# Of these, what is the order from highest pH to lowest pH? LiOH(aq), HBrO(aq), Sr(OH)_2(aq), NH_3(aq), and HI(aq)

Jun 1, 2017

The bases gives rise to more alkaline solution, and thus higher $p H$

#### Explanation:

And so from highest $p H$ to lowest.........I propose...........

$S r {\left(O H\right)}_{2} \left(a q\right) , L i O H \left(a q\right) , N {H}_{3} \left(a q\right) , H B r O \left(a q\right) , H I \left(a q\right)$.

The right hand side includes the strong acid $H I$. $H B r O$ is a weak acid; ammonia, $N {H}_{3}$, behaves as a bas in aqueous solution.

Why will $S r {\left(O H\right)}_{2}$ gives a higher $p H$ than $L i O H$ given equal concentration?