Which has the higher [H+], 0.40 M RbOH or 0.20 M Ca(OH)2?

Won't the H^+ be the same?

OH for 0.40 M RbOH is 0.4M
OH for 0.20 M Ca(OH)2 is 0.4 M.

To determine which solution has the higher concentration of [H+], we need to consider the concept of acidity and the dissociation of hydroxide ions (OH-) in both RbOH and Ca(OH)2.

RbOH and Ca(OH)2 are both strong bases that dissociate completely in water. The dissociation reactions are as follows:

RbOH -> Rb+ + OH-
Ca(OH)2 -> Ca2+ + 2OH-

The concentration of hydroxide ions (OH-) in each solution is the same as the concentration of the respective base Ions. Therefore:

For RbOH:
[OH-] = 0.40 M

For Ca(OH)2:
[OH-] = 2 x 0.20 M = 0.40 M

As we can see, both solutions have the same concentration of hydroxide ions. However, the concentration of hydrogen ions ([H+]) is related to the concentration of hydroxide ions through the autoionization of water:

2H2O -> H3O+ + OH-

In neutral water, the concentrations of [H3O+] and [OH-] are equal at 1 x 10^-7 M. However, in basic solutions, the concentration of [OH-] is higher than [H3O+], which means that the concentration of [H+] is lower.

Since both RbOH and Ca(OH)2 produce the same concentration of [OH-], they will also have the same concentration of [H+]. Therefore, both solutions have the same higher [H+] concentration.

In conclusion, both 0.40 M RbOH and 0.20 M Ca(OH)2 have the same higher concentration of [H+].