Write balanced equations for the formation of K4[Ni(NCS)6] starting from an anhydrous sample of nickel(II) nitrate. (3 equations necessary)
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Please post what you think.
I think that nickel(II) nitrate has the formula Ni(NO3)2. As we are starting from anhyrdrous nickel nitrate I thought the first step might be to hydrate it
Ni(NO3)2 + 6H2O --> [Ni(H2O)6](NO3)2
and then I thought a reaction with potassium thiocyanate KSCN but I am not sure how to get 3 equations overall.
See my response to your later question. I think you may be on the right track.
To write balanced equations for the formation of K4[Ni(NCS)6] starting from an anhydrous sample of nickel(II) nitrate, we need to follow the steps involved in the formation.
1. The first step is the reaction between nickel(II) nitrate and potassium thiocyanate to form nickel(II) thiocyanate:
Ni(NO3)2 + 2KSCN → Ni(SCN)2 + 2KNO3
In this reaction, two moles of potassium thiocyanate react with one mole of nickel(II) nitrate to produce one mole of nickel(II) thiocyanate and two moles of potassium nitrate.
2. The second step involves the reaction between nickel(II) thiocyanate and potassium nitrate to form potassium nickel(II) thiocyanate:
Ni(SCN)2 + 2KNO3 → K2[Ni(SCN)4] + 2NO2 + O2
In this step, one mole of nickel(II) thiocyanate reacts with two moles of potassium nitrate to form one mole of potassium nickel(II) thiocyanate, two moles of nitrogen dioxide gas, and one mole of oxygen gas.
3. Finally, the product from the previous step, potassium nickel(II) thiocyanate, can react with potassium thiocyanate to form the desired compound, K4[Ni(NCS)6]:
K2[Ni(SCN)4] + 2KSCN → K4[Ni(NCS)6]
Here, one mole of potassium nickel(II) thiocyanate reacts with two moles of potassium thiocyanate to produce four moles of the target compound, K4[Ni(NCS)6].
These three equations summarize the formation of K4[Ni(NCS)6] from an anhydrous sample of nickel(II) nitrate.