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Calculate [H3O+] for each solution.(a) pH = 8.55(b) pH = Problem 71P Chapter 14

Introductory Chemistry | 5th Edition

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Problem 71P

Calculate [H3O+] for each solution.

(a) pH = 8.55

(b) pH = 11.23

(c) pH = 2.87

(d) pH = 1.22

Step-by-Step Solution:
Step 1 of 3

The concentration of [OH-] ion and [H3O+]  can be determined as follows   ,

It is known that pH = -log [H3O+]

-pH = log [H3O+]

10 -pH  = 10log [H3O+]   or

[H3O+] = 10-pH

1.0 10-14

And   [OH-  ]  =  --------------

[H3O+]

Step-1

(a) pH = 8.25

pH = 8.25

The  [H3O+]  from pH =  8.25 can be calculated as follows,

[H3O+] = 10-pH  or  [H3O+] = antilog (- pH)

8.25 = - log [H3O+]

-  8.25 = log [H3O+]

[H3O+] = 10- 8.25  = 5.62 10-9 M

1.0 10-14       1.0 10-14

Thus,  [OH-]  =  -------------- =     -----------    = 1.7 10-6M

[H3O+]           5.62 10-9

(b) pH = 11.23

We can calculate [OH− ], by using the following formula.

1.0 10-14

[OH-  ]  =  --------------

[H3O+]

Now the  [H3O+]  from pH = 11.23can be calculated as follows,

[H3O+] = 10-pH  or  [H3O+] = antilog (- pH)

11.23= - log [H3O+]

- 11.23= log [H3O+]

[H3O+] = 10- 11.23 = 15.9 10-9 M

1.0 10-14       1.0 10-14

Thus,  [OH-  ]  =  -------------- =     -----------    = 1.8 *1010M

[H3O+]...

Step 2 of 3

Step 3 of 3

ISBN: 9780321910295

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