You mix a 133.0 mL sample of a solution that is 0.0100 M in NiCl2 with...

You mix a 133.0 mL sample of a solution that is 0.0100 M in NiCl2 with a 183.5 mL sample of a solution that is 0.220 M in NH3. After the solution reaches equilibrium, what concentration of Ni2+(aq) remains? (Formation constant is Kf=2.0×108.)

Expert Solution

queen_honey_blossom answered 2 years ago

You mix a 124.0 mL sample of a solution that is 0.0121 M in NiCl2 with...

You mix a 124.0 mL sample of a solution that is 0.0121 M in NiCl2 with a 183.5 mL sample of a solution that is 0.254 M in NH3. Part A After the solution reaches equilibrium, what concentration of Ni2+(aq) remains? (Formation constant is Kf=2.0×108.) Express your answer with the appropriate units.

You mix a 131.0 mL sample of a solution that is 0.0115 M in NiCl2 with...

You mix a 131.0 mL sample of a solution that is 0.0115 M in NiCl2 with a 173.5 mL sample of a solution that is 0.256 M in NH3. After the solution reaches equilibrium, what concentration of Ni2+(aq) remains? (Formation constant is Kf=2.0×108.)

You mix a 116.0 mL sample of a solution that is 0.0102 M in NiCl2 with...

You mix a 116.0 mL sample of a solution that is 0.0102 M in NiCl2 with a 165.0 mL sample of a solution that is 0.232 M in NH3. After the solution reaches equilibrium, what concentration of Ni2+(aq) remains? (Formation constant is Kf=2.0×108.)

You mix a 150.0 −mL sample of a solution that is 0.0140 M in NiCl2 with...

You mix a 150.0 −mL sample of a solution that is 0.0140 M in NiCl2 with a 175.0 −mL sample of a solution that is 0.500 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 120.5 mL sample of a solution that is 0.0123 M in NiCl2 with...

You mix a 120.5 mL sample of a solution that is 0.0123 M in NiCl2 with a 183.0 mL sample of a solution that is 0.270 M in NH3. After the solution reaches equilibrium, what concentration of Ni2+(aq) remains? (Formation constant is Kf=2.0×108.)

A. You mix a 125.5 mL sample of a solution that is 0.0111 M in NiCl2...

A. You mix a 125.5 mL sample of a solution that is 0.0111 M in NiCl2 with a 183.0 mL sample of a solution that is 0.225 M in NH3 After the solution reaches equilibrium, what concentration of Ni2+(aq) remains? (Formation constant is Kf=2.0×108.)Express your answer with the appropriate units. B. A 120.0 −mL sample of a solution that is 2.7×10−3 M in AgNO3 is mixed with a 230.0 −mL sample of a solution that is 0.10 M in NaCN....

A 130.0 mL sample of a solution that is 0.0126 M in NiCl2 is mixed with...

A 130.0 mL sample of a solution that is 0.0126 M in NiCl2 is mixed with a 190.0 mL sample of a solution that is 0.400 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.

11 mL of 0.0100 M HCl are added to 25.0 mL of a buffer solution that...

11 mL of 0.0100 M HCl are added to 25.0 mL of a buffer solution that is 0.010 M HC2H3O2 and 0.08 M C2H3O2-. What is the pH of the resulting solution?

You mix a 140.0 −mL−mL sample of a solution that is 0.0124 MM in NiCl2NiCl2 with...

You mix a 140.0 −mL−mL sample of a solution that is 0.0124 MM in NiCl2NiCl2 with a 200.0 −mL−mL sample of a solution that is 0.350 MM in NH3NH3. 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. Express the concentration to two significant figures and include the appropriate units.

A 35 mL sample of water is triated with 0.0100 M EDTA. Exactly 9.70 mL of...

A 35 mL sample of water is triated with 0.0100 M EDTA. Exactly 9.70 mL of EDTA are required to reach the EBT endpoint. Calculate the total hardness in ppm CaCO3.

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