# For the aqueous [Cu(NH3)4]^2+ complex =Kf=5.6x10^11 at 25°C.Suppose equal volumes of 0.0058M Cu(NO3)2 solution and 0.66M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Cu^2+ ion.Round your answer to 2 significant digits.

Question
27 views

For the aqueous [Cu(NH3)4]^2+ complex =Kf=5.6x10^11 at 25°C.

Suppose equal volumes of 0.0058M Cu(NO3)2 solution and 0.66M

NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Cu^2+ ion.

check_circle

Step 1

The overall formation constant for the reaction is shown in equation  (1) in which Kf is the overall formation constant, HA is the reactant and  and  are the products

Step 2

The equal volumes of copper nitrate and ammonia makes the molarity half. Thus, the molarity of Cu(NO3)2 is shown in equation (2).

The molarity of ...

### Want to see the full answer?

See Solution

#### Want to see this answer and more?

Solutions are written by subject experts who are available 24/7. Questions are typically answered within 1 hour.*

See Solution
*Response times may vary by subject and question.
Tagged in