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Get Full Access to Introductory Chemistry - 5 Edition - Chapter 14 - Problem 69p
Get Full Access to Introductory Chemistry - 5 Edition - Chapter 14 - Problem 69p

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# Calculate the pH of each solution.(a) [H3O+] = 1.7 × 10?8 M(b) [H3O+] = 1.0 × 10?7 M(c)

ISBN: 9780321910295 34

## Solution for problem 69P Chapter 14

Introductory Chemistry | 5th Edition

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Problem 69P

Calculate the pH of each solution.

(a) $$\mathrm{[H_3O^+]=1.7 \times 10^{-8} ~M}$$

(b) $$\mathrm{[H_3O^+]=1.0 \times 10^{-7} ~M}$$

(c) $$\mathrm{[H_3O^+]=2.2 \times 10^{-6} ~M}$$

(d) $$\mathrm{[H_3O^+]=7.4 \times 10^{-4} ~M}$$

Equation Transcription:

Text Transcription:

[H_3O^+]=1.7 x 10^{-8} M

[H_3O^+]=1.0 x 10^{-7} M

[H_3O^+]=2.2 x 10^{-6} M

[H_3O^+]=7.4 x 10^{-4} M

Step-by-Step Solution:
Step 1 of 3

To calculate the pH of an aqueous solution you need to know the concentration of the hydronium ion in moles per liter (molarity). The pH is then calculated using the expression:

pH = - log [H3O+].

(a) [H3O+] = 1.7 × 10−8 M

Solution :

pH = - log  [ 1.7 × 10−8 M]

Step 2 of 3

Step 3 of 3

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