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Verified Answer :

Willchemistry

\([ H_3O^+] = 10 ^{-pH}\)

\([H_3O^+] = 10 ^{-8.7}\)

\([H_3O^+] = 1.995*10 ^{-9} M\)

hope this helps!

The h3o+ of a solution with pH = 8.7 is 1.995×10∧-9

Relation between pH and concentration of H+

The pH is equal to logarithm of reciprocal of concentration of H+.

pH = ㏒1/[H+]

pH = - ㏒[H+]

- pH = ㏒[H+]

[H+] = 10∧-pH

If pH =  8.7 of h3o+

Then, h3o+ dissociates as.

H3O+ ⇄ H+ + H2O

Then,

[H+] = 10∧-pH

[H+] = 10∧-8.7

[H+] = 1.995×10∧-9

To learn more about pH here.

https://brainly.com/question/15289741

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