1. Calculate the [H3O+] of a 1.93 M HBrO solution at 25 ºC.
please show work.
To do this, you need to show the reaction involved of the hydrolisis of this compound, and you should take account of the Ka of this acid, because HBrO is a medium strong acid, but it does not dissociate completely in solution. The Ka reported is 2x10-9. Now the reaction, along with the ICE chart to calculate the H3O+ is:
r: HBrO + H2O <-------->
H3O+ + BrO- Ka =
i: 1.93 0 0
e: 1.93-x x x
Writting the expression for the equilibrium constant:
2x10-9 = x2 / 1.93-x
Ka is a very small value, so we can assume that x would be very small too, and we can neglect the substract of 1.93-x to 1.93 only. Solving for x:
2x10-9 * 1,93 = x2
x = 6.21x10-5 M = [H3O+]
Hope this helps
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