A solution is prepared in which 0.00100 mol of Ni(NO3)2 and 0.500 mole of NH3 are...

A solution is prepared in which 0.00100 mol of Ni(NO3)2 and 0.500 mole of NH3 are dissolved in a total volume of 1.00 L. What is the concentration of Ni(H2O)62+ ions in the solution at equilibrium?

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

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?

The complex ion Cu(NH3)42 is formed in a solution made of 0.0400 M Cu(NO3)2 and 0.500...

The complex ion Cu(NH3)42 is formed in a solution made of 0.0400 M Cu(NO3)2 and 0.500 M NH3. What are the concentrations of Cu2 , NH3, and Cu(NH3)42 at equilibrium? The formation constant*, Kf, of Cu(NH3)42 is 1.70 × 1013.

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?

100.0 mL of 0.500 M lead(II) nitrate (Pb(NO3)2, 331 g/mol) and 100.0 mL of 0.500 M...

100.0 mL of 0.500 M lead(II) nitrate (Pb(NO3)2, 331 g/mol) and 100.0 mL of 0.500 M sodium sulfate (Na2SO4, 142 g/mol) are mixed together. (I) Write the overall balanced equation. Include the states of each species. (II) Write the overall (or total) ionic equation for the reaction. Identify any spectator ions. Include states of each species. (III) Write the net ionic equation. Include states of each species. (IV) Determine the limiting reactant and the theoretical yield of the non-aqueous product....

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?

(A) A current of 4.62 A is passed through a Ni(NO3)2 solution for 1.70 hours. How...

(A) A current of 4.62 A is passed through a Ni(NO3)2 solution for 1.70 hours. How much nickel is plated out of the solution? (B) A current of 4.09 A is passed through a Cr(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 7.70 g of chromium?

A. Calculate the concentrations of K1 and NO3 2 in an aqueous solution prepared by dissolving...

A. Calculate the concentrations of K1 and NO3 2 in an aqueous solution prepared by dissolving 30.3 g KNO3 in enough water to make 300. mL of solution. B. Calculate the concentrations of Al13 and SO4 22 in an aqueous solution prepared by dissolving 17.1 g Al2 (SO4 ) 3 in enough water to make 400. mL of solution. C. Calculate the concentrations of Na1 and SO4 22 in an aqueous solution prepared by dissolving 852 g Na2 SO4 in...

a buffer solution is prepared by mixing 100cm3 aqueous NH3 0.1mol dm-3 with 100cm3 NH4Cl mol...

a buffer solution is prepared by mixing 100cm3 aqueous NH3 0.1mol dm-3 with 100cm3 NH4Cl mol dm-3 . Given that KB for NH3 =1.74x10^-5 ... 1) calculate pH of the buffer solution. ... 2)calculate the solution after addition 50cm3 HCl of 0.1 mol dm-3.

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?

A solution was prepared by dissolving 0.0170 mole of propionic acid and 0.0179 mole of sodium...

A solution was prepared by dissolving 0.0170 mole of propionic acid and 0.0179 mole of sodium propionate in 1.00 L? What would be the pH of the solution in beaker after 2.00 mL of 0.0154 M HCl were added to 10.0 mL of the prepared solution?

Subjects