In a 1.0 x 10-6 M solution of Ba(OH), (aq) at 25 °C, arrange the species...

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In a 1.0 x 10-6 M solution of Ba(OH), (aq) at 25 °C, arrange the species by their relative molar amounts in solution. Greates

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Answer 1

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Answer #1

H2O is solvent and hence it will be present in greatest amount
Ba(OH)2 will dissolve completely.
So, Ba(OH)2 will be in least amount.

Since we are adding base,
[OH-] > [H3O+]

Ba(OH)2 -> Ba2+ + 2OH-
So, [OH-] > [Ba2+]

Infact:
[Ba2+] = 1.0*10^-6 M
[OH-] = 2.0*10^-6 M

use:
[H3O+] = Kw/[OH-]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[H3O+] = (1.0*10^-14)/[OH-]
[H3O+] = (1.0*10^-14)/2*10^-6
[H3O+] = 5.0*10^-9 M

Answer:
H2O
OH-
Ba2+
H2O+
Ba(OH)2

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Answer 2

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