Question

Calculate the value of [H3O+] from the given [−OH] in each solution and label the solution...

Calculate the value of

[H3O+] from the given [−OH] in each solution and label the solution as acidic or basic:

(a) [−OH] = 6.8 × 10−9M;

(b) [−OH] = 2.8 × 10−2M.

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Homework Answers

Answer #1

use the formula

ionic product of water

[H3O+][HO-] = 1.0 x 10^-14

and pH = -log[H3O+]

pOH = -log[HO-]

a.

given concentration is [HO-] = 1.0 x 10^-14

[H3O+] [ 6.8 × 10−9M] = 1.0 x 10^-14

[H3O+] = 1.0 x 10^-14 / 6.8 × 10−9M   = 1.47 x 10^-6 M

pH = -log[H3O+] = -log[1.47 x 10^-6 M]   = 5.83 M

pH is less than 7 so acidic

b.

given concentration is [HO-] =2.8 × 10−2M

[H3O+] [ 2.8 × 10−2M = 1.0 x 10^-14

[H3O+] = 1.0 x 10^-14 / 2.8 × 10−2M   = 3.57 x 10^-13 M

pH = -log[H3O+] = -log[3.57 x 10^-13 M]   = 12.44 M

pH is more than basic

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