Question
Asked Oct 30, 2019
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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.

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Expert Answer

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

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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 ...

0.0058 M
Cu(NO,)
(2)
2
=0.0029 M
0.66M
NH
...... (3)
2
= 0.33M
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0.0058 M Cu(NO,) (2) 2 =0.0029 M 0.66M NH ...... (3) 2 = 0.33M

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