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

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Answer 1 · 2017-06-01T05:20:47

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

And so from highest $pH$ to lowest.........I propose...........

$Sr(OH)_2(aq), LiOH(aq), NH_3(aq), HBrO(aq), HI(aq)$ .

The right hand side includes the strong acid $HI$ . $HBrO$ is a weak acid; ammonia, $NH_3$ , behaves as a bas in aqueous solution.

Why will $Sr(OH)_2$ gives a higher $pH$ than $LiOH$ given equal concentration?

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