You mix a 120.0 −mL − m L sample of a solution that is 0.0123 M...
You mix a 120.0 −mL − m L sample of a solution that is 0.0123 M M in NiCl2 N i C l 2 with a 185.0 −mL − m L sample of a solution that is 0.300 M M in NH3 N H 3 .
After the solution reaches equilibrium, what concentration of Ni2+(aq)Ni2+(aq) remains? The value of KfKf for Ni(NH3)62+Ni(NH3)62+ is 2.0×1082.0×108.
Homework Answers
You mix a 105.0 −mL sample of a solution that is 0.0130 M in NiCl2 with...
You mix a 105.0 −mL sample of a solution that is 0.0130 M in NiCl2 with a 185.0 −mL sample of a solution that is 0.300 M in NH3. After the solution reaches equilibrium, what concentration of Ni2+(aq) remains? The value of Kf for Ni(NH3)62+ is 2.0×108.
You mix a 140.0 −mL sample of a solution that is 0.0146 M in NiCl2 with...
You mix a 140.0 −mL sample of a solution that is 0.0146 M in NiCl2 with a 175.0 −mL sample of a solution that is 0.250 M in NH3. Part A After the solution reaches equilibrium, what concentration of Ni2+(aq) remains? The value of Kf for Ni(NH3)62+ is 2.0×10^8 Express the concentration to two significant figures and include the appropriate units.
Review Constants Periodic Table You mix a 120.0-ml sample of a solution that is 0.0134 M...
Review Constants Periodic Table You mix a 120.0-ml sample of a solution that is 0.0134 M in NiCl, with a 195.0-ml sample of a solution that is 0.500 Min NH You may want to reference Pages 778 - 783) Section 17.7 while completing this problem Part A After the solution reaches equilibrium, what concentration of Ni2+ (aq) remains? The value of K for Ni(NH4)2 | 2.0 x 10*. Express the concentration to two significant figures and include the appropriate units....
2. You mix a 105.0 mL sample of a solution that is 0.0114 M in Ni(NO3)2...
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.
you mix a 200.0 ml sample of a solution that is 1.5x10^-3 M in Cu(NO3)2 with...
you mix a 200.0 ml sample of a solution that is 1.5x10^-3 M in Cu(NO3)2 with a 250.0 ml sample of a solution that is .20 M in NH3. After the solution reaches equilibrium, what concentration of cu2+ remains?
One millimole of Ni(NO3)2 dissolves in 230.0 mL of a solution that is 0.300 M in...
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
2. Consider a 100.0 mL sample of 0.0200 M Ni(NO3)2. Then 10.0 mL of 0.300 M...
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) Krfor [Ni(NH3).]?* = 2.0 x 108
2. Consider a 100.0 mL sample of 0.0200 M NI(NO3)2. Then 10.0 mL of 0.300 M...
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
Consider a 100.0 mL sample of 0.0200 M Ni(NO3)2.. Then 10.0 mL of 0.300 M NH3...
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)6]2+ at equilibrium? Kf for [Ni(NH3)6]2+ = 2.0 x 108
One millimole of Ni(NO3)2 dissolves in 240.0 mL of a solution that is 0.500 M in...
One millimole of Ni(NO3)2 dissolves in 240.0 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?
Review Constants Periodic Table You mix a 120.0-ml sample of a solution that is 0.0134 M in NiCl, with a 195.0-ml sample of a solution that is 0.500 Min NH You may want to reference Pages 778 - 783) Section 17.7 while completing this problem Part A After the solution reaches equilibrium, what concentration of Ni2+ (aq) remains? The value of K for Ni(NH4)2 | 2.0 x 10*. Express the concentration to two significant figures and include the appropriate units....
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.
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) Krfor [Ni(NH3).]?* = 2.0 x 108
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
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