From the value kf=1.2×109 for ni(nh3)62+, calculate the concentration of nh3 required to just dissolve 0.011 mol of nic2o4 (ksp = 4×10−10) in 1.00 l of solution. (hint: you can neglect the hydrolysis of c2o42− because the solution will be quite basic.)

The molar concentration of NH₃ required is 0,54M

Explanation:

In this problem you need to sum the two reactions, thus:

NiC₂O₄(s) ⇄ Ni²⁺ + C₂O₄²⁻ ksp: 4x10⁻¹⁰

Ni²⁺ + 6NH₃ ⇄ Ni(NH₃)₆²⁺ kf: 1,2x10⁹

The sum of the reactions is:

NiC₂O₄(s) + 6NH₃ ⇄ Ni(NH₃)₆²⁺ + C₂O₄²⁻ k' = kf×ksp = 0,48

The equation for this equilibrium is:

If we are lloking for the complete dissolution of 0,11mol/L of NiC₂O₄(s), the molar concentrations of Ni(NH₃)₆²⁺ and C₂O₄²⁻ are 0,11M, replacing:

The molar concentration of NH₃ required is:

[NH₃]⁶ = 0,0252

[NH₃] = ⁶√0,0252

[NH₃] = 0,54M

I hope it helps!

most likely he is cheating on you

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prevailing winds carry air toward the mountain range. as the air rises up over a mountain range, the air cools, water vapor condenses, and clouds form. on this side of the mountains, called the windward side, precipitation falls in the form of  rain  or snow. this dry air produces a  rain shadow.