Which of the following is not correct for `D_(2)O`

Options

A. Boiling point is higher than `H_(2)O`
B. `D_(2)O` reacts slowly than `H_(2)O`
C. Viscosity is higher than `H_(2)O` at `25^(@)`
D. Solubility of NaCl in it is more than `H_(2)O`

Answer

D

Explanation

When NaCl is dissolved in water, Na ion attracted towards the negative part of water (i.e. O atom) and `Cl^(-)` ion attracted towards the positive part of water (H atom) . This causes the sodium chloride to split in water and the NaCl dissolves into separate `Na^(+)` and `Cl^(-)` ions. A hydration shell is formed around them which prevents `Na^(+)` and `Cl^(-)` to form ionic bonds.
In case of `D_(2)O`, due to lower electronegativity of D, O atom has more negative charge so D - O bond is stronger than H - O bond. Moreover due to stronger hydrogen bond in `D_(2)O`, the rearrangement of `D_(2)O` molecules around `Na^(+)` and `Cl^(-)` ions is tougher than in `H_(2)O`. So solubility of NaCl will be less in `D_(2)O` compare to that in `H_(2)O`.