M
MathGurl
Guest
Sodium hydride, NaH(s), reacts with liquid water to form NaOH(aq) and H2 gas.
(a) Write the equation of the reaction and explain it from the veiwpoint of the Bronsted-Lowry acid-base theory.
(b) Calculate pOH and pH for the solution formed from dissolving 10.0 g NaH(s) in enough water to make 1.00 L of a solution.
(c) How many grams of N2O5 would be required to neutralize this solution?
Any help would be much appreciated!!
I'm only completely sure of the equation:
NaH (s) + H2O (l) -> NaOH (aq) + H2 (g)
I think i have the first two parts:
I got a pH of 0.38 and a pOH of 13.62.
I'm confused about the third part. Where does the N2O5 come in? Do we assume a 1:1 mole ration between N2O5 and NaH?
(a) Write the equation of the reaction and explain it from the veiwpoint of the Bronsted-Lowry acid-base theory.
(b) Calculate pOH and pH for the solution formed from dissolving 10.0 g NaH(s) in enough water to make 1.00 L of a solution.
(c) How many grams of N2O5 would be required to neutralize this solution?
Any help would be much appreciated!!
I'm only completely sure of the equation:
NaH (s) + H2O (l) -> NaOH (aq) + H2 (g)
I think i have the first two parts:
I got a pH of 0.38 and a pOH of 13.62.
I'm confused about the third part. Where does the N2O5 come in? Do we assume a 1:1 mole ration between N2O5 and NaH?