A solution is made that is 1.2×10−3 M in Zn(NO3)2 and 0.130 M in NH3. After the solution reaches equilibrium, what concentration of Zn2+(aq) remains?

Explanation:

Equation for the reaction can be expressed as:

    ⇄    

From the equation above; we use the ICE table to determine how much complex ion forms  in order to be able to calculate  the at equilibrium.

So;

                                     ⇄    

Initial                                                    

Change                          

Equilibrium                                                    

  ⇒  

=  

=  

=

Therefore, the concentration of Zn2+(aq) after the solution reaches equilibrium =

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%

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