The hydride ion H^{-} is a stronger base than | vedclass

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(B) Since $H^{-}$ is a stronger base than $OH^{-}$,it will readily accept a proton from water.$H^{-}$ acts as a Bronsted-Lowry base and $H_2O$ acts as

Vedclass · Accepted Answer

$H^{-}_{(aq)} + H_2O_{(l)} 	o OH^{-}_{(aq)} + H_{2(g)}$

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(B) Since $H^{-}$ is a stronger base than $OH^{-}$,it will readily accept a proton from water.$H^{-}$ acts as a Bronsted-Lowry base and $H_2O$ acts as a Bronsted-Lowry acid.The reaction is: $H^{-}_{(aq)} + H_2O_{(l)} 	o OH^{-}_{(aq)} + H_{2(g)}$This is an acid-base reaction where the stronger base $(H^{-})$ reacts with the acid $(H_2O)$ to form a weaker base $(OH^{-})$ and a weaker acid $(H_2)$.

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

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