Question

The hydride ion, $H^-$, is a stronger base than the hydroxide ion, $OH^-$. Which one of the following reactions will occur if sodium hydride (NaH) is dissolved in water?

• A. $\ce{H^{-} (aq) + H_2O(l) -> H_3O^{-} (aq)}$
• B. $\ce{H^{-} (aq) + H_2O(l) -> OH^{-} (aq) + H_2 (g)}$
• C. $\ce{H^{- } (aq) + H_2O(l) -> OH^{-} (aq) + 2H^{+} (aq) + 2e}$
• D. $\ce{H^{-} (aq) + H2O(l) ->}$ No reaction

Answer 1

Answer: (B)

$\ce{H^{-} (aq) + H_2O(l) -> OH^{-} (aq) + H_2 (g)}$

Answer 2

In this reaction $H^-$ acts as bronsted base as it accepts one proton $(H^+)$ from $H_2O$ and for $H_2$.