Out of `Cr^(2+)` and `Cr^(3+)`, which one is stable in aqueous solution?

Explain why Cu^+ ion is not stable in aqueous solution?

Calculate the number of unpaired electrons in the following gaseous ions: Mn^(3+) , Cr^(3+) , V^(2+) and Ti^(3+) , Which one of these as the most stable in aqueous solution?

The stable +2 ions of lanthanides in aqueous solution are

How would you account for the following: i. Of the dot d^(4) species, Cr ^2+ is strongly reducing while manganese(III) is strongly oxidising. ii. Cobalt(II) is stable in aqueous solution but. in the presence of complexing reagents it is easily oxidised. ii. The d^1 configuration is very unstable in ions?

Assertion : The complex K_3 [Cr(C_2O_4)_3] when present in aqueous solution, will give test for K^(+), Cr^(3+) and oxalate ions. Reason : The complex K_3[Cr(C_2O_4)_3] will dissociate completely in solution.

If the formula mass of C r _(2) O _(7) ^( 2-) ion is M, then in the reaction Cr _(2) O _(7) ^( 2-) + 14 H ^(+) + 6 e ^(-) to 2 Cr ^(3+) + 7 H _(2) O, The equivalent mass of Cr _(2) O _(7) ^(2-) is

The standard electrode potential corresponding to the reduction Cr^(3+)+ e to Cr^(2+) is E^@=-0.407 volt. IF excess Fe(s) is added to a solution in which [Cr^(3+)]=1M , what will be [Fe^(2+)] when equilibrium is established at 25^@C [Fe (s)+2Cr^(3+) leftrightarrow Fe^(2+)+ 2Cr^(2+)]

Among the following which one of the aqueous solutions has highest boiling point?