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# Calculate [H3O+] given [OH ] in each aqueous solution and ISBN: 9780321910295 34

## Solution for problem 65P Chapter 14

Introductory Chemistry | 5th Edition

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Problem 65P

Calculate [H3O+] given [OH ] in each aqueous solution and classify each solution as acidic or basic.

(a) [OH−] = 2.7 × 10−12M

(b) [OH−] = 2.5 × 10−2 M

(c) [OH−] = 1.1 × 10−10 M

(d) [OH−] = 3.3 × 10−4 M

Step-by-Step Solution:
Step 1 of 3

Solution: Here, we are going to calculate hydronium ion concentration in each of the solution.

Step1:

In pure water, one H2O molecule donates proton and acts as an acid and another water molecule accepts a proton and acts as a base at the same time. The following equilibrium exists:

H2O(l) + H2O(l) ------> H3O+(aq) + OH-(aq)

The equilibrium constant for the reaction is given by:

Kw= [H3O+][OH−]        -----(1)

Where, Kw is called the ionic product of water and its value is 1 x 10-14 M2.

We can distinguish acidic, neutral and basic aqueous solutions by the relative values of the H3O+ and OH− concentrations:

Acidic: [H3O+] > [OH−]

Neutral: [H3O+] = [OH−]

Basic: [H3O+] < [OH−]

Step2:

Given, [OH-] = 2.7 x 10-12 M

From equation (1), [H3O+] = Kw / [OH-]

[H3O+] = (1 x 10-14 M2) / (2.7 x 10-12 M)

...

Step 2 of 3

Step 3 of 3

##### ISBN: 9780321910295

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