When NiCl2.6H2O dissolves in water, what does it form (i.e. balanced equation)?
Ni forms ions, Cl forms ions.
NiCl2.6H2O ==> Ni(H2O)4^+2 + 2Cl^- + 2H2O
http://en.wikipedia.org/wiki/Nickel%28II%29_chloride
When NiCl2.6H2O dissolves in water, it forms hydrated nickel(II) chloride. The balanced equation for this dissolution can be represented as:
NiCl2.6H2O(s) + H2O(l) → NiCl2(aq) + 6H2O(l)
To determine the balanced equation for the dissolution of NiCl2.6H2O in water, we first need to understand the components involved.
NiCl2.6H2O is a hydrated nickel chloride compound, specifically nickel(II) chloride hexahydrate. When it dissolves in water, it dissociates into its constituent ions. The formula for the hydrated nickel chloride is NiCl2.6H2O, indicating that there are six water molecules associated with each nickel chloride molecule.
The balanced equation for the dissolution of NiCl2.6H2O can be written as follows:
NiCl2.6H2O(s) → Ni2+(aq) + 2Cl-(aq) + 6H2O(l)
In this equation, (s) represents the solid state for NiCl2.6H2O, (aq) represents the aqueous (dissolved) state for the ions, and (l) represents the liquid state for water.
Once dissolved, the hydrated nickel chloride dissociates into nickel(II) ions (Ni2+) and chloride ions (Cl-), along with six water molecules (H2O).