×
Log in to StudySoup
Get Full Access to Introductory Chemistry - 5 Edition - Chapter 14 - Problem 100p
Join StudySoup for FREE
Get Full Access to Introductory Chemistry - 5 Edition - Chapter 14 - Problem 100p

Already have an account? Login here
×
Reset your password

For each [OH?], determine the pH and state whether the solution is acidic or basic.(a)

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

Solution for problem 100P Chapter 14

Introductory Chemistry | 5th Edition

  • Textbook Solutions
  • 2901 Step-by-step solutions solved by professors and subject experts
  • Get 24/7 help from StudySoup virtual teaching assistants
Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

4 5 1 432 Reviews
19
0
Problem 100P

For each [OH−], determine the pH and state whether the solution is acidic or basic.

(a) [OH−] = 1.8 × 10−5 M

(b) [OH−] = 8.9 × 10−12 M

(c) [OH−] = 3.1 × 10−2 M

(d) [OH−] = 1.96 × 10−9 M

Step-by-Step Solution:
Step 1 of 3

Solution: Here, we are going to determine the pH of the given solutions.

Step1:

pH is the negative logarithm to base 10 of hydrogen ion concentration whereas pOH is the negative logarithm to base 10 of hydroxyl ion concentration, i.e.,

 pOH =  - log[OH- ] and pH = - log[H+ ]

And pH + pOH =14

We can distinguish acidic, neutral and basic aqueous solutions by the relative values of their pH

                        Acidic: pH < 7

                        Neutral: pH = 7

                        Basic: pH > 7

Step2:

  1. Given, [OH- ] = 1.8 x 10-5 M

Therefore pOH =  - log[OH- ]

                = - log (1.8 x 10-5)

                = - log 1.8 - log 10-5

= -0.255 + 5

= 4.745

Therefore, pH = 14 - pOH

                = 14 - 4.745

                = 9.255

Thus, pH = 9.255

Since, pH > 7, therefore, the solution is basic.

     b)        Given, [OH- ] = 8.9 x 10-12 M

Therefore pOH =  - log[OH- ]

                = - log (8.9 x 10-12)

                = - log 8.9 - log 10-12

= - 0.949 + 12

= 11.051

Therefore, pH = 14 - pOH

                = 14 - 11.051

                = 2.949

Thus, pH = 2.949

Since, pH < 7, therefore, the solution is acidic.

   c)        Given, [OH- ] = 3.1 x 10-2 M

Therefore pOH =  - log[OH- ]

                = - log (3.1 x 10-2)

                = - log 3.1 - log 10-2

= - 0.491 + 2

= 1.509

Therefore, pH = 14 - pOH

                = 14 - 1.509

                = 12.491

Thus, pH = 12.491

Since, pH > 7, therefore, the solution is basic.

    d)        Given, [OH- ] = 1.96 x 10-9 M

Therefore pOH =  - log[OH- ]

                = - log (1.96 x 10-9)

                = - log 1.96 - log 10-9

= -0.292 + 9

= 8.708

Therefore, pH = 14 - pOH

                = 14 - 8.708

                = 5.292

Thus, pH = 5.292

Since, pH < 7, therefore, the solution is acidic.

                                        ----------------------------

Step 2 of 3

Chapter 14, Problem 100P is Solved
Step 3 of 3

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

Other solutions

People also purchased

Related chapters

Unlock Textbook Solution

Enter your email below to unlock your verified solution to:

For each [OH?], determine the pH and state whether the solution is acidic or basic.(a)