+ For the aqueous [Ni(NH3)6] complex K, = 5.50 × 108 at 25 °C. Suppose equal volumes of 0.0062M Ni (NO3), solution and 0.78M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Round your answer to 2 significant digits. 2 Ni 2+ Ом x10 ☑ ك ion.
+ For the aqueous [Ni(NH3)6] complex K, = 5.50 × 108 at 25 °C. Suppose equal volumes of 0.0062M Ni (NO3), solution and 0.78M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Round your answer to 2 significant digits. 2 Ni 2+ Ом x10 ☑ ك ion.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section12.3: Determining Equilibrium Constants
Problem 12.3PSP
Related questions
Question
![+
For the aqueous
[Ni(NH3)6] complex K, = 5.50 × 108 at 25 °C.
Suppose equal volumes of 0.0062M Ni (NO3), solution and 0.78M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous
Round your answer to 2 significant digits.
2
Ni 2+
Ом
x10
☑
ك
ion.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7bc30bfd-54a4-45be-8be6-a7bac17a47af%2F9f5fb726-e0e5-4175-b77a-7977ec97ddf2%2Fxqe56he_processed.png&w=3840&q=75)
Transcribed Image Text:+
For the aqueous
[Ni(NH3)6] complex K, = 5.50 × 108 at 25 °C.
Suppose equal volumes of 0.0062M Ni (NO3), solution and 0.78M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous
Round your answer to 2 significant digits.
2
Ni 2+
Ом
x10
☑
ك
ion.
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