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?

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) H-(aq) + H2O (l)arrow OH-(aq) + 2H2(g) (B) H-(aq) + H2O(l) arrow H3O-(aq) (C) H-(aq) + H2O (l)arrow OH-(aq) + 2H+(aq) + 2e (D) H-(aq) + H2O (l) arrow No reaction

Tardigrade Admin · Accepted Answer

undersetbase 1H-(aq) + undersetacid 1 H2O(l) arrow undersetbase 2 OH-(aq) + undersetacid 2H2(g) In this reaction H- acts as Bronsted base as it accepts one proton (H+) from H2O and for H2.

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

$H_{(a q)}^{-} + H_{2} O (l) \to O H^{-} (a q) + 2 H_{2} (g)$

$H^{-} (a q) + H_{2} O (l) \to H_{3} O^{-} (a q)$

$H^{-} (a q) + H_{2} O (l) \to O H^{-} (a q) + 2 H^{+} (a q) + 2 e$

$H^{-} (a q) + H_{2} O (l) \to$ No reaction

$ba se 1 H^{-} (a q) + a c i d 1 H_{2} O (l) \to ba se 2 O H^{-} (a q) + a c i d 2 H_{2} (g)$
In this reaction $H^{-}$ acts as Bronsted base as it accepts one proton $(H^{+})$ from $H_{2} O$ and for $H_{2}$ .

Q. 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?

H(aq)−​+H2​O(l)→OH−(aq)+2H2​(g)

H−(aq)+H2​O(l)→H3​O−(aq)

H−(aq)+H2​O(l)→OH−(aq)+2H+(aq)+2e

H−(aq)+H2​O(l)→ No reaction