For the aqueous [Ni(NH₂)]²* complex K₁ = 5.50 × 108 at 25 °C. Suppose equal volumes of 0.0078M Ni(NO3)2 solution and 0.96M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Ni²+ ion. •2+ Round your answer to 2 significant digits. M x10

For the aqueous [Ni(NH₂)]²* complex K₁ = 5.50 × 108 at 25 °C. Suppose equal volumes of 0.0078M Ni(NO3)2 solution and 0.96M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Ni²+ ion. •2+ Round your answer to 2 significant digits. M x10

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter16: Solubility And Complex Ion Equilibria

Section: Chapter Questions

Problem 8RQ: What is a complex ion? The stepwise formation constants for the complex ion Cu(NH3)42+ are K1 1 ...

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Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

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2+
For the aqueous [Ni(NH3)
[Ni(NH3)]²+ complex K₁ = 5.50 × 108 at 25 °C.
Suppose equal volumes of 0.0078M Ni(NO3), solution and 0.96M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous
Ni²+ ion.
Round your answer to 2 significant digits.
M
0x₁
x10
X
?
Ś

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