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Determine if each solution is acidic, basic, or neutral.(a) [H3O+] = 1 × 10?5 M; [OH?] =

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 61P Chapter 14

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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Problem 61P

Determine if each solution is acidic, basic, or neutral.

(a) [H3O+] = 1 × 10−5 M; [OH−] = 1 × 10−9 M

(b) [H3O+] = 1 × 10−6 M; [OH−] = 1 × 10−8 M

(c) [H3O+] = 1 × 10−7 M; [OH−] = 1 × 10−7 M

(d) [H3O+] = 1 × 10−8 M; [OH−] = 1 × 10−6 M

Step-by-Step Solution:
Step 1 of 3

Solution 61P:

Here,  we are going find out the nature of the solution.

Water is amphoteric and it undergoes autoionization. Water behaves as an acid and a base with itself.

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

The equilibrium constant is Kw= [H3O+][OH]

Kw is known as ion product constant for water  and it is equal to  1 × 10−14  at 25oC.

Thus,

  1. A neutral solution ,  [H3O+] = [OH-] = 1 × 10−14 M at 25oC.
  2.  An acidic solution [H3O+] >  [OH-].
  3. A basic solution, [OH-] >  [H3O+].

(a) [H3O+] = 1 × 10−5 M; [OH] = 1 × 10−9 M

Here,  [H3O+] > [OH]

Therefore, the solution is acidic in nature.

(b) [H3O+] = 1 × 10−6 M; [OH] = 1 × 10−8 M

 

Here,  [H3O+] > [OH]

Therefore, the solution is acidic in nature.

(c) [H3O+] = 1 × 10−7 M; [OH] = 1 × 10−7 M

Here,   [H3O+] = [OH]

Therefore, the solution is neutral in nature.

(d) [H3O+] = 1 × 10−8 M; [OH] = 1 × 10−6 M

Here,  [OH] >  [H3O+]

Therefore, the solution is basic in nature.

Step 2 of 3

Chapter 14, Problem 61P is Solved
Step 3 of 3

Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

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Determine if each solution is acidic, basic, or neutral.(a) [H3O+] = 1 × 10?5 M; [OH?] =