# Question ad049

Dec 28, 2016

Ammonia gas behaves as an alkali in water........................

#### Explanation:

Ammonia gas is exceptionally soluble in water, and an experiment called the $\text{ammonia fountain}$ (which you'll have to seek out on the interwebz) spectacularly demonstrates this. In aqueous solution, ammonia behaves as a weak base, and the given equilibrium lies somewhat to the right:

$N {H}_{3} \left(a q\right) + {H}_{2} O \left(a q\right) r i g h t \le f t h a r p \infty n s N {H}_{4}^{+} + H {O}^{-}$ ;K_"eq"=10^(-4.75)#

If you are in first year university, can you tell me the $p H$ of a $1 \cdot m o l \cdot {L}^{-} 1$ solution of $N {H}_{3} \left(a q\right)$?

${K}_{\text{eq}} = {10}^{- 4.75} = \frac{\left[N {H}_{4}^{+}\right] \left[H {O}^{-}\right]}{\left[N {H}_{3} \left(a q\right)\right]}$