (Ksp for Cu(OH)2 is 2.6x10-19). Now find the concentration of OH− ions in this solution at equilibrium. (Enter in M.)

Calculate the equilibrium concentration of Ag+(aq ) in a solution that is initially 0.170 M AgNO3...

Calculate the equilibrium concentration of Ag+(aq ) in a solution that is initially 0.170 M AgNO3 and 0.990 M NH3, and in which the following reaction takes place: Ag+(aq)+2NH3(aq)=Ag(NH3)2+(aq) (Kf = 1.70x107)

4. Calculate the equilibrium concentration of Ag+ (aq) in a solution that is initially 0.150 M...

4. Calculate the equilibrium concentration of Ag+ (aq) in a solution that is initially 0.150 M AgNO3 and 0.500 M KCN. The formation constant for [Ag(CN)2]- (aq) is Kf= 1.0 x 1021 a. 8.9 x 10-21 M b. 2.3 x 10 -21 M c. 4.3 x 10 -22 M d. 7.5 x 10 -22 M e. 3.8 x 10 -21 M 5. If a solution of Pb(NO3)2 (aq) is mixed with a solution of NaBr(aq), what condition would cause precipitation...

Calculate the equilibrium concentration of Ag^+(aq ) in a solution that is initially 0.140 M AgNO3...

Calculate the equilibrium concentration of Ag^+(aq ) in a solution that is initially 0.140 M AgNO3 and 0.850 M NH3, and in which the following reaction takes place: Ag^+(aq)+2NH3(aq)<---->Ag(NH3)2^+(aq) (Kf = 1.70x10^7)

Calculate the equilibrium concentration of Ag+ (aq) in a solution that is initially 0.130 M AgNO3...

Calculate the equilibrium concentration of Ag+ (aq) in a solution that is initially 0.130 M AgNO3 and 0.610 M NH3 and in which the following reaction takes place: Ag+ (aq) + 2NH3(aq) <--> Ag(NH3)2+ (aq) Kf = 1.7 x 107

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